7. Gases

Gas Stoichiometry

7. Gases

Gas Stoichiometry

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Gas Stoichiometry Example 1

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Step by Step Gas Stoichiometry - Final Exam Review

14:56

Step by Step Gas Stoichiometry - Final Exam Review

Gas Stoichiometry: Equations Part 1

STP Gas Chemistry (Standard Temperature and Pressure) Examples Practice Problems Questions Shortcut

Gas Stoichiometry for Gases at STP

Guillotined Chemistry

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Molar Gas Volume: Stoichiometry With Gases

05:10

Molar Gas Volume: Stoichiometry With Gases

Professor Dave Explains

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Practice this topic

Multiple Choice

The metabolic breakdown of glucose (C₆H₁₂O₆) (MW:180.156 g/mol) is given by the following equation:

C₆H₁₂O₆ (s) + 6 O₂ (g) → 6 CO₂ (g) + 6 H₂O (l)

Calculate the volume (in mL) of CO₂ produced at 34°C and 1728.9 torr when 231.88 g glucose is used up in the reaction.

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Multiple Choice

The oxidation of phosphorus can be represented by the following equation:

P₄ (s) + 5 O₂ (g) → 2 P₂O₅ (g)

If 1.85 L of diphosphorus pentoxide form at a temperature of 50.0 ºC and 1.12 atm, what is the mass (in g) of phosphorus that reacted?

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Multiple Choice

Determine the mass (in grams) of water formed when 15.3 L NH3 (at 298 K and 1.50 atm) is reacted with 21.7 L of O2 (at 323 K and 1.1 atm).

4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)

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Textbook Question

Magnesium can be used as a 'getter' in evacuated enclosures to react with the last traces of oxygen. (The magnesium is usually heated by passing an electric current through a wire or ribbon of the metal.) If an enclosure of 5.67 L has a partial pressure of O2 of 7.066 mPa at 30 °C, what mass of magnesium will react according to the following equation? 2 Mg1s2 + O21g2¡2 MgO1s2

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Textbook Question

Calcium hydride, CaH2, reacts with water to form hydrogen gas: CaH21s2 + 2 H2O1l2¡Ca1OH221aq2 + 2 H21g2 This reaction is sometimes used to inflate life rafts, weather balloons, and the like, when a simple, compact means of generating H2 is desired. How many grams of CaH2 are needed to generate 145 L of H2 gas if the pressure of H2 is 110 kPa at 21 °C?

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Textbook Question

Both Jacques Charles and Joseph Louis Guy-Lussac were avid balloonists. In his original flight in 1783, Jacques Charles used a balloon that contained approximately 31,150 L of H2. He generated the H2 using the reaction between iron and hydrochloric acid: Fe1s2 + 2 HCl1aq2 ¡ FeCl21aq2 + H21g2 How many kilograms of iron were needed to produce this volume of H2 if the temperature was 22 °C?

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Textbook Question

Acetylene gas, C2H21g2, can be prepared by the reaction of calcium carbide with water: CaC21s2 + 2 H2O1l2¡Ca1OH221aq2 + C2H21g2 Calculate the volume of C2H2 that is collected over water at 23 °C by reaction of 1.524 g of CaC2 if the total pressure of the gas is 100.4 kPa. (The vapor pressure of water is tabulated in Appendix B.)

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Textbook Question

The hydrogen gas formed in a chemical reaction is collected over water at 30.0 °C at a total pressure of 732 mmHg. What is the partial pressure of the hydrogen gas collected in this way? If the total volume of gas collected is 722 mL, what mass of hydrogen gas is collected?

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Textbook Question

The air in a bicycle tire is bubbled through water and collected at 25 °C. If the total volume of gas collected is 5.45 L at a temperature of 25 °C and a pressure of 745 torr, how many moles of gas were in the bicycle tire?

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Textbook Question

The zinc in a copper-plated penny will dissolve in hydrochloric acid if the copper coating is filed down in several spots (so that the hydrochloric acid can get to the zinc). The reaction between the acid and the zinc is 2 H+ (aq) + Zn(s)¡ H2( g) + Zn2 + (aq). When the zinc in a certain penny dissolves, the total volume of gas collected over water at 25 °C is 0.951 L at a total pressure of 748 mmHg. What mass of hydrogen gas is collected?

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Textbook Question

Consider the chemical reaction: C(s) + H2O( g)¡CO( g) + H2( g) How many liters of hydrogen gas are formed from the complete reaction of 15.7 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 355 K.

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Textbook Question

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn1s2 + 2 HCl1aq2¡ZnCl21aq2 + H21g2 (a) How many liters of H2 would be formed at 742 mm Hg and 15 °C if 25.5 g of zinc was allowed to react?

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Textbook Question

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn1s2 + 2 HCl1aq2¡ZnCl21aq2 + H21g2 (b) How many grams of zinc would you start with if you wanted to prepare 5.00 L of H2 at 350 mm Hg and 30.0 °C?

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Textbook Question

Consider the chemical reaction: 2 H2O(l )¡2 H2( g) + O2( g) What mass of H2O is required to form 1.4 L of O2 at a temperature of 315 K and a pressure of 0.957 atm?

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Textbook Question

CH3OH can be synthesized by the reaction: CO( g) + 2 H2( g)¡CH3OH( g) What volume of H2 gas (in L), at 748 mmHg and 86 °C, is required to synthesize 25.8 g CH3OH? How many liters of CO gas, measured under the same conditions, are required?

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Textbook Question

Ammonium nitrate can decompose explosively when heated according to the equation 2 NH4NO31s2¡2 N21g2 + 4 H2O1g2 + O21g2 How many liters of gas would be formed at 450 °C and 1.00 atm pressure by explosion of 450 g of NH4NO3?

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Textbook Question

Oxygen gas reacts with powdered aluminum according to the reaction: 4 Al(s) + 3 O2( g)¡2 Al2O3(s) What volume of O2 gas (in L), measured at 782 mmHg and 25 °C, completely reacts with 53.2 g Al?

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Textbook Question

Titanium(III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl4 vapor with H2: 2 TiCl41g2 + H21g2¡2 TiCl31s2 + 2 HCl1g2 (a) How many grams of TiCl4 are needed for complete reaction with 155 L of H2 at 435 °C and 795 mm Hg pressure?

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Textbook Question

Assume that you have 1.00 g of nitroglycerin in a 500.0-mL steel container at 20.0 °C and 1.00 atm pressure. An explosion occurs, raising the temperature of the container and its contents to 425 °C. The balanced equation is 4 C3H5N3O91l2¡ 12 CO21g2 + 10 H2O1g2 + 6 N21g2 + O21g2 (c) What is the pressure in atmospheres inside the container after the explosion according to the ideal gas law?

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Textbook Question

Ozone is depleted in the stratosphere by chlorine from CF3Cl according to this set of equations: CF3Cl + UV light¡CF3 + Cl Cl + O3¡ClO + O2 O3 + UV light¡O2 + O ClO + O¡Cl + O2 What total volume of ozone at a pressure of 25.0 mmHg and a temperature of 225 K is destroyed when all of the chlorine from 15.0 g of CF3 Cl goes through 10 cycles of the given reactions?

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Textbook Question

Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2( g) + 3 F2( g)¡2 ClF3( g) A 2.00-L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 729 mmHg. Identify the limiting reactant. Determine the theoretical yield of ClF3 in grams.

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Textbook Question

Carbon monoxide gas reacts with hydrogen gas to form methanol. CO( g) + 2 H2( g)¡CH3OH( g) A 1.50-L reaction vessel, initially at 305 K, contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 397 mmHg. Identify the limiting reactant. Determine the theoretical yield of methanol in grams.

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Textbook Question

A sample of magnesium metal reacts with aqueous HCl to yield H2 gas: Mg1s2 + 2 HCl1aq2¡MgCl21aq2 + H21g2 The gas that forms is found to have a volume of 3.557 L at 25 °C and a pressure of 747 mm Hg. Assuming that the gas is saturated with water vapor at a partial pressure of 23.8 mm Hg, what is the partial pressure in millimeters of mercury of the H2? How many grams of magnesium metal were used in the reaction?

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Textbook Question

Chlorine gas was first prepared in 1774 by the oxidation of NaCl with MnO2: 2 NaCl1s2 + 2 H2SO41l2 + MnO21s2¡ Na2SO41s2 + MnSO41s2 + 2 H2O1g2 + Cl21g2 Assume that the gas produced is saturated with water vapor at a partial pressure of 28.7 mm Hg and that it has a volume of 0.597 L at 27 °C and 755 mm Hg pressure. (b) How many grams of NaCl were used in the experiment, assuming complete reaction?

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Textbook Question

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Textbook Question

Gaseous compound Q contains only xenon and oxygen. When 0.100 g of Q is placed in a 50.0-mL steel vessel at 0 °C the pressure is 0.229 atm. (b) When the vessel and its contents are warmed to 100 °C, Q decomposes into its constituent elements. What is the total pressure, and what are the partial pressures of xenon and oxygen in the container?

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Textbook Question

Modern pennies are composed of zinc coated with copper. A student determines the mass of a penny to be 2.482 g and then makes several scratches in the copper coating (to expose the underlying zinc). The student puts the scratched penny in hydrochloric acid, where the following reaction occurs between the zinc and the HCl (the copper remains undissolved): Zn(s) + 2 HCl(aq)¡ H2( g) + ZnCl2(aq) The student collects the hydrogen produced over water at 25 °C. The collected gas occupies a volume of 0.899 L at a total pressure of 791 mmHg. Calculate the percent zinc (by mass) in the penny. (Assume that all the Zn in the penny dissolves.)

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Textbook Question

Consider the reaction: 2 Ag2O(s)¡4 Ag(s) + O2( g) If this reaction produces 15.8 g of Ag(s), what total volume of gas can be collected over water at a temperature of 25 °C and a total pressure of 752 mmHg?

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Textbook Question

Ammonium carbonate decomposes upon heating according to the balanced equation: (NH4)2CO3(s)¡ 2 NH3( g) + CO2( g) + H2O( g) Calculate the total volume of gas produced at 22 °C and 1.02 atm by the complete decomposition of 11.83 g of ammonium carbonate.

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Textbook Question

Assume that a single cylinder of an automobile engine has a volume of 524 cm3. (a) If the cylinder is full of air at 74 C and 99.3 kPa, how many moles of O2 are present? (The mole fraction of O2 in dry air is 0.2095.) (b) How many grams of C8H18 could be combusted by this quantity of O2, assuming complete combustion with formation of CO2 and H2O?

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Textbook Question

Ammonium nitrate decomposes explosively upon heating according to the balanced equation: 2 NH4NO3(s)¡2 N2( g) + O2( g) + 4 H2O( g) Calculate the total volume of gas (at 125 °C and 748 mmHg) produced by the complete decomposition of 1.55 kg of ammonium nitrate.

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Textbook Question

Assume that an exhaled breath of air consists of 74.8% N2, 15.3% O2, 3.7% CO2, and 6.2% water vapor. (c) How many grams of glucose 1C6H12O62 would need to be metabolized to produce this quantity of CO2? (The chemical reaction is the same as that for combustion of C6H12O6. See Section 3.2 and Problem 10.57.)

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Textbook Question

A catalytic converter in an automobile uses a palladium or platinum catalyst (a substance that increases the rate of a reaction without being consumed by the reaction) to convert carbon monoxide gas to carbon dioxide according to the reaction: 2 CO( g) + O2( g)¡2 CO2( g) A chemist researching the effectiveness of a new catalyst combines a 2.0:1.0 mole ratio mixture of carbon monoxide and oxygen gas (respectively) over the catalyst in a 2.45-L flask at a total pressure of 745 torr and a temperature of 552 °C. When the reaction is complete, the pressure in the flask has dropped to 552 torr. What percentage of the carbon monoxide was converted to carbon dioxide?

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Textbook Question

A mixture of CO(g) and O2(g) in a 1.0-L container at 1.0 * 103 K has a total pressure of 2.2 atm. After some time, the total pressure falls to 1.9 atm as the result of the formation of CO2. Determine the mass (in grams) of CO2 that forms.

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Textbook Question

Baking soda (sodium bicarbonate, NaHCO3) reacts with acids in foods to form carbonic acid 1H2CO32, which in turn decomposes to water and carbon dioxide gas. In a cake batter, the CO21g2 forms bubbles and causes the cake to rise. (c) If 1/2 teaspoon of baking soda is indeed completely neutralized by the lactic acid in sour milk, calculate the volume of carbon dioxide gas that would be produced at 1 atm pressure, in an oven set to 350 F.

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Textbook Question

A 4.00-g sample of a mixture of CaO and BaO is placed in a 1.00-L vessel containing CO2 gas at a pressure of 97.33 kPa and a temperature of 25 °C. The CO2 reacts with the CaO and BaO, forming CaCO3 and BaCO3. When the reaction is complete, the pressure of the remaining CO2 is 20.0 kPa. (b) Calculate the mass percentage of CaO in the mixture.

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Textbook Question

Ammonia and hydrogen chloride react to form solid ammonium chloride: NH₃(g) + HCl(g) → NH₄Cl(s)

Two 2.00-L flasks at 25 °C are connected by a valve, as shown in the drawing. One flask contains 5.00 g of NH₃(g), and the other contains 5.00 g of HCl(g). When the valve is opened, the gases react until one is completely consumed. (b) What will be the final pressure of the system after the reaction is complete? (Neglect the volume of the ammonium chloride formed.)

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Textbook Question

Binary compounds of alkali metals and hydrogen react with water to liberate H2( g). The H2 from the reaction of a sample of NaH with an excess of water fills a volume of 0.490 L above the water. The temperature of the gas is 35 °C and the total pressure is 758 mmHg. Determine the mass of H2 liberated and the mass of NaH that reacted.

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Textbook Question

Natural gas is very abundant in many Middle Eastern oil fields. However, the costs of shipping the gas to markets in other parts of the world are high because it is necessary to liquefy the gas, which is mainly methane and has a boiling point at atmospheric pressure of -164 °C. One possible strategy is to oxidize the methane to methanol, CH3OH, which has a boiling point of 65 °C and can therefore be shipped more readily. Suppose that 3.03 * 108 m3 of methane at atmospheric pressure and 25 °C is oxidized to methanol. What volume of methanol is formed if the density of CH3OH is 0.791 g>mL?

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