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Ch.10 - Gases
All textbooksBrown 14th EditionCh.10 - GasesProblem 124
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Chapter 10, Problem 124

Chlorine dioxide gas (ClO2) is used as a commercial bleaching agent. It bleaches materials by oxidizing them. In the course of these reactions, the ClO2 is itself reduced. One method of preparing ClO2 is by the reaction of chlorine and sodium chlorite: Cl2(g) + 2 NaClO2(s) → 2 ClO2(g) + 2 NaCl(s). If you allow 15.0 g of NaClO2 to react with 2.00 L of chlorine gas at a pressure of 152.0 kPa at 21°C, how many grams of ClO2 can be prepared?

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1
Step 1: Calculate the moles of NaClO2 using its molar mass. The molar mass of NaClO2 is the sum of the atomic masses of sodium (Na), chlorine (Cl), and two oxygen (O) atoms. Use the formula: moles = mass / molar mass.
Step 2: Use the ideal gas law to calculate the moles of Cl2 gas. The ideal gas law is given by PV = nRT, where P is pressure, V is volume, n is moles, R is the ideal gas constant, and T is temperature in Kelvin. Convert the temperature from Celsius to Kelvin and solve for n (moles of Cl2).
Step 3: Determine the limiting reactant by comparing the mole ratio of NaClO2 to Cl2 from the balanced chemical equation. The balanced equation shows that 1 mole of Cl2 reacts with 2 moles of NaClO2. Calculate the theoretical moles of ClO2 produced from each reactant and identify the limiting reactant.
Step 4: Calculate the moles of ClO2 produced using the limiting reactant. Use the stoichiometry of the balanced equation, which shows that 2 moles of NaClO2 produce 2 moles of ClO2.
Step 5: Convert the moles of ClO2 to grams using its molar mass. The molar mass of ClO2 is the sum of the atomic masses of chlorine (Cl) and two oxygen (O) atoms. Use the formula: mass = moles * molar mass.
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Textbook Question

Ammonia and hydrogen chloride react to form solid ammonium chloride: NH31g2 + HCl1g2¡NH4Cl1s2 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 NH31g2, and the other contains 5.00 g of HCl(g). When the valve is opened, the gases react until one is completely consumed. (a) Which gas will remain in the system after the reaction is complete?

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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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Open Question
Gas pipelines are used to deliver natural gas (methane, CH4) to the various regions of the United States. The total volume of natural gas that is delivered is on the order of 2.7 * 10^12 L per day, measured at STP. Calculate the total enthalpy change for the combustion of this quantity of methane. (Note: Less than this amount of methane is actually combusted daily. Some of the delivered gas is passed through to other regions.)
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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Textbook Question

Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I21s2 + 5 F21g2¡2 IF51g2 A 5.00-L flask containing 10.0 g of I2 is charged with 10.0 g of F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (a) What is the partial pressure of IF5 in the flask?

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Textbook Question

Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I21s2 + 5 F21g2¡2 IF51g2 A 5.00-L flask containing 10.0 g of I2 is charged with 10.0 g of F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (c) Draw the Lewis structure of IF5.

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