Chemical Quantities and Reactions

When linoleic acid, an unsaturated fatty acid, reacts with hydrogen, it forms a saturated fatty acid. Is linoleic acid oxidized or reduced in the hydrogenation reaction? 

 ${\mathrm{C}}_{18}{\mathrm{H}}_{32}{\mathrm{O}}_2 + 2{\mathrm{H}}_2 \to {\mathrm{C}}_{18}{\mathrm{H}}_{36}{\mathrm{O}}_2$ 

Linoleic acid

In one of the reactions in the citric acid cycle, which provides energy, succinic acid is converted to fumaric acid. 

$C_4{H}_6{O}_4 \to C_4{H}_4{O}_4 + 2H$

Succinic acid    Fumaric acid 

The reaction is accompanied by a coenzyme, flavin adenine dinucleotide 

$\mathrm{FAD} + 2\mathrm{H} \to {\mathrm{FADH}}_2$

a. Is succinic acid oxidized or reduced? 

b. Is FAD oxidized or reduced? 

c. Why would the two reactions occur together?

In each of the following, identify the reactant that is oxidized and the reactant that is reduced: 

a)$2\mathrm{Li}\left(\mathrm{s}\right) + {\mathrm{F}}_2\left(\mathrm{g}\right) \to 2\mathrm{LiF}\left(\mathrm{s}\right)$ 

b)${\mathrm{Cl}}_2\left(\mathrm{g}\right) + 2\mathrm{KI}\left(\mathrm{aq}\right) \to \mathrm{I}\left(\mathrm{s}\right) + 2\mathrm{KCl}\left(\mathrm{aq}\right)$ 

c)$2\mathrm{Al}\left(\mathrm{s}\right) + 3{\mathrm{Sn}}^{2+}\left(\mathrm{aq}\right) \to 3\mathrm{Sn}\left(\mathrm{s}\right) + 2{\mathrm{Al}}^{3+}\left(\mathrm{aq}\right)$ 

d)$\mathrm{Fe}\left(\mathrm{s}\right) + {\mathrm{CuSO}}_4\left(\mathrm{aq}\right) \to \mathrm{Cu}\left(\mathrm{s}\right) + {\mathrm{FeSO}}_4\left(\mathrm{aq}\right)$ 

Write all of the mole-mole factors for each of the following chemical equations: 

a.$2S{O}_2\left(g\right)+O_2\left(g\right)\to 2S{O}_3\left(g\right)$

b.data-custom-editor="chemistry" $4P\left(s\right)+5{\mathrm{O}}_2\left(g\right)\to 2P_{\mathit{2}}{O}_{\mathit{5}}\left(s\right)$

Write all of the mole-mole factors for each of the following chemical equations:

a. $2\mathrm{Al}\left(\mathrm{s}\right) + 3{\mathrm{Cl}}_2\left(\mathrm{g}\right) \to 2{\mathrm{AICI}}_3\left(\mathrm{s}\right)$

b.$4\mathrm{HCI}\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right)\to 2{\mathrm{Cl}}_2\left(\mathrm{g}\right) + 2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

The chemical reaction of hydrogen with oxygen produces water. 

$2H_2\left(g\right) + O_2\left(g\right) \to 2H_{2}O\left(g\right)$

a. How many moles of ${\mathrm{O}}_2$are required to react with $2.6$ moles of H?

b. How many moles of ${\mathrm{H}}_2$are needed to react with $5.0$ moles of${\mathrm{O}}_2$?

c. How many moles of ${\mathrm{H}}_2\mathrm{O}$form when $2.5$ moles of ${\mathrm{O}}_2$react?

Carbon disulfide and carbon monoxide are produced when carbon is heated with sulfur dioxide.

a. How many moles of $C$ are needed to react with $0.500 mole$ of $S{O}_2$?

b. How many moles of $CO$ are produced when $1.2$moles of $C$ reacts?

c. How many moles of $S{O}_2$ are needed to produce $0.50$mole of $C{S}_2$?

d. How many moles of $C{S}_2$ are produced when $2.5$moles of $C$ reacts?

Nitrogen gas reacts with hydrogen gas to produce ammonia.

$N_2$(g) + $3H_2$(g) $\to$$2N{H}_3$(g)

(a) If you have $3.64$ g of H, how many grams of $N{H}_3$ can be

produced? 

(b) How many grams of H, are needed to react with $2.80$ g

of N? 

(c) How many grams of $N{H}_3$ can be produced from $12.0$ g

of H?

Ammonia and oxygen react to form nitrogen and water.

$4N{H}_3\left(g\right)+3O_2\left(g\right)\to 2N_2\left(g\right)+6H_{2}O\left(g\right)$

a. How many grams of $O_2$ are needed to react with$13.6 \mathrm{g}$ of $N{H}_3?$

b. How many grams of $N_2$ can be produced when$6.50 \mathrm{g}$ of $O_2$ reacts?

c. How many grams of $H_{2}O$ are formed from the reaction of $34.0 \mathrm{g}$ of $N{H}_3?$

Iron(III) oxide reacts with carbon to give iron and carbon monoxide.

$F{e}_2{O}_3\left(s\right)+3C\left(s\right)\to 2Fe\left(s\right)+3CO\left(g\right)$

a. How many grams of $C$ are required to react with $16.5 \mathrm{g}$ of $F{e}_2{O}_3?$

b. How many grams of $CO$ are produced when$36.0 \mathrm{g}$ of $C$reacts ?

c. How many grams of Fe can be produced when $6.00 \mathrm{g}$of $F{e}_2{O}_3$ reacts?

Sodium reacts with oxygen to produce sodium oxide.

a. How many grams of $N{a}_{2}O$ are produced when $57.5g$ of $Na$ reacts?

b. If you have $18.0g$ of $Na$, how many grams of $O_2$ are needed for the reaction?

c. How many grams of $O_2$ are needed in a reaction that produces $75.0g$ of $N{a}_{2}O$?

When the gases dihydrogen sulfide and oxygen react, they form the gases sulfur dioxide and water vapor.

a. Write the balanced chemical equation for the reaction.

b. How many grams of oxygen are needed to react with $2.50 \mathrm{g}$ of dihydrogen sulfide?

c. How many grams of sulfur dioxide can be produced when $38.5 \mathrm{g}$ of oxygen reacts?

d. How many grams of oxygen are needed to produce$55.8 \mathrm{g}$ of water vapor?

When solid lead(II) sulfide reacts with oxygen gas, the products are solid lead(II) oxide and sulfur dioxide gas.

a. Write the balanced chemical equation for the reaction.

b. How many grams of oxygen are required to react with $29.9 \mathrm{g}$of lead(II) sulfide?

c. How many grams of sulfur dioxide can be produced when $65.0 \mathrm{g}$of lead(II) sulfide reacts?

d. How many grams of lead(II) sulfide are used to produce$128 \mathrm{g}$ of lead(II) oxide?

Nitrogen dioxide and water react to produce nitric acid, $HN{O}_3$ and nitrogen oxide.

$3N{O}_2\left(g\right)+H_{2}O\left(l\right)\to 2HN{O}_3\left(aq\right)+NO\left(g\right)$

a. How many grams of $H_{2}O$ are needed to react with $28.0 \mathrm{g}$ of  $N{O}_2$ ?

b. How many grams of $NO$ are produced from $15.8 \mathrm{g}$of  $H_{2}O$ ?

c. How many grams of $HN{O}_3$are produced from$8.25 \mathrm{g}$ of $N{O}_2$ ?

Calcium cyanamide, $CaC{N}_2$ reacts with water to form calcium carbonate and ammonia.

$CaC{N}_2\left(s\right)+3H_{2}O\left(l\right)\to CaC{O}_3\left(s\right)+2N{H}_3\left(g\right)$

a. How many grams of $H_{2}O$ are needed to react with $75.0 \mathrm{g}$of $CaC{N}_2?$

b. How many grams of$N{H}_3$ are produced from $5.24 \mathrm{g}$ of $CaC{N}_2?$

c. How many grams of $CaC{O}_3$ form if  $155 \mathrm{g}$ of $H_{2}O$ reacts?

Classify each of the following as exothermic or endothermic:

a. The energy level of the products is lower than that of the reactants.

b. In the body, the synthesis of proteins requires energy.

c. A reaction absorbs $125 \mathrm{kJ}.$

Classify each of the following as exothermic or endothermic:

a. A reaction releases $550 \mathrm{kJ}.$

b. The energy level of the products is higher than that of the reactants.

c. The metabolism of glucose in the body provides energy.

a. What is measured by the heat of reaction?

b. In an endothermic reaction, is the energy of the products higher or lower than that of the reactants?

c. Draw an energy diagram for an endothermic reaction.

a. Why do chemical reactions require energy of activation ?

b. In an exothermic reaction, is the energy of the products higher or lower than that of the reactants?

c. Draw an energy diagram for an exothermic reaction.

Classify each of the following as exothermic or endothermic:

a. ${\mathrm{CH}}_4 \left(\mathrm{g}\right) + 2{\mathrm{O}}_2 \left(\mathrm{g}\right)\stackrel{∆}{\to }{\mathrm{CO}}_2 \left(\mathrm{g}\right) + 2{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right) + 802 \mathrm{kJ}$

b. $\mathrm{Ca}{\left(\mathrm{OH}\right)}_2 \left(\mathrm{s}\right) + 65.3 \mathrm{kJ} \to \mathrm{CaO} \left(\mathrm{s}\right) + {\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$

c. $2\mathrm{Al} \left(\mathrm{s}\right) + {\mathrm{Fe}}_2{\mathrm{O}}_3 \left(\mathrm{s}\right) \to {\mathrm{Al}}_2{\mathrm{O}}_3 \left(\mathrm{s}\right) + 2\mathrm{Fe} \left(\mathrm{s}\right) + 850 \mathrm{kJ}$

Classify each of the following as exothermic or endothermic: 

a. ${\mathrm{C}}_3{\mathrm{H}}_8 \left(\mathrm{g}\right) + 5{\mathrm{O}}_2 \left(\mathrm{g}\right)\stackrel{∆}{\to } 3{\mathrm{CO}}_2 \left(\mathrm{g}\right) + 4{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right) + 2220 \mathrm{kJ}$

b. $2 \mathrm{Na} \left(\mathrm{s}\right) +{\mathrm{Cl}}_2 \left(\mathrm{g}\right)\to 2 \mathrm{NaCl} \left(\mathrm{s}\right) + 819 \mathrm{kJ}$

c. ${\mathrm{PCl}}_5 \left(\mathrm{g}\right) + 67 \mathrm{kJ} \to {\mathrm{PCl}}_3 \left(\mathrm{g}\right) + {\mathrm{Cl}}_2 \left(\mathrm{g}\right)$

a. What is meant by the rate of a reaction?

b. Why does bread grow mold more quickly at room temperature than in the refrigerator?

a. How does a catalyst affect the activation energy?

b. Why is pure oxygen used in respiratory distress?

How would each of the following change the rate of the reaction shown here?

$2{\mathrm{SO}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \to 2{\mathrm{SO}}_3\left(\mathrm{g}\right)$

a. adding some ${\mathrm{SO}}_2\left(\mathrm{g}\right)$

b. increasing the temperature

c. adding a catalyst

d. removing some ${\mathrm{O}}_2\left(\mathrm{g}\right)$

How would each of the following change the rate of the reaction shown here:

$2NO\left(g\right) + 2H_2\left(g\right) \to N_2\left(g\right) + 2H_{2}0\left(g\right)$

a. adding some $NO\left(g\right)$

b. decreasing the temperature

c. removing some $H_2\left(g\right)$

d. adding a catalyst

a. During cellular respiration, aqueous $C_6{H}_{12}{O}_6$ (glucose) in the cells undergoes a reaction with oxygen gas to form gaseous carbon dioxide and liquid water. Write and balance the chemical equation for reaction of glucose in the human body.

b. In plants, carbon dioxide gas and liquid water are converted to aqueous glucose $C_6{H}_{12}{O}_6$and oxygen gas. Write and balance the chemical equation for production of glucose in plants.

Fatty acids undergo reaction with oxygen gas and form gaseous carbon dioxide and liquid water when utilized for energy in the body.

(a)Write and balance the equation for the combustion of the fatty acid aqueous capric acid $C_{10}{H}_{20}{O}_2$

(b)   Write and balance the equation for the combustion of the fatty acid aqueous myristic acid, $C_{14}{H}_{28}{0}_2$

Using the models of the molecules (black = C, white = H, yellow = S, red = O), determine each of the following for models of compounds $1 and 2$:

(a). Molecular formula.

(b). Molar mass.

(c). No. of moles in $10 g$.

Using the models of the molecules (black = C, white = H, yellow = S, green = Cl), determine each of the following for compounds $1$and $2$:

(a) Molecular formula.

(b) Molecular mass.

(c) No of moles in$10 g$ .

A dandruff shampoo contains dipyrithione,${\mathrm{C}}_{10}{\mathrm{H}}_8{\mathrm{N}}_2{\mathrm{O}}_2{\mathrm{S}}_2$ , which acts as an antibacterial and antifungal agent. 

1. What is the molar mass of dipyrithione?
2. How many moles of dipyrithione are in $25.0 g$?

3. How many moles of $C$ are in $25.0 g$of dipyrithione?

4. How many moles of dipyrithione contain $8.2 \times {10}^{24}$atoms of $N$?

Ibuprofen, an anti-inflammatory drug in Advil, has the formula . $C_{13}{H}_{18}{0}_2$

Ibuprofen is an anti inflammatory.

1. What is the molar mass of ibuprofen?
2. How many grams of ibuprofen are in $0.525$ mole?
3. How many moles of $C$ are in $12$g of ibuprofen?
4. How many moles of ibuprofen contain $1.22 x {10}^{23}$ atoms of $C$?

Balance each of the following by adding coefficients, and identify the type of reaction for each

If red spheres represent oxygen atoms, blue spheres represent nitrogen atoms, and all the Molecules are gases, 

1. Write the formula for each of the reactants and products.
2. Write a balanced equation for the reaction.
3. Indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

If green sphere represents the chlorine atoms and red sphere represents the oxygen atoms and all are gases.

1. Write the formula for each of the reactants and products.     
2. Write the balanced equation.
3. Indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

If purple spheres represent iodine atoms, white spheres represent hydrogen atoms, and all the molecules are gases

(a) Write the formula for each of the reactants and products.

(b) Write a balanced equation for the reaction.

(c) Indicate the type of reaction as combination, decomposition, single replacement, double replacement.

If blue spheres represent nitrogen atoms, purple spheres represent iodine atoms and the reacting molecules are solid, while the products are gases.

1. Write the formula for each of the reactants and products.
2. Write a balanced equation for the reaction.
3. Indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

If green spheres represent chlorine atoms, yellow-green spheres represent fluorine atoms, white spheres represent hydrogen atoms, and all the molecules are gases.

1. Write the formula for each of the reactants and products.
2. Write a balanced equation for the reaction.
3. Indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

If purple sphere represents the Iodine atoms and blue sphere represents the nitrogen atoms and reacting molecules are gases and products are solid.

1. Write the formula for each of the reactants and products.     
2. Write the balanced equation.
3. Indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

Calculate the molar mass for each of the following: ($7.2$)

a. data-custom-editor="chemistry" ${\mathrm{ZnSO}}_4$, zinc sulfate, zinc supplement

b. data-custom-editor="chemistry" $\mathrm{Ca}{\left({\mathrm{IO}}_3\right)}_2$, calcium iodate, iodine source in table salt

c. data-custom-editor="chemistry" ${\mathrm{C}}_5{\mathrm{H}}_8{\mathrm{NNaO}}_4$,monosodium glutamate, flavor enhancer

d. data-custom-editor="chemistry" ${\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_2$,isoamyl formate, used to make artificial fruit syrups

Calculate the molar mass for each of the following: ($7.2$)

a. data-custom-editor="chemistry" ${\mathrm{MgCO}}_3$, magnesium carbonate, used in antacids

b. data-custom-editor="chemistry" $\mathrm{Au}{\left(\mathrm{OH}\right)}_3$, gold(III) hydroxide, used in gold plating

c. data-custom-editor="chemistry" ${\mathrm{C}}_{18}{\mathrm{H}}_{34}{\mathrm{O}}_2$, oleic acid, from olive oil

d. data-custom-editor="chemistry" ${\mathrm{C}}_{21}{\mathrm{H}}_{26}{\mathrm{O}}_5$, prednisone, anti-inflammatory

How many grams are in $0.150$ mole of each of the following? ($7.3$)

a. $\mathrm{K}$

b. ${\mathrm{Cl}}_2$

c. $N{a}_{2}C{O}_3$

How many grams are in $2.25$ mole of each of the following? ($7.3$)

a. ${\mathrm{N}}_2$

b. $\mathrm{NaBr}$

c. ${\mathrm{C}}_6{\mathrm{H}}_{14}$

How many moles are in $25.0$ g of each of the following compounds? ($7.3$)

a. ${\mathrm{CO}}_2$

b. ${\mathrm{Al}}_2{\mathrm{O}}_3$

c. ${\mathrm{MgCl}}_2$

How many moles are in $4.00$ g of each of the following compounds? ($7.3$)

a. ${\mathrm{NH}}_3$

b. $\mathrm{Ca}{\left({\mathrm{NO}}_3\right)}_2$

c. ${\mathrm{SO}}_3$

Identify the type of reaction for each of the following as combination, decomposition, single replacement, double replacement, or combustion: ($7.5$)

a. A metal and a nonmetal form an ionic compound.

b. A compound of hydrogen and carbon reacts with oxygen to produce carbon dioxide and water. 

c. Heating calcium carbonate produces calcium oxide and carbon dioxide. 

d. Zinc replaces copper in data-custom-editor="chemistry" $\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2$.

Identify the type of reaction for each of the following as combination, decomposition, single replacement, double replacement, or combustion: ($7.5$)

a. A compound breaks apart into its elements. 

b. Copper and bromine form copper($II$) bromide.

c. Iron($II$) sulfite breaks down to iron($II$) oxide and sulfur dioxide.

d. Silver ion from data-custom-editor="chemistry" ${\mathrm{AgNO}}_3$(aq.) forms a solid with bromide ion from data-custom-editor="chemistry" $\mathrm{KBr}$(aq).

Balance each of the following chemical equations, and identify the type of reaction: ($7.4, 7.5$)

a. data-custom-editor="chemistry" ${\mathrm{NH}}_3\left(\mathrm{g}\right) + \mathrm{HCl}\left(\mathrm{g}\right) \to {\mathrm{NH}}_4\mathrm{Cl}\left(\mathrm{s}\right)$ 

b.  ${\mathrm{C}}_4{\mathrm{H}}_8\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \stackrel{∆}{\to }{\mathrm{CO}}_2\left(\mathrm{g}\right) + {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

c. data-custom-editor="chemistry" $\mathrm{Sb}\left(\mathrm{s}\right) + {\mathrm{Cl}}_2\left(\mathrm{g}\right) \to {\mathrm{SbCl}}_3\left(\mathrm{s}\right)$

d. data-custom-editor="chemistry" ${\mathrm{NI}}_3\left(\mathrm{s}\right)\to {\mathrm{N}}_2\left(\mathrm{g}\right) + {\mathrm{I}}_2\left(\mathrm{g}\right)$ 

e. data-custom-editor="chemistry" $\mathrm{KBr}\left(\mathrm{aq}\right) + {\mathrm{Cl}}_2\left(\mathrm{aq}\right) \to \mathrm{KCl}\left(\mathrm{aq}\right) + {\mathrm{Br}}_2\left(\mathrm{l}\right)$

f. data-custom-editor="chemistry" $\mathrm{Fe}\left(\mathrm{s}\right) + {\mathrm{H}}_2{\mathrm{SO}}_4\left(\mathrm{aq}\right) \to {\mathrm{H}}_2\left(\mathrm{g}\right) + {\mathrm{Fe}}_2{\left({\mathrm{SO}}_4\right)}_3\left(\mathrm{aq}\right)$

g. data-custom-editor="chemistry" ${\mathrm{Al}}_2{\left({\mathrm{SO}}_4\right)}_3\left(\mathrm{aq}\right) + \mathrm{NaOH}\left(\mathrm{aq}\right) \to \mathrm{Al}{\left(\mathrm{OH}\right)}_3\left(\mathrm{s}\right) + {\mathrm{Na}}_2{\mathrm{SO}}_4\left(\mathrm{aq}\right)$

Balance each of the following chemical equations, and identify the type of reaction: ($7.4, 7.5$) 

a. ${\mathrm{Si}}_3{\mathrm{N}}_4\left(\mathrm{s}\right) \to \mathrm{Si}\left(\mathrm{s}\right) + {\mathrm{N}}_2\left(\mathrm{g}\right)$

b. $\mathrm{Mg}\left(\mathrm{s}\right) + {\mathrm{N}}_2\left(\mathrm{g}\right) \to {\mathrm{Mg}}_3{\mathrm{N}}_2\left(\mathrm{s}\right)$

c. $\mathrm{Al}\left(\mathrm{s}\right) + {\mathrm{H}}_2{\mathrm{PO}}_4\left(\mathrm{aq}\right) \to {\mathrm{H}}_2\left(\mathrm{g}\right) + {\mathrm{AIPO}}_4\left(\mathrm{aq}\right)$

d. ${\mathrm{C}}_3{\mathrm{H}}_4\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right) + {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

e. ${\mathrm{Cr}}_2{\mathrm{O}}_3\left(\mathrm{s}\right) + {\mathrm{H}}_2\left(\mathrm{g}\right)\to \mathrm{Cr}\left(\mathrm{s}\right) + {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

f. $\mathrm{Al}\left(\mathrm{s}\right) + {\mathrm{Cl}}_2\left(\mathrm{g}\right)\to {\mathrm{AlCl}}_3\left(\mathrm{s}\right)$

g. ${\mathrm{MgCl}}_2\left(\mathrm{aq}\right) + {\mathrm{AgNO}}_3\left(\mathrm{aq}\right) \to \mathrm{AgCl}\left(\mathrm{s}\right) + \mathrm{Mg}{\left({\mathrm{NO}}_3\right)}_2\left(\mathrm{aq}\right)$

Identify each of the following as an oxidation or a reduction: ($7.6$)

a. ${\mathrm{Zn}}^{2+}(\mathrm{aq}.)+2{\mathrm{e}}^{-}\to \mathrm{Zn}\left(\mathrm{s}\right)$

b. $\mathrm{Al}\left(\mathrm{s}\right)\to {\mathrm{Al}}^{3+}\left(\mathrm{aq}\right)+3{\mathrm{e}}^{-}$-

c. $\mathrm{Pb}\left(\mathrm{s}\right)\to {\mathrm{Pb}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}$

d. ${\mathrm{Cl}}_2\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}\to 2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)$