Equilibrium: The Extent of Chenmical Reactions

Is K very large or very small for a reaction that goes essentially to completion? Explain.

White phosphorous, ${\mathbf{p}}_{\mathbf{4}}$, is produced by the reduction of phosphate rock, ${\mathbf{Ca}}_{\mathbf{3}}{\left({\mathrm{PO}}_4\right)}_{\mathbf{2}}$.If exposed to oxygen, the waxy, white solid smokes, bursts into flames, and releases a large quantity of heat. Does the reaction ${\mathbf{P}}_{\mathbf{4}}\left(g\right)\mathbf{+}\mathbf{5}{\mathbf{O}}_{\mathbf{2}}\left(g\right)\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{P}}_{\mathbf{4}}{\mathbf{O}}_{\mathbf{10}}\left(S\right)$ have a large or small equilibrium constant? Explain. 

Does Q for the formation of 1 mol of NO from its elements differ from Q for the decomposition of 1 mol of NO to its elements? Explain and give the relationship between the two Q’s.

Does Q for the formation of 1 mol of ${\mathbf{NH}}_{\mathbf{3}}$from ${\mathbf{H}}_{\mathbf{2}}\mathbf{ }{\mathbf{N}}_{\mathbf{2}}$differs from Q for the formation of ${\mathbf{NH}}_{\mathbf{3}}$from ${\mathbf{H}}_{\mathbf{2}}$ and 1 mol of ${\mathbf{N}}_{\mathbf{2}}$? Explain and give the relationship between the two Q’s

Balance each reaction and write its reaction quotient, ${\mathbf{Q}}_{\mathbf{c}}$:

$$\begin{gathered} \mathbf{\left(}\mathbf{a}\mathbf{\right)}\mathbf{ }\mathbf{NO}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }{\mathbf{N}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathbf{ }{\mathbf{SF}}_{\mathbf{6}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{SO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }{\mathbf{SO}}_{\mathbf{2}}{\mathbf{F}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathbf{ }{\mathbf{SCIF}}_{\mathbf{5}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }{\mathbf{S}}_{\mathbf{2}}{\mathbf{F}}_{\mathbf{10}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{HCI}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \end{gathered}$$

Balance each reaction and write its reaction quotient, ${\mathbf{Q}}_{\mathbf{c}}$ :

$$\begin{gathered} \mathbf{\left(}\mathbf{a}\mathbf{\right)}\mathbf{ }\mathbf{ }{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{6}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }{\mathbf{CO}}_{\mathbf{2}}\mathbf{ }\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathbf{ }{\mathbf{CH}}_{\mathbf{4}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{F}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }{\mathbf{CF}}_{\mathbf{4}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{4}\mathbf{HF}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{,}\mathbf{ } \\ \mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathbf{ }{\mathbf{SO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }{\mathbf{SO}}_{\mathbf{2}}\mathbf{\left(}\mathbf{G}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{,}\mathbf{ } \end{gathered}$$

Balance each reaction and write its reaction quotient,${\mathbf{Q}}_{\mathbf{C}}$ :

$$\begin{gathered} \mathbf{\left(}\mathbf{a}\mathbf{\right)}\mathbf{ }{\mathbf{NO}}_{\mathbf{2}}\mathbf{CI}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{NO}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{CI}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathbf{ }{\mathbf{POCI}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }{\mathbf{PCI}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathbf{ }{\mathbf{NH}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }{\mathbf{N}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \end{gathered}$$ 

Explain the difference between a heterogeneous and a homogeneous equilibrium. Give an example of each.

For a given reaction at a given temperature, the value of K is constant. Is the value of Q also constant? Explain.

In a study of formation of HI from its elements, 
${\mathbf{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{I}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{\rightleftharpoons }\mathbf{2}\mathbf{HI}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

Equal amounts of hydrogen and iodine were placed in a container which was then sealed and heated.

(a) On one set of axes, sketch concentration vs. Time curves for hydrogen and hydrogen iodide, and explain how Q changes as a function of time.

(b) Is the value of Q different if [iodine] is plotted instead of [hydrogen]?

In a study of the thermal decomposition of Lithium peroxide, 

$\mathbf{2}{\mathbf{Li}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{\rightleftharpoons }\mathbf{2}{\mathbf{Li}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

A chemist finds that, as long as some Lithium peroxide is present at the end of the experiment, the amount of oxygen obtained in a given container at a given temperature is the same. Explain.

Balance each of the following examples of heterogeneous

equilibria and write its reaction quotient, Qc:

$$\begin{gathered} \mathbf{\left(}\mathbf{a}\mathbf{\right)}\mathbf{ }{\mathbf{Na}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}{\mathbf{CO}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{Na}}_{\mathbf{2}}{\mathbf{CO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathbf{ }{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{I}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathbf{ }{\mathbf{NH}}_{\mathbf{4}}\mathbf{CI}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{NH}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{HCI}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \end{gathered}$$

Balance each of the following examples of heterogeneous()

equilibria and write its reaction quotient, Qc:

$$\begin{gathered} \mathbf{\left(}\mathbf{a}\mathbf{\right)}\mathbf{ }{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{I}\mathbf{\right)}\mathbf{+}{\mathbf{SO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{𝆏}\mathbf{ }{\mathbf{H}}_{\mathbf{2}}{\mathbf{SO}}_{\mathbf{4}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathbf{ }{\mathbf{KNO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{𝆏}\mathbf{ }{\mathbf{KNO}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{ }\mathbf{+}\mathbf{ }{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathbf{ }{\mathbf{S}}_{\mathbf{8}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{ }\mathbf{+}\mathbf{ }{\mathbf{F}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{𝆏}\mathbf{ }\mathbf{ }{\mathbf{SF}}_{\mathbf{6}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ } \end{gathered}$$

Question: Balance each of the following examples of heterogeneous

equilibria and write its reaction quotient, Qc:

$$\begin{gathered} \left(a\right)\mathbf{ }{\mathbf{NaHCO}}_{\mathbf{3}}\mathbf{ }\left(s\right)\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{֏}\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{Na}}_{\mathbf{2}}{\mathbf{CO}}_{\mathbf{3}}\left(s\right)\mathbf{+}{\mathbf{CO}}_{\mathbf{2}}\left(g\right)\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{+}\mathbf{ }{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\left(g\right) \\ \left(b\right)\mathbf{ }{\mathbf{SNO}}_{\mathbf{2}}\left(s\right)\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{+}\mathbf{ }\mathbf{ }{\mathbf{H}}_{\mathbf{2}}\mathbf{ }\left(g\right)\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{֏}\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{Sn}\left(s\right)\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\left(g\right) \\ \left(c\right)\mathbf{ }{\mathbf{H}}_{\mathbf{2}}{\mathbf{SO}}_{\mathbf{4}}\left(I\right)\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{+}\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{SO}}_{\mathbf{3}}\left(g\right)\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{֏}\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{H}}_{\mathbf{2}}{\mathbf{S}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{7}}\left(I\right) \end{gathered}$$

Question: For the following equilibrium system, which of the changes will form more CaCO₃?

${\mathbf{CO}}_{\mathbf{2}}\left(g\right)\mathbf{+}\mathbf{Ca}{\left(\mathrm{OH}\right)}_{\mathbf{2}}\left(s\right)\mathbf{\to }{\mathbf{CaCO}}_{\mathbf{3}}\left(s\right)\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\left(l\right)\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{∆}{\mathbf{H}}^{\mathbf{o}}\mathbf{=}\mathbf{-}\mathbf{113}\mathbf{kJ}$

(a) Decrease temperature at constant pressure (no phase change)

(b) Increase volume at constant temperature

(c) Increase partial pressure of CO₂

(d) Remove one-half of the initial CaCO₃

At ${\mathbf{100}}^{\mathbf{\circ }}\mathbf{C}\mathbf{,}\mathbf{ }{\mathbf{K}}_{\mathbf{p}}\mathbf{=}\mathbf{60}\mathbf{.}\mathbf{6}$for the reaction 

$\mathbf{2}{\mathbf{NOBr}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{\square }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{2}{\mathbf{NO}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{Br}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$

In a given experiment, 0.10 atm of each component is placed in a container. Is the system at equilibrium? If not, in which direction will the reaction proceed?

In the 1980s, CFC-11 was one of the most heavily produced chlorofluorocarbons. The last step in its formation is 

${\mathbf{CCI}}_{\mathbf{4}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{HF}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }}\mathbf{ }\mathbf{ }\mathbf{\square }\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{CFCI}}_{\mathbf{3}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{HCI}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$

If you start the reaction with equal concentrations of ${\mathbf{CCI}}_{\mathbf{4}}$ and HF, you obtain

equal concentrations of ${\mathbf{CFCI}}_{\mathbf{3}}$ and HCl at equilibrium. Are the final

concentrations of ${\mathbf{CFCI}}_{\mathbf{3}}$and HCl equal if you start with unequal 

concentrations of ${\mathbf{CCI}}_{\mathbf{4}}$ and HF? Explain.

For a problem involving the catalysed reaction of methane and 

steam, the following reaction table was prepared:

Explain the entries in the “Change” and “Equilibrium” rows.

Question: Calculate Kc for each of the following equilibria:

$$\begin{gathered} \left(\mathbf{a}\right){\mathbf{H}}_{\mathbf{2}}\left(\mathbf{g}\right)\mathbf{+}{\mathbf{I}}_{\mathbf{2}}\left(\mathbf{g}\right)\rightleftharpoons \mathbf{2}\mathbf{HI}\left(\mathbf{g}\right)\mathbf{;}{\mathbf{K}}_{\mathbf{P}}\mathbf{=}\mathbf{49}\mathbf{at}\mathbf{730}\mathbf{.}\mathbf{K} \\ \left(\mathbf{b}\right)\mathbf{2}{\mathbf{SO}}_{\mathbf{2}}\left(\mathbf{g}\right)\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\left(\mathbf{s}\right)\rightleftharpoons \mathbf{2}{\mathbf{SO}}_{\mathbf{3}}\left(\mathbf{g}\right)\mathbf{;}{\mathbf{K}}_{\mathbf{p}}\mathbf{=}\mathbf{2}\mathbf{.}\mathbf{5}\mathbf{\times }{\mathbf{10}}^{\mathbf{10}}\mathbf{at}\mathbf{500}\mathbf{.}\mathbf{K} \end{gathered}$$

Question: Calculate Kc for each of the following equilibria:

$$\begin{gathered} \left(\mathbf{a}\right)\mathbf{CO}\left(\mathbf{g}\right)\mathbf{+}{\mathbf{Cl}}_{\mathbf{2}}\left(\mathbf{g}\right)\rightleftharpoons {\mathbf{COCl}}_{\mathbf{2}}\left(\mathbf{g}\right)\mathbf{;}{\mathbf{K}}_{\mathbf{P}}\mathbf{=}\mathbf{3}\mathbf{.}\mathbf{9}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{2}}\mathbf{at}\mathbf{1000}\mathbf{.}\mathbf{K} \\ \left(\mathbf{b}\right){\mathbf{S}}_{\mathbf{2}}\left(\mathbf{g}\right)\mathbf{+}\mathbf{C}\left(\mathbf{s}\right)\rightleftharpoons {\mathbf{CS}}_{\mathbf{2}}\left(\mathbf{g}\right)\mathbf{;}{\mathbf{K}}_{\mathbf{p}}\mathbf{=}\mathbf{28}\mathbf{.}\mathbf{5}\mathbf{at}\mathbf{500}\mathbf{.}\mathbf{K} \end{gathered}$$

 At ${\mathbf{425}}^{\mathbf{0}}\mathbf{C}\mathbf{,}{\mathbf{K}}_{\mathbf{p}}\mathbf{=}\mathbf{4}\mathbf{.}\mathbf{18}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{9}}$ for the reaction

$\mathbf{2}{\mathbf{HBr}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{\rightleftharpoons }{\mathbf{H}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{Br}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$

In one experiment, 0.20 atm of HBr(g), 0.010 atm of ${\mathbf{H}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$ , and 0.010 atm of ${\mathbf{Br}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$ are introduced into a container. Is the reaction at equilibrium? If not, in which direction will it proceed?

The water-gas shift reaction plays a central role in the chemical methods for obtaining cleaner fuels from coal: 

${\mathbf{CO}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{\rightleftharpoons }{\mathbf{CO}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{H}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$

At a given temperature, Kp = 2.7. If 0.13 mol of CO, 0.56 mol of ${\mathbf{H}}_{\mathbf{2}}\mathbf{O}$ , 0.62 mol of ${\mathbf{CO}}_{\mathbf{2}}$ , and 0.43 mol of ${\mathbf{H}}_{\mathbf{2}}$ are put in a 2.0-L flask, in which direction, does the reaction proceed?

For a problem involving the catalysed reaction of methane and steam, the following reaction table was prepared:

Explain the entries in the “Change” and “Equilibrium” rows.

(a) What is the basis of the approximation that avoids using the quadratic formula to find an equilibrium concentration?

 (b) When should this approximation not be made?

Gaseous decomposes according to the reaction 

${\mathbf{PCI}}_{\mathbf{5}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{\square }\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{PCI}}_{\mathbf{3}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{CI}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$

In one experiment, 0.15 mol of ${\mathbf{PCI}}_{\mathbf{5}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$ was introduced into a 2.0-L container.

Construct the reaction table for this process.

Hydrogen fluoride, HF, can be made from the reaction 

${\mathbf{H}}_{\mathbf{2}\left(g\right)}\mathbf{+}{\mathbf{F}}_{\mathbf{2}\left(g \right)}\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{\square }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{2}{\mathbf{HF}}_{\left(g\right)}$

In one experiment, 0.10 mol of ${\mathbf{H}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$and 0.050 mol of ${\mathbf{F}}_{\mathbf{2}\left(g\right)}$are added to a 0.50-L f

lask. Write a reaction table for this process.

 A key step in the extraction of iron from its or 

$\mathbf{FeO}\mathbf{ }\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{ }\mathbf{+}\mathbf{CO}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\square }\mathbf{ }\mathbf{Fe}\mathbf{ }\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{ }\mathbf{+}{\mathbf{CO}}_{\mathbf{2}\mathbf{ }}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }{\mathbf{K}}_{\mathbf{P}}\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{403}\mathbf{at}{\mathbf{1000}}^{\mathbf{\circ }}\mathbf{C}$

This step occurs in the ${\mathbf{700}}^{\mathbf{\circ }}$C to ${\mathbf{1200}}^{\mathbf{\circ }}\mathbf{C}$  zone within a blast furnace. What are the equilibrium partial pressures of CO(g) and ${\mathbf{CO}}_{\mathbf{2}}$(g) when 1.00 atm of CO(g) and excess FeO(s) react in a sealed container at ${\mathbf{1000}}^{\mathbf{\circ }}\mathbf{C}$?

Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 

$\mathbf{2}{\mathbf{NH}}_{\mathbf{3}\left(g\right)}\mathbf{ }\mathbf{֏}\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{N}}_{\mathbf{2}\left(g\right)}\mathbf{ }\mathbf{ }\mathbf{+}\mathbf{3}{\mathbf{H}}_{\mathbf{2}\left(g\right)}$

At equilibrium, $\left[{\mathrm{NH}}_3\right]\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{0225}\mathbf{ }\mathbf{M}\mathbf{ }\mathbf{,}\mathbf{ }\mathbf{ }\left[N_2\right]\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{114}\mathbf{ }\mathbf{M}\mathbf{,}\mathbf{ }\mathbf{ }\mathbf{and}\mathbf{ }\left[H_2\right]\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{342}\mathbf{ }\mathbf{M}$. Calculate Kc for the reaction at this temperature.

What does “disturbance” mean in Le Châtelier’s principle?

What is the difference between the equilibrium position and the equilibrium constant of a reaction? Which changes as a result of a change in reactant concentration?

Scenes A, B, and C below depict this reaction at three temperatures:

${\mathbf{NH}}_{\mathbf{4}}\mathbf{CI}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{\rightleftharpoons }{\mathbf{NH}}_{\mathbf{3}}\mathbf{ }\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{HCI}\mathbf{\left(}\mathbf{g}\mathbf{\right)}{\mathbf{\Delta H}}_{\mathbf{rxn}}^{\mathbf{0}}\mathbf{ }\mathbf{=}\mathbf{176}\mathbf{kj}$ 

(a) Which best represents the reaction mixture at the highest temperature? Explain. (b) Which best represents the reaction mixture at the lowest temperature? Explain.

What is implied by the word “constant” in the term equilibrium constant? Give two reaction parameters that can be changed without changing the value of an equilibrium constant.

Le Châtelier's principle is related ultimately to the rates of the forward and reverse steps in a reaction. Explain (a) why an increase in reactant concentration shifts the equilibrium position to the right but does not change K; (b) why a decrease in V shifts the equilibrium position toward fewer moles of gas but does not change K; (c) why a rise in T shifts the equilibrium position of an exothermic reaction toward reactants and also changes K; and (d) why a rise in temperature of an endothermic reaction from ${}^{{\mathbf{T}}_{\mathbf{1}}}$ to ${}^{{\mathbf{T}}_{\mathbf{2}}}$ results in ${}^{{\mathbf{K}}_{\mathbf{2}}}$ being larger than ${}^{{\mathbf{K}}_{\mathbf{1}}}$ .

The "filmstrip" represents five molecular scenes of a gaseous mixture as it reaches equilibrium over time:

X is purple and Y is orange: ${\mathbf{X}}_{\mathbf{2}}\left(g\right)\mathbf{+}{\mathbf{Y}}_{\mathbf{2}}\left(g\right)\mathbf{\to }\mathbf{2}\mathbf{XY}\left(g\right)$.

(a) Write the reaction quotient, Q, for this reaction.

(b) If each particle represents $\mathbf{0}\mathbf{.}\mathbf{1}\mathbf{ }\mathbf{mol}$, find Q for each scene.

(c) If K>1, is time progressing to the right or to the left? Explain.

(d) Calculate K at this temperature.

(e) If $\mathbf{∆}{\mathbf{H}}_{\mathbf{rxn}}^{\mathbf{o}}$, which scene, if any, best represents the mixture at a higher temperature? Explain.

(f) Which scene, if any, best represents the mixture at a higher pressure (lower volume)? Explain.

The powerful chlorinating agent sulfuryl dichloride $\left({\mathrm{SO}}_2{\mathrm{Cl}}_2\right)$ can be prepared by the following two-step sequence:

${\mathbf{H}}_{\mathbf{2}}\mathbf{S}\left(g\right)\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\left(g\right)\mathbf{\to }{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\left(g\right)\mathbf{+}{\mathbf{SO}}_{\mathbf{2}}\left(g\right)$

${\mathbf{SO}}_{\mathbf{2}}\left(g\right)\mathbf{+}{\mathbf{Cl}}_{\mathbf{2}}\left(g\right)\mathbf{\to }{\mathbf{SO}}_{\mathbf{2}}{\mathbf{Cl}}_{\mathbf{2}}\left(g\right)$

1. Balance each step, and write the overall equation.
2. Show that the overall ${\mathbf{Q}}_{\mathbf{c}}$ equals the product of the ${\mathbf{Q}}_{\mathbf{c}}$'s for the individual steps.

The formation of methanol is important to the processing of new fuels. At $\mathbf{298}\mathbf{ }\mathit{K}\mathbf{,}{\mathit{K}}_{\mathbf{P}}\mathbf{=}\mathbf{2}\mathbf{.}\mathbf{25}\mathbf{\times }{\mathbf{10}}^{\mathbf{4}}$ for the reaction

$\mathit{C}\mathit{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{2}{\mathit{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathit{C}{\mathit{H}}_{\mathbf{3}}\mathit{O}\mathit{H}\mathbf{\left(}\mathbf{I}\mathbf{\right)}$

If$\mathbf{∆}{\mathit{H}}_{\mathbf{ran}}\mathbf{=}\mathbf{-}\mathbf{128}\mathbf{ }\mathit{k}\mathit{J}\mathbf{/}\mathit{m}\mathit{o}\mathit{l}\mathit{C}{\mathit{H}}_{\mathbf{3}}\mathit{O}\mathit{H}$, calculate ${\mathit{K}}_{\mathbf{p}}$ at ${\mathbf{0}}^{\mathbf{°}}\mathit{C}$.

Predict the effect of increasing the temperature on the amounts of products in the following reactions:

(a) ${\mathbf{\text{CO(g)+2H}}}_{\mathbf{\text{2}}}\mathbf{\text{(g)}}\mathbf{\rightleftharpoons }{\mathbf{\text{CH}}}_{\mathbf{\text{3}}}{\mathbf{\text{OH(g)\hspace{1em}ΔH}}}_{\mathbf{\text{rxn}}}^{\mathbf{\text{°}}}\mathbf{\text{=-90.7 kJ}}$ 

(b) ${\mathbf{\text{C(s)+H}}}_{\mathbf{\text{2}}}\mathbf{\text{O(g)}}\mathbf{\rightleftharpoons }{\mathbf{\text{CO(g)+H}}}_{\mathbf{\text{2}}}{\mathbf{\text{(g)\hspace{1em}ΔH}}}_{\mathbf{\text{ran}}}^{\mathbf{\text{°}}}\mathbf{\text{=131 kJ}}$

(c) $\mathbf{2}\mathit{N}{\mathit{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathbf{2}\mathit{N}\mathit{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathit{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$ (endothermic)

(d) $\mathbf{2}\mathbf{C}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{2}\mathbf{CO}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$ (exothermic)

How would you adjust the volume of the container in order to maximize product yield in each of the following reactions?

(a) $\mathit{F}{\mathit{r}}_{\mathbf{3}}{\mathit{O}}_{\mathbf{4}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}\mathbf{4}{\mathit{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{3}\mathit{F}\mathit{e}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}\mathbf{4}{\mathit{H}}_{\mathbf{2}}\mathit{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$ 

(b) $\mathbf{2}\mathbf{C}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}{\mathbf{0}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{2}\mathbf{CO}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

Predict the effect of decreasing the container volume on the amounts of each reactant and product in the following reactions:

(a) ${\mathit{C}}_{\mathbf{3}}{\mathit{H}}_{\mathbf{8}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{50}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathbf{3}\mathit{C}{\mathit{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{4}{\mathit{H}}_{\mathbf{2}}\mathit{O}\mathbf{\left(}\mathbf{I}\mathbf{\right)}$ 

(b) $\mathbf{4}\mathit{N}{\mathit{H}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{3}{\mathit{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathbf{2}\mathbf{ }{\mathit{N}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{6}{\mathit{H}}_{\mathbf{2}}\mathit{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

Predict the effect of decreasing the container volume on the amounts of each reactant and product in the following reactions:

(a) ${\mathbf{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{Cl}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{2}\mathbf{HCl}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$
 

(b) $\mathbf{2}{\mathbf{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{2}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{I}\mathbf{\right)}$

Predict the effect of increasing the container volume on the amounts of each reactant and product in the following reactions:

(a) $\mathit{C}{\mathit{H}}_{\mathbf{3}}\mathit{O}\mathit{H}\mathbf{\left(}\mathbf{I}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathit{C}{\mathit{H}}_{\mathbf{3}}\mathit{O}\mathit{H}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$ 

(b) $\mathit{C}{\mathit{H}}_{\mathbf{4}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathit{N}{\mathit{H}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathit{H}\mathit{C}\mathit{N}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{3}{\mathit{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

Predict the effect of increasing the container volume on the amounts of each reactant and product in the following reactions:

(a) ${\mathbf{F}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathbf{2}\mathbf{ }\mathbf{F}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

(b) $\mathbf{2}\mathit{C}{\mathit{H}}_{\mathbf{4}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathbf{ }{\mathit{C}}_{\mathbf{2}}{\mathit{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{3}{\mathit{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

Sodium bicarbonate undergoes thermal decomposition according to the reaction

$\mathbf{2}\mathit{N}\mathit{a}\mathit{H}\mathit{C}{\mathit{O}}_{\mathbf{3}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{ }\mathbf{ }\mathit{N}{\mathit{a}}_{\mathbf{2}}\mathit{C}{\mathit{O}}_{\mathbf{3}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}\mathit{C}{\mathit{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathit{H}}_{\mathbf{2}}\mathit{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$

How does the equilibrium position shift as a result of each of the following disturbances? (a) $\mathbf{0}\mathbf{.}\mathbf{20}\mathbf{ }\mathit{a}\mathit{t}\mathit{m}$of argon gas is added. 

(b) $\mathit{N}\mathit{a}\mathit{H}\mathit{C}{\mathit{O}}_{\mathbf{3}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}$is added.

(c) $\mathit{M}\mathit{g}{\left(CI{O}_4\right)}_{\mathbf{2}}\left(s\right)$ is added as a drying agent to remove ${\mathit{H}}_{\mathbf{2}}\mathit{O}$.

(d) Dry ice is added at constant T.

Consider this equilibrium system:

${\mathbf{\text{CO(g)+Fe}}}_{\mathbf{\text{3}}}{\mathbf{\text{O}}}_{\mathbf{\text{4}}}\mathbf{\text{(s)}}\mathbf{\rightleftharpoons }{\mathbf{\text{CO}}}_{\mathbf{\text{2}}}\mathbf{\text{(g)+3FeO(s)}}$

How does the equilibrium position shift as a result of each of the following disturbances? (a) $\mathit{C}\mathit{O}$is added.

(b) $\mathit{C}{\mathit{O}}_{\mathbf{2}}$ is removed by adding solid $\mathit{N}\mathit{a}\mathit{O}\mathit{H}$.

(c) Additional $\mathit{F}{\mathit{e}}_{\mathbf{3}}{\mathit{O}}_{\mathbf{4}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}$ is added to the system.

(d) Dry ice is added at constant temperature.

An equilibrium mixture of two solids and a gas, in the reaction$\mathbf{\text{XY(s)}}\mathbf{\rightleftharpoons }\mathbf{\text{X(g)+Y(s)}}$, is depicted at right (X is green and Y is black). Does scene A, B, or C best represent the system at equilibrium after two formula units of Y(s) is added? Explain.

Predict the effect of decreasing the temperature on the amounts of reactants in the following reactions:

(a) ${\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{2}}\left(g\right)\mathbf{ }\mathbf{+}\mathbf{ }{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{ }\left(g\right)\mathbf{ }\mathbf{\rightleftharpoons }{\mathbf{CH}}_{\mathbf{3}}\mathbf{ }\mathbf{CHO}\mathbf{ }\left(g\right)\mathbf{ }\mathbf{ }{\mathbf{\Delta H}}_{\mathbf{rxn}}^{\mathbf{0}}\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{=}\mathbf{-}\mathbf{151}\mathbf{kj}$ 

(b) ${\mathbf{CH}}_{\mathbf{3}}{\mathbf{CH}}_{\mathbf{2}}\mathbf{OH}\left(I\right)\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{ }\left(g\right)\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }{\mathbf{CH}}_{\mathbf{3}}{\mathbf{CO}}_{\mathbf{2}}\mathbf{H}\left(I\right)\mathbf{+}{\mathbf{HO}}_{\mathbf{2}}\mathbf{ }\left(g\right)\mathbf{ }\mathbf{ }{\mathbf{\Delta H}}_{\mathbf{rxn}}^{\mathbf{0}}\mathbf{ }\mathbf{=}\mathbf{-}\mathbf{451}\mathbf{kj}$

The molecule ${}^{{\mathbf{D}}_{\mathbf{2}}}$ (where D, deuterium, is ${}^{{}^{\mathbf{2}}\mathbf{H}}$) undergoes a reaction with ordinary ${}^{{\mathbf{H}}_{\mathbf{2}}}$ that leads to isotopic equilibrium: ${}^{{\mathbf{D}}_{\mathbf{2}}\mathbf{ }\left(g\right)\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{ }\left(g\right)\mathbf{ }\mathbf{\rightleftharpoons }\mathbf{ }\mathbf{2}\mathbf{DH}\mathbf{ }\left(g\right)\mathbf{ }\mathbf{ }\mathbf{ }{\mathbf{K}}_{\mathbf{P}}\mathbf{ }\mathbf{=}\mathbf{1}\mathbf{.}\mathbf{80}}$ If ${}^{\mathbf{∆}{\mathbf{H}}_{\mathbf{rxn}}^{\mathbf{0}}}$ is 0.32 kJ/mol DH, calculate ${}^{{\mathbf{K}}_{\mathbf{P}}}$ at 500. K.

The minerals hematite ${}^{\left({\mathrm{Fe}}_2{O}_3\right)}$ and magnetite ${}^{\left({\mathrm{Fe}}_3{O}_4\right)}$ exist in equilibrium with atmospheric oxygen: ${}^{{\mathrm{Fe}}_3{O}_{4 }\left(s\right) +O_2 \left(g\right) \rightleftharpoons {\mathrm{Fe}}_6{O}_{3 }\left(s\right) K_P=2.5\times {10}^{87}}$ (a) Determine ${}^{{\mathbf{P}}_{{\mathbf{O}}_{\mathbf{2}}}}$ at equilibrium. (b) Given that ${}^{{\mathbf{P}}_{{\mathbf{O}}_{\mathbf{2}}}}$ in air is 0.21 atm, in which direction will the reaction proceed to reach equilibrium? (c) Calculate ${}^{{\mathbf{K}}_{\mathbf{C}}}$ at 298 K.

The oxidation of ${}^{{\mathbf{SO}}_{\mathbf{2}}}$ is the key step in ${}^{{\mathbf{H}}_{\mathbf{2}}{\mathbf{SO}}_4}$ production:  ${}^{{\mathbf{SO}}_{\mathbf{2}}\mathbf{ }\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{+}\frac{\mathbf{1}}{\mathbf{2}}{\mathbf{O}}_{\mathbf{2}}\mathbf{ }\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }\mathbf{\rightleftharpoons }{\mathbf{SO}}_{\mathbf{3}}\mathbf{ }\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{ }{\mathbf{\Delta H}}_{\mathbf{rxn}}^{\mathbf{0}}\mathbf{ }\mathbf{=}\mathbf{-}\mathbf{99}\mathbf{.}\mathbf{2}\mathbf{ }\mathbf{kj}}$ (a) What qualitative combination of T and P maximizes ${}^{{\mathbf{SO}}_{\mathbf{3}}}$ yield? (b) How does addition of  affect Q? K? (c) Why is catalysis used for this reaction?

An industrial chemist introduces $\mathbf{2}\mathbf{.}\mathbf{0}\mathbf{ }\mathbf{atm}$ of ${\mathbf{H}}_{\mathbf{2}}$ and $\mathbf{2}\mathbf{.}\mathbf{0}\mathbf{ }\mathbf{atm}$ of  into a $\mathbf{1}\mathbf{.}\mathbf{00}\mathbf{-}\mathbf{L}$ container at $\mathbf{25}\mathbf{.}{\mathbf{0}}^{\mathbf{°}}\mathbf{C}$ and then raises the temperature to ${\mathbf{700}}^{\mathbf{°}}\mathbf{C}$, at which : ${\mathbf{K}}_{\mathbf{c}}\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{534}$

${\mathbf{H}}_{\mathbf{2}}\left(g\right)\mathbf{+}{\mathbf{CO}}_{\mathbf{2}}\left(g\right)\mathbf{\to }{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\left(g\right)\mathbf{+}\mathbf{CO}\left(g\right)$

How many grams of ${\mathbf{H}}_{\mathbf{2}}$ are present at equilibrium?