What is the volume occupied by 0.255 mol of helium gas at 1.25 atm and 305 K?

What is pressure?

Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose a can contains a residual amount of gas at a pressure of 755 mm Hg and \(25^{\circ} \mathrm{C}\). What would the pressure be if the can were heated to \(1155^{\circ} \mathrm{C}\)? Equation Transcription: Text Transcription: 25 degrees C 1155 degrees C

Explain how drinking from a straw works. What causes the beverage to go up the straw? Is there an upper limit to how long a straw can theoretically be and still work as a drinking straw?

What are the main assumptions of kinetic molecular theory?

Why do we experience pain in our ears during changes in altitude?

Describe the main properties of a gas. How are these predicted by kinetic molecular theory?

What units are used to measure pressure?

What is Boyle’s law? Explain Boyle’s law from the perspective of kinetic molecular theory.

Explain why scuba divers should not hold their breath as they ascend to the surface.

Why would it be impossible to breathe air through an extra-long snorkel (greater than a couple of meters) while swimming underwater?

What is Charles’s law? Explain Charles’s law from the perspective of kinetic molecular theory.

Explain why hot-air balloons float above the ground.

What is the combined gas law? When is it useful?

PROBLEM 13Q What is Avogadro's law? Explain Avogadro's law from the perspective of kinetic molecular theory.

What is the ideal gas law? When is it useful?

Under what conditions is the ideal gas law most accurate? Under what conditions does the ideal gas law break down? Why?

What is partial pressure?

What is Dalton’s law?

Describe hypoxia and oxygen toxicity.

Why do deep-sea divers breathe a mixture of helium and oxygen?

When a gas is collected over water, is the gas pure? Why or why not?

What is vapor pressure?

What is standard temperature and pressure (STP)? What is the molar volume of a gas at STP?

Convert each measurement to atm. (a) \(1277 \mathrm{~mm}\ \mathrm{Hg}\) (b) \(2.38 \times 10^{5} \mathrm{~Pa}\) (c) \(127 \text { psi }\) (d) \(455 \text { torr }\) Equation Transcription: Text Transcription: 1277 mm Hg 2.38 times 10^5 Pa 127 psi 455 torr

Convert each measurement to atm. (a) \(921 \text { torr }\) (b) \(4.8 \times 10^{4} \mathrm{~Pa}\) (c) \(87.5\ p s i\) (d) \(34.22 \text { in. } H g\) Equation Transcription: Text Transcription: 921 torr 4.8 times 10^4 Pa 87.5 psi 34.22 in. Hg

Perform each conversion. (a) 2.3 atm to torr (b) \(4.7 \times 10^{-2} \mathrm{~atm}\) to millimeters of mercury (c) 24.8 psi to millimeters of mercury (d) 32.84 in Hg to torr

Complete the table.

The pressure in Denver, Colorado (5280-ft elevation), averages about 24.9 in. Hg. Convert this pressure to: (a) atmospheres (b) millimeters of mercury (c) pounds per square inch (d) pascals

The pressure on top of Mount Everest averages about 235 mm Hg. Convert this pressure to: (a) torr (b) pounds per square inch (c) inches of mercury (d) atmospheres

Perform each conversion. (a) 1.06 atm to millimeters of mercury (b) 95,422 Pa to millimeters of mercury (c) 22.3 psi to torr (d) 35.78 in. Hg to millimeters of mercury

The North American record for highest recorded barometric pressure is 31.85 in. Hg, set in 1989 in Northway, Alaska. Convert this pressure to: (a) millimeters of mercury (b) atmospheres (c) torr (d) kilopascals

A sample of gas has an initial volume of 3.95 L at a pressure of 705 mm Hg. If the volume of the gas is increased to 5.38 L, what is the pressure? (Assume constant temperature.)

PROBLEM 34P A sample of gas has an initial volume of 22.8 L at a pressure of 1.65 atm. If the sample is compressed to a volume of 10.7 L, what is its pressure? (Assume constant temperature.)

PROBLEM 35P A snorkeler with a lung capacity of 6.3 L inhales a lungful of air at the surface, where the pressure is 1.0 atm. The snorkeler then descends to a depth of 25 m, where the pressure increases to 3.5 atm. What is the capacity of the snorkeler's lungs at this depth? (Assume constant temperature.)

PROBLEM 36P A scuba diver with a lung capacity of 5.2 L inhales at a depth of 45 m and a pressure of 5.5 atm. If the diver were to ascend to the surface (where the pressure is 1.0 atm) while holding her breath, to what volume would the air in her lungs expand? (Assume constant temperature.)

Use Boyle’s law to complete the table (assume temperature and number of moles of gas to be constant).

Use Boyle’s law to complete the table (assume temperature and number of moles of gas to be constant).

A balloon with an initial volume of 3.2 L at a temperature of 299 K is warmed to 376 K. What is its volume at 376 K?

A dramatic classroom demonstration involves cooling a balloon from room temperature (298 K) to liquid nitrogen temperature (77 K). If the initial volume of the balloon is 2.7 L, what is its volume after it cools? (Ignore the effect of any gases that might liquefy upon cooling.)

A 48.3-mL sample of gas in a cylinder equipped with a piston is warmed from \(22^{\circ} \mathrm{C} \text { to } 87^{\circ} \mathrm{C}\). What is its volume at the final temperature? Equation Transcription: Text Transcription: 22 degrees C to 87 degrees C

A syringe containing 1.55 mL of oxygen gas is cooled from \(95.3^{\circ} \mathrm{C} \text { to } 0.0^{\circ} \mathrm{C}\). What is the final volume of oxygen gas? Equation Transcription: Text Transcription: 95.3 degrees C to 0.0 degrees C

PROBLEM 44P Use Charles's law to complete the table (assume pressure and number of moles of gas to be constant). V1 T1 V2 T2 119 L 10.5 °C _______ 112.3 °C _______ 135 K 176 mL 315 K 2.11 L 15.4 °C 2.33 L _______ 15.4 cm3 _______ 19.2 cm3 10.4 °C

A 0.12-mole sample of nitrogen gas occupies a volume of 2.55 L. What is the volume of 0.32 mol of nitrogen gas under the same conditions?

PROBLEM 43P Use Charles's law to complete the table (assume pressure and number of moles of gas to be constant). V1 T1 V2 T2 1.08 L 25.4 °C 1.33 L _______ _______ 77 K 228 mL 298 K 115 cm3 _______ 119 cm3 22.4 °C 232 L 18.5 °C _______ 96.2 °C

A 0.48-mole sample of helium gas occupies a volume of 11.7 L. What is the volume of 0.72 mol of helium gas under the same conditions?

A balloon contains 0.128 mol of gas and has a volume of 2.76 L. If an additional 0.073 mol of gas is added to the balloon, what is its final volume?

A cylinder with a moveable piston contains 0.87 mol of gas and has a volume of 334 mL. What will its volume be if an additional 0.22 mol of gas is added to the cylinder?

Use Avogadro’s law to complete the table (assume pressure and temperature to be constant).

Use Avogadro’s law to complete the table (assume pressure and temperature to be constant).

PROBLEM 51P A sample of gas with an initial volume of 28.4 L at a pressure of 725 mm Hg and a temperature of 305 K is compressed to a volume of 14.8 L and warmed to a temperature of 375 K. What is the final pressure of the gas?

A cylinder with a moveable piston contains 218 mL of nitrogen gas at a pressure of 1.32 atm and a temperature of 298 K. What must the final volume be for the pressure of the gas to be 1.55 atm at a temperature of 335 K?

PROBLEM 53P A scuba diver takes a 2.8-L balloon from the surface, where the pressure is 1.0 atm and the temperature is 34 °C, to a depth of 25 m, where the pressure is 3.5 atm and the temperature is 18 °C. What is the volume of the balloon at this depth?

A bag of potato chips contains 585 mL of air at \(25^{\circ} \mathrm{C}\) and a pressure of 765 mm Hg. Assuming the bag does not break, what will be its volume at the top of a mountain where the pressure is 442 mm Hg and the temperature is \(5.0^{\circ} \mathrm{C}\)? Equation Transcription: Text Transcription: 25 degrees C 5 degrees C

A gas sample with a volume of 5.3 L has a pressure of 735 mm Hg at \(28^{\circ} \mathrm{C}\). What is the pressure of the sample if the volume remains at 5.3 L but the temperature rises to \(86^{\circ} \mathrm{C}\)? Equation Transcription: Text Transcription: 28 degrees C 86 degrees C

The total pressure in a 11.7-L automobile tire is 44 psi at \(11^{\circ} \mathrm{C}\). How much does the pressure in the tire rise if its temperature increases to \(37^{\circ} \mathrm{C}\) and the volume remains at 11.7 L? Equation Transcription: Text Transcription: 11 degrees C 37 degrees C

Use the combined gas law to complete the table (assume the number of moles of gas to be constant).

What is the volume occupied by 0.255 mol of helium gas at 1.25 atm and 305 K?

Use the combined gas law to complete the table (assume the number of moles of gas to be constant).

What is the pressure in a 20.0-L cylinder filled with 0.683 mol of nitrogen gas at 325 K?

A cylinder contains 28.5 L of oxygen gas at a pressure of 1.8 atm and a temperature of 298 K. How many moles of gas are in the cylinder?

What is the temperature of 0.52 mol of gas at a pressure of 1.3 atm and a volume of 11.8 L?

A cylinder contains 11.8 L of air at a total pressure of 43.2 psi and a temperature of \(25^{\circ} \mathrm{C}\). How many moles of gas does the cylinder contain? Equation Transcription: Text Transcription: 25 degrees C

What is the pressure in millimeters of mercury of 0.0115 mol of helium gas with a volume of 214 mL at \(45^{\circ} \mathrm{C}\)? Equation Transcription: Text Transcription: 45 degrees C

Use the ideal gas law to complete the table.

How many moles of gas must be forced into a 4.8-L tire to give it a gauge pressure of 32.4 psi at \(25^{\circ} \mathrm{C}\)? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.7 psi so that the total pressure in the tire is 47.1 psi. Equation Transcription: Text Transcription: 25 degrees C

How many moles of gas must be forced into a 3.5-L ball to give it a gauge pressure of 9.4 psi at \(25^{\circ} \mathrm{C}\)? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.7 psi so that the total pressure in the ball is 24.1 psi. Equation Transcription: Text Transcription: 25 degrees C

Use the ideal gas law to complete the table.

PROBLEM 69P An experiment shows that a 248-mL gas sample has a mass of 0.433 g at a pressure of 745 mm Hg and a temperature of 28 °C. What is the molar mass of the gas?

PROBLEM 70P An experiment shows that a 113-mL gas sample has a mass of 0.171 g at a pressure of 721 mm Hg and a temperature of 32 °C. What is the molar mass of the gas?

PROBLEM 71Q A sample of gas has a mass of 38.8 mg. Its volume is 224 mL at a temperature of 55 °C and a pressure of 886 torr. Find the molar mass of the gas.

A sample of gas has a mass of 0.555 g. Its volume is 117 mL at a temperature of \(85^{\circ} \mathrm{C}\) and a pressure of 753 mm Hg. Find the molar mass of the gas.

A gas mixture contains each gas at the indicated partial pressure. \(N_{2}\) 217 torr \(O_{2}\) 106 torr \(\text { He }\) 248 torr What is the total pressure of the mixture?

A heliox deep-sea diving mixture delivers an oxygen partial pressure of 0.30 atm when the total pressure is 11.0 atm. What is the partial pressure of helium in this mixture?

A gas mixture contains each gas at the indicated partial pressure. \(\mathrm{CO}_{2}\) 422 mm Hg \(A r\) 102 mm Hg \(\mathrm{O}_{2}\) 165 mm Hg \(H_{2}\) 52 mm Hg What is the total pressure of the mixture? Equation Transcription: Text Transcription: CO_2 Ar O_2 H_2

A mixture of helium, nitrogen, and oxygen has a total pressure of 752 mm Hg. The partial pressures of helium and nitrogen are 234 mm Hg and 197 mm Hg, respectively. What is the partial pressure of oxygen in the mixture?

The hydrogen gas formed in a chemical reaction is collected over water at \(30^\circ \mathrm C\) at a total pressure of 732 mm Hg. What is the partial pressure of the hydrogen gas collected in this way?

The oxygen gas emitted from an aquatic plant during photosynthesis is collected over water at \(25^{\circ} \mathrm{C}\) and a total pressure of 753 torr. What is the partial pressure of the oxygen gas? Equation Transcription: Text Transcription: 25 degrees C

A gas mixture contains 78% nitrogen and 22% oxygen. If the total pressure is 1.12 atm, what are the partial pressures of each component?

An air sample contains 0.038% \(\mathrm{CO}_{2}\). If the total pressure is 758 mm Hg, what is the partial pressure of \(\mathrm{CO}_{2}\)? Equation Transcription: Text Transcription: CO_2

A heliox deep-sea diving mixture contains 4.0% oxygen and 96.0% helium. What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.5 atm?

A scuba diver breathing normal air descends to 100 m of depth, where the total pressure is 11 atm. What is the partial pressure of oxygen that the diver experiences at this depth? Is the diver in danger of experiencing oxygen toxicity?

Calculate the volume of each gas sample at STP. (a) 73.9 g \(N_{2}\) (b) 42.9 g \(O_{2}\) (c) 148 g \(\mathrm{NO}_{2}\) (d) 245 mg \(\mathrm{CO}_{2}\) Equation Transcription: Text Transcription: N_2 O_2 NO_2 CO_2

Calculate the volume of each gas sample at STP. (a) 22.5 mol \(\mathrm{Cl}_{2}\) (b) 3.6 mol nitrogen (c) 2.2 mol helium (d) 27 mol \(\mathrm{CH}_{4}\) Equation Transcription: Text Transcription: Cl_2 CH_4

Calculate the volume of each gas sample at STP. (a) 21.2 mol \(\mathrm{N}_{2} \mathrm{O}\) (b) 0.215 mol \(C O\) (c) 0.364 mol \(\mathrm{CO}_{2}\) (d) 8.6 mol \(C_{2} H_{6}\) Equation Transcription: Text Transcription: N_2 O CO CO_2 C_2 H_6

Calculate the mass of each gas sample at STP. (a) 178 mL \(\mathrm{CO}_{2}\) (b) 155 mL \(\mathrm{O}_{2}\) (c) 1.25 L \(S F_{6}\) Equation Transcription: Text Transcription: CO_2 O_2 SF_6

PROBLEM 88P Calculate the mass of each gas sample at STP. (a) 5.82 L NO (b) 0.324 LN2 (c) 139 cm3 Ar

Calculate the volume of each gas sample at STP. (a) 48.9 g \(\mathrm{He}\) (b) 45.2 g \(X e\) (c) 48.2 mg \(\mathrm{Cl}_{2}\) (d) 3.83 kg \(\mathrm{SO}_{2}\) Equation Transcription: Text Transcription: He Xe Cl_2 SO_2

Consider the chemical reaction: \(\mathrm{C}(s)+\mathrm{H}_2 \mathrm{O}(g) \longrightarrow \mathrm{CO}(g)+\mathrm{H}_2(g)\) How many liters of hydrogen gas are formed from the complete reaction of 1.07 mol of C? Assume that the hydrogen gas is collected at 1.0 atm and 315 K.

Consider the chemical reaction: \(2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g)\) How many moles of \({H}_{2}O\) are required to form 1.3 L of \({O}_{2}\) at 325 K and 0.988 atm? Equation Transcription: Text Transcription: 2 H_2 O(l) right arrow 2 H_2 (g) + O_2 (g)

Oxygen gas reacts with powdered aluminum according to the reaction: \(4 \mathrm{Al}(\mathrm{s})+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{~s})\) How many liters of \({O}_{2}\) gas, measured at 782 mm Hg and \(25^{\circ} \mathrm{C}\), are required to completely react with 2.4 mol of Al? Equation Transcription: Text Transcription: 4 Al(s)+3 O_2 (g) right arrow 2 Al_2 O_3 (s) 25 degrees C

\(\mathrm{CH}_{3} \mathrm{OH}\) can be synthesized by the reaction: \(\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(g)\) How many liters of \(H_{2}\) gas, measured at 748 mm Hg and \(86^{\circ} \mathrm{C}\), are required to synthesize 0.55 mol of \(\mathrm{CH}_{3} \mathrm{OH}\)? How many liters of CO gas, measured under the same conditions, are required? Equation Transcription: Text Transcription: CH_3 OH CO(g)+2 H_2 (g) right arrow CH_3 OH(g) H_2 86 degrees C

Nitrogen reacts with powdered aluminum according to the reaction: \(2\ A l(s)+N_{2}(g) \rightarrow 2\ A l N(s)\) How many liters of \({N}_{2}\) gas, measured at 892 torr and \(95^{\circ} \mathrm{C}\), are required to completely react with 18.5 g of Al? Equation Transcription: Text Transcription: 2 Al(s) + N_2 (g) right arrow 2 AlN(s) 95 degrees C

Sodium reacts with chlorine gas according to the reaction: \(2\ \mathrm{Na}(\mathrm{s})+\mathrm{Cl}_{2}(g) \rightarrow 2\ \mathrm{NaCl}(\mathrm{s})\) What volume of \({C l}_{2}\) gas, measured at 687 torr and \(35^{\circ} \mathrm{C}\), is required to form 28 g of NaCl? Equation Transcription: Text Transcription: 2 Na(s)+Cl_2 (g) right arrow 2 NaCl(s) 35 degrees C

Lithium reacts with nitrogen gas according to the reaction: \(6\ \mathrm{Li}(\mathrm{s})+N_{2}(g) \rightarrow 2\ L i_{3} N(s)\) How many grams of lithium are required to completely react with 58.5 mL of \({N}_{2}\) gas measured at STP? Equation Transcription: Text Transcription: 6 Li(s) + N_2 (g) right arrow 2 Li_3 N(s)

How many grams of \({N H}_{3}\) form when 24.8 L of \({H}_{2}\)( g) (measured at STP) reacts with \({N}_{2}\) to form \({N H}_{3}\) according to this reaction? \(N_{2}(g)+3\ H_{2}(g) \rightarrow 2\ N H_{3}(g)\) Equation Transcription: Text Transcription: N_2 (g) + 3 H_2 (g) right arrow 2 NH_3 (g)

How many grams of calcium are consumed when 156.8 mL of oxygen gas, measured at STP, reacts with calcium according to this reaction? \(2 \mathrm{Ca}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{CaO}(\mathrm{s})\) Equation Transcription: Text Transcription: 2 Ca(s)+O_2 (g) right arrow 2 CaO(s)

How many grams of magnesium oxide form when 14.8 L of oxygen gas, measured at STP, completely reacts with magnesium metal according to this reaction? \(2\ \mathrm{Mg}(\mathrm{s})+\mathrm{O}_{2}(g) \rightarrow 2\ \mathrm{MgO}(\mathrm{s})\) Equation Transcription: Text Transcription: 2 Mg(s) + O_2 (g) right arrow 2 MgO(s)

Use the ideal gas law to show that 28.0 g of nitrogen gas and 4.00 g of helium gas occupy the same volume at any temperature and pressure.

Use the ideal gas law to show that the molar volume of a gas at STP is 22.4 L.

The mass of an evacuated 255-mL flask is 143.187 g. The mass of the flask filled with 267 torr of an unknown gas at \(25^{\circ} \mathrm{C}\) is 143.289 g. Calculate the molar mass of the unknown gas. Equation Transcription: Text Transcription: 25 degrees C

A 118-mL flask is evacuated, and its mass is measured as 97.129 g. When the flask is filled with 768 torr of helium gas at \(35^{\circ} \mathrm{C}\), it is found to have a mass of 97.171 g. Is the gas pure helium? Equation Transcription: Text Transcription: 35 degrees C

A gaseous compound containing hydrogen and carbon is decomposed and found to contain 82.66% carbon and 17.34% hydrogen by mass. The mass of 158 mL of the gas, measured at 556 mm Hg and \(25^{\circ} \mathrm{C}\), is 0.275 g. What is the molecular formula of the compound?

PROBLEM 105P The reaction between zinc and hydrochloric acid is carried out as a source of hydrogen gas in the laboratory: Zn(s) + 2 HCl(aq) ? ZnCl2(aq) + H2(q) If 325 mL of hydrogen gas is collected over water at 25 °C at a total pressure of 748 mm Hg, how many grams of Zn reacted?

A gaseous compound containing hydrogen and carbon is decomposed and found to contain 85.63% C and 14.37% H by mass. The mass of 258 mL of the gas, measured at STP, is 0.646 g. What is the molecular formula of the compound?

Consider the reaction: \(2\ \mathrm{NiO}(\mathrm{s}) \rightarrow 2\ \mathrm{Ni}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g})\) If \({O}_{2}\) is collected over water at \(40^{\circ} \mathrm{C}\) and a total pressure of 745 mm Hg, what volume of gas will be collected for the complete reaction of 24.78 g of NiO? Equation Transcription: Text Transcription: 2 NiO(s) right arrow 2 Ni(s) + O_2 (g) 40 degrees C

How many grams of oxygen are collected in a reaction where 235 mL of oxygen gas is collected over water at a temperature of \(25^{\circ} \mathrm{C}\) and a total pressure of 697 torr? Equation Transcription: Text Transcription: 25 degrees C

How many grams of hydrogen are collected in a reaction where 1.78 L of hydrogen gas is collected over water at a temperature of \(40^{\circ} \mathrm{C}\) and a total pressure of 748 torr? Equation Transcription: Text Transcription: 40 degrees C

The decomposition of a silver oxide sample forms 15.8 g of Ag(s): \(2\ \mathrm{Ag}_{2} \mathrm{O}(\mathrm{s}) \rightarrow 4\ \mathrm{Ag}(\mathrm{s})+\mathrm{O}_{2}(g)\) What total volume of \({O}_{2}\) gas forms if it is collected over water at a temperature of \(25^{\circ} \mathrm{C}\) and a total pressure of 752 mm Hg? Equation Transcription: Text Transcription: 2 Ag_2 O(s) right arrow 4 Ag(s) + O_2 (g) 25 degrees C

The following reaction consumes 2.45 kg of CO(g): \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)\) How many total liters of gas are formed if the products are collected at STP? Equation Transcription: Text Transcription:

PROBLEM 112P When hydrochloric acid is poured over potassium sulfide, 42.9 mL of hydrogen sulfide gas is produced at a pressure of 752 torr and a temperature of 25.8 °C. Write an equation for the gas evolution reaction and determine how much potassium sulfide (in grams) reacted.

When hydrochloric acid is poured over a sample of sodium bicarbonate, 28.2 mL of carbon dioxide gas is produced at a pressure of 0.954 atm and a temperature of \(22.7^{\circ} \mathrm{C}\). Write an equation for the gas evolution reaction and determine how much sodium bicarbonate reacted. Equation Transcription: Text Transcription: 22.7 degrees C

Consider the reaction: \(P_{4}(s)+6\ \mathrm{H}_{2}(g) \rightarrow 4\ \mathrm{PH}_{3}(g)\) (a) If 88.6 L of \({H}_{2}\)( g), measured at STP, is allowed to react with 158.3 g of \({P}_{4}\), what is the limiting reactant? (b) If 48.3 L of \({P H}_{3}\), measured at STP, forms, what is the percent yield? Equation Transcription: Text Transcription: P_4 (s) + 6 H_2 (g) right arrow 4 PH_3 (g)

PROBLEM 115P Consider the reaction for the synthesis of nitric acid: 3 NO2(g) + H2O(l) ? 2 HNO3(aq) + NO(g) (a) If 12.8 L of NO2(g), measured at STP, is allowed to react with 14.9 g of water, find the limiting reagent and the theoretical yield of HNO3 in grams. ________________ (b) If 14.8 g of HNO3 forms, what is the percent yield?

Consider the reaction for the production of \({N O}_{2}\) from NO: \(2\ \mathrm{NO}(g)+\mathrm{O}_{2}(g) \rightarrow 2\ \mathrm{NO}_{2}(g)\) (a) If 84.8 L of \({O}_{2}\)( g), measured at \(35^{\circ} \mathrm{C}\) and 632 mm Hg, is allowed to react with 158.2 g of NO, find the limiting reagent. (b) If 97.3 L of \({N O}_{2}\) forms, measured at \(35^{\circ} \mathrm{C}\) and 632 mm Hg, what is the percent yield? Equation Transcription: Text Transcription: 2 NO(g) + O_2 (g) right arrow 2 NO_2 (g) 35 degrees C

Ammonium carbonate decomposes upon heating according to the balanced equation: \(\left(\mathrm{NH}_{4}\right) \mathrm{CO}_{3}(s) \rightarrow 2\ \mathrm{NH}_{3}(g)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) Calculate the total volume of gas produced at \(22^{\circ} \mathrm{C}\) and 1.02 atm by the complete decomposition of 11.83 g of ammonium carbonate. Equation Transcription: Text Transcription: (NH_4 )CO_3 (s) right arrow 2 NH_3 (g) + CO_2 (g) + H_2 O(g) 22 degrees C

Ammonium nitrate decomposes explosively upon heating according to the balanced equation: \(2\ \mathrm{NH}_{4} \mathrm{NO}_{3}(s) \rightarrow 2 \mathrm{~N}_{2}(g)+\mathrm{O}_{2}(g)+4\ \mathrm{H}_{2} \mathrm{O}(g)\) Calculate the total volume of gas (at \(25^{\circ} \mathrm{C}\) and 748 mm Hg) produced by the complete decomposition of 1.55 kg of ammonium nitrate. Equation Transcription: Text Transcription: 2 NH_4 NO_3 (s) right arrow 2 N_2 (g) + O_2 (g) + 4 H_2 O(g) 25 degrees C

A mixture containing 4.33 g of \(\mathrm{CO}_{2}\) and 3.11 g of \(\mathrm{CH}_{4}\) has a total pressure of 1.09 atm. What is the partial pressure of \(\mathrm{CO}_{2}\) in the mixture? Equation Transcription: Text Transcription: CO_2 CH_4

A mixture containing 235 mg of helium and 325 mg of neon has a total pressure of 453 torr. What is the partial pressure of helium in the mixture?

Consider the reaction: \(2\ \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2\ \mathrm{SO}_{3}(g)\) A reaction flask initially contains 0.10 atm of \({S O}_{2}\) and 0.10 atm of \({O}_{2}\). What is the total pressure in the flask once the limiting reactant is completely consumed? Assume a constant temperature and volume and a 100% reaction yield. Equation Transcription: Text Transcription: 2 SO_2 (g) + O_2 (g) right arrow 2 SO_3 (g)

Consider the reaction: \(\mathrm{CO}(g)+2\ \mathrm{H}_{2}(g) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(g)\) A reaction flask initially contains 112 torr of CO and 282 torr of \({H}_{2}\). The reaction is allowed to proceed until the pressure stops changing, at which point the total pressure is 196 torr. Determine the percent yield for the reaction. Assume a constant temperature and that no other reactions occur other than the one indicated. Equation Transcription: Text Transcription: CO(g)+2 H_2 (g) right arrow CH_3 OH(g)

Which gas sample has the greatest pressure? Assume they are all at the same temperature. Explain.

This image represents a sample of gas at a pressure of 1 atm, a volume of 1 L, and a temperature of \(25^{\circ} \mathrm{C}\). Draw a similar picture showing what happens if the volume is reduced to 0.5 L and the temperature is increased to \(250^{\circ} \mathrm{C}\). What happens to the pressure? Equation Transcription: 25°C 250°C Text Transcription: 25 Degree C 250 Degree C

Automobile air bag inflate following a serious impact. The impact triggers the chemical reaction: \(2 \mathrm{NaN}_{3}(s) \rightarrow 2 \mathrm{Na}(s)+3 \mathrm{~N}_{2}(g)\) If an automobile air bag has a volume of 11.8 L, how much \(\mathrm{NaN}_{3}\) in grams is required to fully inflate the air bag upon impact? Assume STP conditions. Equation Transcription: NaN3 Text Transcription: 2 NaN_3(s) rightarrow 2 Na(s) + 3 N_2(g) NaN_3

In a common classroom demonstration, a balloon is filled with air and submerged into liquid nitrogen. The balloon contracts as the gases within the balloon cool. Suppose the balloon initially contains 2.95 L of air at \(25.0^{\circ} \mathrm{C}\) and a pressure of 0.998 atm. Calculate the expected volume of the balloon upon cooling to \(-196^{\circ} \mathrm{C}\) (the boiling point of liquid nitrogen). When the demonstration is carried out, the actual volume of the balloon decreases to 0.61 L. How well does the observed volume of the balloon compare to your calculated value? Can you explain the difference? Equation Transcription: 25.0°C -196°C Text Transcription: 25.0 degree C -196 degree C

Olympic cyclists fill their tires with helium to make them lighter. Calculate the mass of air in an air-filled tire and the mass of helium in a helium-filled tire. What is the mass difference between the two? Assume that the volume of the tire is 855 mL, that it is filled with a total pressure of 125 psi, and that the temperature is \(25^{\circ} \mathrm{C}\). Also, assume an average molar mass for air of 28.8 g/mol. Equation Transcription: Text Transcription: 25 degrees C

PROBLEM 23P Convert each measurement to atm. (a) 1277 mm Hg (b) 2.38 × 105 Pa (c) 127 psi (d) 455 torr

PROBLEM 24P Convert each measurement to atm. (a) 921 torr (b) 4.8 × 104Pa (c) 87.5 psi (d) 34.22 in. Hg

PROBLEM 25P Perform each conversion. (a) 2.3 atm to torr (b) 4.7 × 10?2 atm to millimeters of mercury (c) 24.8 psi to millimeters of mercury (d) 32.84 in. Hg to tor

A sample of gas has a mass of 38.8 mg. Its volume is 224 mL at a temperature of \(55^{\circ} \mathrm{C}\) and a pressure of 886 torr. Find the molar mass of the gas. Equation Transcription: Text Transcription: 55 degrees C