Chapter 12

You have a sample of helium gas at \(-33^{\circ} \mathrm{C},\) and you want to increase the average speed of helium atoms by \(10.0 \% .\) To what temperature should the gas be heated to accomplish this?

If \(12.0 \mathrm{g}\) of \(\mathrm{O}_{2}\) is required to inflate a balloon to a certain size at \(27^{\circ} \mathrm{C},\) what mass of \(\mathrm{O}_{2}\) is required to inflate it to the same size (and pressure) at \(5.0^{\circ} \mathrm{C} ?\)

You have two gas-filled balloons, one containing He and the other containing \(\mathrm{H}_{2} .\) The \(\mathrm{H}_{2}\) balloon is twice the size of the He balloon. The pressure of gas in the \(\mathrm{H}_{2}\) balloon is 1 atm, and that in the He balloon is 2 atm. The \(\mathrm{H}_{2}\) balloon is outside in the snow \(\left(-5^{\circ} \mathrm{C}\right),\) and the He balloon is inside a warm building \(\left(23^{\circ} \mathrm{C}\right)\) (a) Which balloon contains the greater number of molecules? (b) Which balloon contains the greater mass of gas?

A bicycle tire has an internal volume of \(1.52 \mathrm{I}\). and contains 0.406 mol of air. The tire will burst if its internal pressure reaches 7.25 atm. To what temperature, in degrees Celsius, does the air in the tire need to be heated to cause a blowout?

The temperature of the atmosphere on Mars can be as high as \(27^{\circ} \mathrm{C}\) at the equator at noon, and the atmospheric pressure is about \(8 \mathrm{mm}\) Hg. If a spacecraft could collect 10\. \(\mathrm{m}^{3}\) of this atmosphere, compress it to a small volume, and send it back to Earth, how many moles would the sample contain?

If you place \(2.25 \mathrm{g}\) of solid silicon in a \(6.56-\mathrm{L}\). flask that contains \(\mathrm{CH}_{3} \mathrm{Cl}\) with a pressure of \(585 \mathrm{mm} \mathrm{Hg}\) at \(25^{\circ} \mathrm{C}\) what mass of dimethyldichlorosilane, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{SiCl}_{2}(\mathrm{g}),\) can be formed? $$\mathrm{Si}(\mathrm{s})+2 \mathrm{CH}_{3} \mathrm{Cl}(\mathrm{g}) \longrightarrow\left(\mathrm{CH}_{3}\right)_{2} \mathrm{Si} \mathrm{Cl}_{2}(\mathrm{g})$$ What pressure of \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{SiCl}_{2}(\mathrm{g})\) would you expect in this same flask at \(95^{\circ}\) C on completion of the reaction? (Dimethyldichlorosilane is one starting material used to make silicones, polymeric substances used as lubricants, antistick agents, and water-proofing caulk.)

\(\mathrm{Ni}(\mathrm{CO})_{4}\) can be made by reacting finely divided nickel with gaseous CO. If you have \(\mathrm{CO}\) in a \(1.50-\mathrm{L}\). flask at a pressure of \(418 \mathrm{mm}\) Hg at \(25.0^{\circ} \mathrm{C},\) along with \(0.450 \mathrm{g}\) of \(\mathrm{Ni}\) powder, what is the theoretical yield of \(\mathrm{Ni}(\mathrm{CO})_{4} ?\)

The gas \(\mathrm{B}_{2} \mathrm{H}_{6}\) burns in air to give \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{B}_{2} \mathrm{O}_{3}\) $$ \mathrm{B}_{2} \mathrm{H}_{6}(\mathrm{g})+3 \mathrm{O}_{2}(\mathrm{g}) \longrightarrow \mathrm{B}_{2} \mathrm{O}_{3}(\mathrm{s})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) $$ (a) Three gases are involved in this reaction. Place them in order of increasing molecular speed. (Assume all are at the same temperature.) (b) A \(3.26-\) I. flask contains \(B_{2} H_{6}\) at a pressure of \(256 \mathrm{mm}\) Hg and a temperature of \(25^{\circ} \mathrm{C}\). Suppose \(\mathrm{O}_{2}\) gas is added to the flask until \(\mathrm{B}_{2} \mathrm{H}_{6}\) and \(\mathrm{O}_{2}\) are in the correct stoichiometric ratio for the combustion reaction. At this point, what is the partial pressure of \(\mathrm{O}_{2} ?\)

You have four gas samples: 1\. \(1.0 \mathrm{L}\) of \(\mathrm{H}_{2}\) at \(\mathrm{STP}\) 2\. \(1.0 \mathrm{L}\) of \(\mathrm{Ar}\) at \(\mathrm{STP}\) 3\. \(1.0 \mathrm{L}\) of \(\mathrm{H}_{2}\) at \(27^{\circ} \mathrm{C}\) and \(760 \mathrm{mm} \mathrm{Hg}\) 4\. \(1.0 \mathrm{L}\) of He at \(0^{\circ} \mathrm{C}\) and \(900 \mathrm{mm} \mathrm{Hg}\) (a) Which sample has the largest number of gas particles (atoms or molecules)? (b) Which sample contains the smallest number of particles? (c) Which sample represents the largest mass?

An automobile tire has a volume of 17 L. What mass of air is contained in the tire at \(25^{\circ} \mathrm{C}\) and a pressure of 3.2 atm? (Molar mass of air \(=28.96 \mathrm{g} / \mathrm{mol}\).)

Diborane, \(\mathrm{B}_{2} \mathrm{H}_{6},\) reacts with oxygen to give boric oxide and water vapor. $$ \mathrm{B}_{2} \mathrm{H}_{6}(\mathrm{g})+3 \mathrm{O}_{2}(\mathrm{g}) \longrightarrow \mathrm{B}_{2} \mathrm{O}_{3}(\mathrm{s})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) $$ If you \(\operatorname{mix} \mathrm{B}_{2} \mathrm{H}_{6}\) and \(\mathrm{O}_{2}\) in the correct stoichiometric ratio, and if the total pressure of the mixture is \(228 \mathrm{mm} \mathrm{Hg}\), what are the partial pressures of \(\mathrm{B}_{2} \mathrm{H}_{6}\) and \(\mathrm{O}_{2}\) ? If the temperature and volume do not change, what is the pressure of the water vapor?

There are five compounds in the family of sulfur-fluorine compounds with the general formula \(\mathrm{S}_{x} \mathrm{F}_{y}\). One of these compounds is \(25.23 \%\) S. If you place 0.0955 g of the compound in a \(89-\mathrm{mL}\). flask at \(45^{\circ} \mathrm{C},\) the pressure of the gas is \(83.8 \mathrm{mm}\) Hg. What is the molecular formula of \(\mathrm{S}_{x} \mathrm{F}_{y}^{2}\)

Iron carbonyl can be made by the direct reaction of iron metal and carbon monoxide. $$ \mathrm{Fe}(\mathrm{s})+5 \mathrm{CO}(\mathrm{g}) \longrightarrow \mathrm{Fe}(\mathrm{CO})_{5}(\ell) $$ What is the theoretical yield of \(\mathrm{Fe}(\mathrm{CO})_{5}\), if \(3.52 \mathrm{g}\) of iron is treated with CO gas having a pressure of \(732 \mathrm{mm}\) Hg in a \(5.50-\) I. Hask at \(23^{\circ} \mathrm{C} ?\)

You are given a solid mixture of \(\mathrm{NaNO}_{2}\) and \(\mathrm{NaCl}\) and are asked to analyze it for the amount of NaNO, present. To do so you allow the mixture to react with sulfamic acid, \(\mathrm{HSO}_{3} \mathrm{NH}_{2},\) in water according to the equation \(\mathrm{NaNO}_{2}(\mathrm{aq})+\mathrm{HSO}_{3} \mathrm{NH}_{2}(\mathrm{aq}) \longrightarrow\) $$ \mathrm{NaHSO}_{4}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{N}_{2}(\mathrm{g}) $$ What is the weight percentage of \(\mathrm{NaNO}_{2}\) in \(1.232 \mathrm{g}\) of the solid mixture if reaction with sulfamic acid produces \(295 \mathrm{mL}\) of \(\mathrm{N}_{2}\) gas with a pressure of \(713 \mathrm{mm} \mathrm{Hg}\) at \(21.0^{\circ} \mathrm{C} ?\)

The density of air \(20 \mathrm{km}\) above the earth's surface is \(92 \mathrm{g} / \mathrm{m}^{3} .\) The pressure of the atmosphere is \(42 \mathrm{mm} \mathrm{Hg}\) and the temperature is \(-63^{\circ} \mathrm{C}\) (a) What is the average molar mass of the atmosphere at this altitude? (b) If the atmosphere at this altitude consists of only \(\mathrm{O}_{2}\) and \(\mathrm{N}_{2}\), what is the mole fraction of each gas?

Phosphine gas, \(\mathrm{PH}_{3},\) is toxic when it reaches a concentration of \(7 \times 10^{-5} \mathrm{mg} / \mathrm{L} .\) To what pressure does this correspond at \(25^{\circ} \mathrm{C} ?\)

A xenon fluoride can be prepared by heating a mixture of Xe and \(\mathrm{F}_{2}\) gases to a high temperature in a pressure-proof container. Assume that xenon gas was added to a \(0.25-\mathrm{L}\) container until its pressure reached 0.12 atm at \(0.0^{\circ} \mathrm{C}\) Fluorine gas was then added until the total pressure reached 0.72 atm at \(0.0^{\circ} \mathrm{C}\). After the reaction was complete, the xenon was consumed completely and the pressure of the \(\mathrm{F}_{2}\) remaining in the container was \(0.36 \mathrm{atm}\) at \(0.0^{\circ} \mathrm{C} .\) What is the empirical formula of the xenon fluoride?

Chlorine dioxide, \(\mathrm{ClO}_{2}\), reacts with fluorine to give a new gas that contains \(\mathrm{Cl}, \mathrm{O},\) and \(\mathrm{F}\). In an experiment you find that \(0.150 \mathrm{g}\) of this new gas has a pressure of \(17.2 \mathrm{mm}\) Hg in a 1850 -mL. flask at \(21^{\circ} \mathrm{C}\). What is the identity of the unknown gas?

A balloon at the circus is filled with helium gas to a gauge pressure of \(22 \mathrm{mm}\) Hg at \(25^{\circ} \mathrm{C}\). The volume of the gas is \(305 \mathrm{mL},\) and the barometric pressure is \(755 \mathrm{mm}\) Hg. What amount of helium is in the balloon? (Remember that gauge pressure \(=\) total pressure - barometric pressure. See page \(550 .)\)

Acetylene can be made by allowing calcium carbide to react with water: $$ \mathrm{CaC}_{2}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{g})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{s}) $$ Suppose you react \(2.65 \mathrm{g}\) of \(\mathrm{CaC}_{2}\) with excess water. If you collect the acetylene and find that the gas has a volume of \(795 \mathrm{mL}\) at \(25.2^{\circ} \mathrm{C}\) with a pressure of \(735.2 \mathrm{mm} \mathrm{Hg},\) what is the percent yield of acetylene?

If you have a sample of water in a closed container, some of the water will evaporate until the pressure of the water vapor, at \(25^{\circ} \mathrm{C},\) is \(23.8 \mathrm{mm}\) Hg. How many molecules of water per cubic centimeter exist in the vapor phase?

You are given \(1.56 \mathrm{g}\) of a mixture of \(\mathrm{KClO}_{3}\) and \(\mathrm{KCl}\). When heated, the KClOs decomposes to KCl and \(\mathrm{O}_{2}\), $$ 2 \mathrm{KClO}_{3}(\mathrm{s}) \longrightarrow 2 \mathrm{KCl}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{g}) $$ and \(327 \mathrm{mL}\) of \(\mathrm{O}_{2}\) with a pressure of \(735 \mathrm{mm} \mathrm{Hg}\) is collected at \(19^{\circ} \mathrm{C}\). What is the weight percentage of \(\mathrm{KClO}_{3}\) in the sample?

A A study of climbers who reached the summit of Mount Everest without supplemental oxygen showed that the partial pressures of \(\mathrm{O}_{2}\) and \(\mathrm{CO}_{2}\) in their lungs were \(35 \mathrm{mm}\) Hg and \(7.5 \mathrm{mm}\) Hg, respectively. The barometric pressure at the summit was \(253 \mathrm{mm}\) Hg. Assume the lung gases are saturated with moisture at a body temperature of \(37^{\circ} \mathrm{C}\) [which means the partial pressure of water vapor in the lungs is \(P\left(\mathrm{H}_{2} \mathrm{O}\right)=47.1 \mathrm{mm} \mathrm{Hg}\) ]. If you assume the lung gases consists of only \(\mathrm{O}_{2}, \mathrm{N}_{2}, \mathrm{CO}_{2},\) and \(\mathrm{H}_{2} \mathrm{O},\) what is the partial pressure of \(\mathrm{N}_{2} ?\)

Nitrogen monoxide reacts with oxygen to give nitrogen dioxide: $$ 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NO}_{2}(\mathrm{g}) $$ (a) Place the three gases in order of increasing rms speed at \(298 \mathrm{K}\) (b) If you mix \(\mathrm{NO}\) and \(\mathrm{O}_{2}\) in the correct stoichiometric ratio, and NO has a partial pressure of \(150 \mathrm{mm} \mathrm{Hg}\) what is the partial pressure of \(\mathrm{O}_{2} ?\) (c) After reaction between \(\mathrm{NO}\) and \(\mathrm{O}_{2}\) is complete, what is the pressure of \(\mathrm{NO}_{2}\) if the NO originally had a pres. sure of \(150 \mathrm{mm} \mathrm{Hg}\) and \(\mathrm{O}_{2}\) was added in the correct stoichiometric amount?

Ammonia gas is synthesized by combining hydrogen and nitrogen: $$ 3 \mathrm{H}_{2}(\mathrm{g})+\mathrm{N}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{g}) $$ (a) If you want to produce 562 g of \(\mathrm{NH}_{3}\), what volume of \(\mathrm{H}_{2}\) gas, at \(56^{\circ} \mathrm{C}\) and \(745 \mathrm{mm} \mathrm{Hg}\), is required? (b) To produce 562 g of \(\mathrm{NH}_{3},\) what volume of air (the source of \(\mathrm{N}_{2}\) ) is required if the air is introduced at \(29^{\circ} \mathrm{C}\) and \(745 \mathrm{mm}\) Hg? (Assume the air sample has \(\left.78.1 \text { mole } \% N_{2} .\right)\)

You have a \(550-\mathrm{ml}\). tank of gas with a pressure of 1.56 atm at \(24^{\circ} \mathrm{C}\). You thought the gas was pure carbon monoxide gas, \(\mathrm{CO}\), but you later found it was contaminated by small quantities of gaseous \(\mathrm{CO}_{2}\) and \(\mathrm{O}_{2}\). Analysis shows that the tank pressure is 1.34 atm (at \(24^{-} \mathrm{C}\) ) if the \(\mathrm{CO}_{2}\) is removed. Another experiment shows that \(0.0870 \mathrm{~g}\) of \(\mathrm{O}_{2}\) can be removed chemically. What are the masses of \(\mathrm{CO}\) and \(\mathrm{CO}_{2}\) in the tank, and what is the partial pressure of each of the three gases at \(25^{\circ} \mathrm{C}\) ?

Methane is burned in a laboratory Bunsen burner to give \(\mathrm{CO}_{2}\) and water vapor. Methane gas is supplied to the burner at the rate of \(5.0 \mathrm{L} / \mathrm{min}\) (at a temperature of \(28^{\circ} \mathrm{C}\) and a pressure of \(773 \mathrm{mm} \mathrm{Hg}\) ). At what rate must oxygen be supplicd to the burner (at a pressure of \(742 \mathrm{mm} \mathrm{Hg}\) and a temperature of \(26^{\circ} \mathrm{C}\) ) \(?\)

Group 2 A metal carbonates are decomposed to the metal oxide and \(\mathrm{CO}_{2}\) on heating: $$ \mathrm{MCO}_{3}(\mathrm{s}) \longrightarrow \mathrm{MO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{g}) $$ You heat \(0.158 \mathrm{g}\) of a white, solid carbonate of a Group \(2 \mathrm{A}\) metal (M) and find that the evolved \(\mathrm{CO}_{2}\) has a pressure of \(69.8 \mathrm{mm} \mathrm{Hg}\) in a \(285-\mathrm{mL}\). Hask at \(25^{\circ} \mathrm{C} .\) Identify \(\mathrm{M}\).

Silane, \(\mathrm{SiH}_{4},\) reacts with \(\mathrm{O}_{2}\) to give silicon dioxide and water vapor: $$ \mathrm{SiH}_{4}(\mathrm{g})+2 \mathrm{O}_{2}(\mathrm{g}) \longrightarrow \mathrm{SiO}_{2}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) $$ If you mix \(\mathrm{SiH}_{4}\) with \(\mathrm{O}_{2}\) in the correct stoichiometric ratio, and if the total pressure of the mixture is \(120 \mathrm{mm} \mathrm{Hg}\), what are the partial pressures of \(\mathrm{SiH}_{4}\) and \(\mathrm{O}_{2} ?\) When the reactants have been completely consumed, what is the total pressure in the flask? (Assume T is constant.)

One way to synthesize diborane, \(\mathrm{B}_{2} \mathrm{H}_{6}\), is the reaction \(2 \mathrm{NaBH}_{4}(\mathrm{s})+2 \mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq}) \longrightarrow\) $$ \mathrm{B}_{2} \mathrm{H}_{6}(\mathrm{g})+2 \mathrm{NaH}_{2} \mathrm{PO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2}(\mathrm{g}) $$ (a) If you have \(0.136 \mathrm{g}\) of \(\mathrm{NaBH}_{4}\) and excess \(\mathrm{H}_{3} \mathrm{PO}_{4},\) and you collect the \(\mathrm{B}_{2} \mathrm{H}_{6}\) in a 2.75 L. flask at \(25^{\circ} \mathrm{C},\) what is the pressure of the \(\mathrm{B}_{2} \mathrm{H}_{6}\) in the flask? (b) A byproduct of the reaction is \(\mathrm{H}_{2}\) gas. If both \(\mathrm{B}_{2} \mathrm{H}_{6}\) and H \(_{2}\) gas come from this reaction, what is the total pressure in the 2.75 -L. flask (after reaction of \(0.136 \mathrm{g}\) of NaBH, with excess \(\mathrm{H}_{3} \mathrm{PO}_{4}\) ) at \(25^{\circ} \mathrm{C} ?^{2}\)

A You have \(1.249 \mathrm{g}\) of a mixture of \(\mathrm{NaHCO}_{3}\) and \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) You find that \(12.0 \mathrm{mL}\) of \(1.50 \mathrm{M} \mathrm{HCl}\) is required to convert the sample completely to \(\mathrm{NaCl}, \mathrm{H}_{2} \mathrm{O},\) and \(\mathrm{CO}_{2}\) \(\mathrm{NaHCO}_{3}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \longrightarrow\) $$ \mathrm{NaCl}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g}) $$ \(\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{aq})+2 \mathrm{HCl}(\mathrm{aq}) \longrightarrow\) $$ 2 \mathrm{NaCl}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g}) $$ What volume of \(\mathrm{CO}_{2}\) is evolved at \(745 \mathrm{mm}\) Hg and \(25^{\circ} \mathrm{C} ?\)

A \(1.0-\) L flask contains \(10.0 \mathrm{g}\) each of \(\mathrm{O}_{2}\) and \(\mathrm{CO}_{2}\) at \(25^{\circ} \mathrm{C}\) (a) Which gas has the greater partial pressure, \(\mathbf{O}_{2}\) or \(\mathbf{C O}_{2}\) or are they the same? (b) Which molecules have the greater average speed, or are they the same? (c) Which molecules have the greater average kinetic energy, or are they the same?

If equal masses of \(\mathrm{O}_{2}\) and \(\mathrm{N}_{2}\) are placed in separate containers of equal volume at the same temperature, which of the following statements is true? If false, tell why it is false. (a) The pressure in the flask containing \(\mathrm{N}_{2}\) is greater than that in the llask containing \(\mathbf{O}_{2}\) (b) There are more molecules in the flask containing \(\mathrm{O}_{2}\) than in the flask containing \(\mathbf{N}_{2}\)

You have two pressure-proof steel cylinders of equal volume, one containing \(1.0 \mathrm{kg}\) of \(\mathrm{CO}\) and the other containing \(1.0 \mathrm{kg}\) of acetylenc, \(\mathrm{C}_{2} \mathrm{H}_{2}\) (a) In which cylinder is the pressure greater at \(25^{\circ} \mathrm{C} ?\) (b) Which cylinder contains the greater number of molecules?

Two flasks, each with a volume of \(1.00 \mathrm{L},\) contain \(\mathrm{O}_{2}\) gas with a pressure of \(380 \mathrm{mm}\) Hg. Flask \(\mathrm{A}\) is at \(25^{\circ} \mathrm{C},\) and flask \(\mathrm{B}\) is at \(0^{\circ} \mathrm{C}\). Which flask contains the greater number of \(\mathrm{O}_{2}\) molecules?

A State whether each of the following samples of matter is a gas. If there is not enough information for you to decide, write "insufficient information." (a) A material is in a steel tank at 100 atm pressure. When the tank is opened to the atmosphere, the material suddenly expands, increasing its volume by \(10 \%\) (b) A 1.0 -mL sample of material weighs \(8.2 \mathrm{g}\) (c) The material is transparent and pale green in color. (d) One cubic meter of material contains as many molecules as \(1.0 \mathrm{m}^{3}\) of air at the same temperature and pressure.

Each of the four tires of a car is filled with a different gas. Each tire has the same volume, and each is filled to the same pressure, 3.0 atm, at \(25^{\circ} \mathrm{C}\). One tire contains \(116 \mathrm{g}\) of air, another tire has \(80.7 \mathrm{g}\) of neon, another tire has \(16.0 \mathrm{g}\) of helium, and the fourth tire has \(160 . \mathrm{g}\) of an unknown gas. (a) Do all four tires contain the same number of gas molecules? If not, which one has the greatest number of molecules? (b) How many times heavier is a molecule of the unknown gas than an atom of helium? (c) In which tire do the molecules have the largest kinetic energy? The highest average speed?

The sodium azide required for automobile air bags is made by the reaction of sodium metal with dinitrogen oxide in liquid ammonia: \(3 \mathrm{N}_{2} \mathrm{O}(\mathrm{g})+4 \mathrm{Na}(\mathrm{s})+\mathrm{NH}_{3}(\ell) \longrightarrow\) $$ \mathrm{NaN}_{3}(\mathrm{s})+3 \mathrm{NaOH}(\mathrm{s})+2 \mathrm{N}_{2}(\mathrm{g}) $$ (a) You have \(65.0 \mathrm{g}\) of sodium and a \(35.0-\mathrm{L}\). flask containing \(\mathrm{N}_{2}\) O gas with a pressure of 2.12 atm at \(23^{\circ} \mathrm{C}\) What is the theoretical yield (in grams) of NaNg? (b) Draw a Lewis structure for the azide ion. Include all possible resonance structures. Which resonance structure is most likely? (c) What is the shape of the azide ion?

If the absolute temperature of a gas doubles, by how much does the average speed of the gaseous molecules increase? (See General ChemistryNow Screen \(12.9 .\) )