Elemental sulfur can be recovered from gaseous hydrogen sulfide (H2S) through the following reaction: 2 H,S(g) + SO2(g) → 3 S(s) + 2 H,O(€) (a) What volume of H,S (in liters at 0°C and 1.00 atm) is required to produce 2.00 kg (2000 g) sulfur by this process? (b) What minimum mass and volume (at 0°C and 1.00 atm) of SO2 are required to produce 2.00 kg sulfur by this reaction?

Elemental sulfur can be recovered from gaseous hydrogen sulfide (H2S) through the following reaction: 2 H,S(g) + SO2(g) → 3 S(s) + 2 H,O(€) (a) What volume of H,S (in liters at 0°C and 1.00 atm) is required to produce 2.00 kg (2000 g) sulfur by this process? (b) What minimum mass and volume (at 0°C and 1.00 atm) of SO2 are required to produce 2.00 kg sulfur by this reaction?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

(b) If a 2.302g sample of impure cobalt(III) carbonate is heated, and 415mL of carbon dioxide is collected at 23°C and a pressure of 1.512atm, what is the percent cobalt(III) carbonate in the sample? (b) If a 2.302 g sample of impure cobalt(III) carbonate is heated, and 415 mL of carbon dioxide is collected at 23°C and a pressure of 1.512 atm, what is the percent. cobalt(III) carbonate in the sample?
The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) (a) what volume of O2 at 798 mmHg and 41 degrees C is required to synthesize 23.0 mol of NO? (b) what volume of H2O (g) is produced by the reaction under the same conditions?
An “empty" spray can contains residual propellant gas that has a pressure of 772 torr at 23°C. The can is then heated to 475 °C. (a) What is the gas pressure in the hot can if the volume remains constant? (b) What is the gas pressure in the hot can if the can slightly expands during heating and its volume increases by 6.50%?
The partial pressure of water vapor in saturated air at 34 °C is 5.25×10-2 atm. (a) How many molecules of water are in 1.16 cm3 of saturated air at 34 °C? (b) What volume of saturated air at 34 °C contains 0.563 mol of water?
Refer to the following equation: Mg (s) + 2HNO3(aq) -> Mg(NO3)2 (aq) + H2 (g) A reaction between 0.359 grams of Mg and 21.12mL of a 0.450M HNO3 solution was conducted in a room witht he following conditions: 27.5 degrees Celius, 723mmHg of atospheric pressure. If .15mL of H2 were collected over water (by the water displacement method), calculate the percent yeild of the reaction. (Pressure H2O at 27.5 degrees Celius = 27.82 mmHg)
A flask of volume 0.753 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.8 degrees C What mass of sodium, in grams, is required to completely react with the chlorine to make sodium chloride? 2 Na (s) + Cl (g) - - > 2 Na C1 (s)
6. A quantity of solid sodium peroxide is reacted with excess water. The products of the reaction are aqueous sodium hydroxide and oxygen gas. (a) If 65.0 mL of oxygen gas at STP and 150.0 mL of sodium hydroxide solution resulted from the reaction, what is the molarity of the sodium hydroxide? (b) How many grams of sodium peroxide were used in problem 6(a)? (c) What would be the answer to question 6(a) if 84.5 mL of oxygen gas was collected at 35°C and 745 torr?
0.300 mol of O2 gas is held at an a 5.00 L container at 45.0 °C. Determine the following:(a) the volume this gas occupies at ST (in L).(b) the pressure of this gas if the temperature isincreased to 60.0 °C assuming the volume does notchange.(c) the volume of NO2 (in L) expected from complete combustion of the excess N2 in O at STP.Hint: Use answer from (a) as a starting point.
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.
The effusion rate of a gaseous compound at a certain temperature and pressure is 25.0 mL/min. Under the same conditions, the diffusion rate of N, is 57.1 mL/min. (a) Calculate the molar mass of the unknown compound. (b) If the compound is composed of 21.95% S and 78.05% F, by mass, what is the empirical formula of the compound?