Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S₂(g) + C(s) CS₂ (g) How many grams of CS₂ (g) can be prepared by heating 11.5 mol S₂ (g) with excess carbon in a 5.60 L reaction vessel held at 900 K until equilibrium is attained? Ke = 9.40 at 900 K

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S₂(g) + C(s) CS₂ (g) How many grams of CS₂ (g) can be prepared by heating 11.5 mol S₂ (g) with excess carbon in a 5.60 L reaction vessel held at 900 K until equilibrium is attained? Ke = 9.40 at 900 K

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

At a certain temperature, 0.3011 mol of N2N2 and 1.501 mol of H2H2 are placed in a 2.50 L container. N2(g)+3H2(g)↽−−⇀2NH3(g)N2(g) At equilibrium, 0.1201 mol of N2 is present. Calculate the equilibrium constant, Kc.
Suppose a 500. mL flask is filled with 0.70 mol of NO2, 1.7 mol of CO and 0.30 mol of NO. The following reaction becomes possible: NO₂(g) + CO (g) → NO(g) + CO₂(g) The equilibrium constant K for this reaction is 8.94 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. ☐M X Ś
At a certain temperature, the equilibrium constant, ?c,Kc, is 6.12×10−36.12×10−3 for the reaction Cl2(g)↽−−⇀2Cl(g)Cl2(g)↽−−⇀2Cl(g) A. If 2.69 g2.69 g Cl2Cl2 is placed in a 2.00 L2.00 L flask at this temperature, what are the equilibrium concentrations of Cl2Cl2 and Cl?
Suppose a 500. mL flask is filled with 1.0 mol of CO, 1.8 mol of CO2 and 0.90 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.932 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places. ☐M X 5
Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "Nox") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 75 L tank with 23. mol of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 17.9 mol of nitrogen dioxide gas. The engineer then adds another 7.7 mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits.
Suppose a 500. mL flask is filled with 0.80 mol of NO and 1.8 mol of NO2. The following reaction becomes possible: NO3(g) + NO(g) - 2NO2(g) The equilibrium constant K for this reaction is 4.37 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 1.0 mol of Br2, 0.40 mol of OC12 and 1.7 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOCI (g) + BrC1 (g) The equilibrium constant K for this reaction is 0.681 at the temperature of the flask. Calculate the equilibrium molarity of OC12. Round your answer to two decimal places. M X
Steam reforming of methane ( CH, ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 2.0 L flask with 3.8 atm of methane gas and 2.0 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 3.0 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K, 0 x10 ?
Suppose a 250. mL flask is filled with 0.80 mol of O2 and 0.30 mol of SO3. This reaction becomes possible: 2SO2(g) + O2(g) ~ 2SO3(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use r to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity.
Suppose a 250. mL flask is filled with 1.4 mol of H₂ and 0.30 mol of HI. This reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H₂. You can leave out the M symbol for molarity. initial change equilibrium H₂ 0 X 0 1₂ 0 0 0 HI 0 0 0 010 X Ś
Suppose a 250. mL flask is filled with 0.60 mol of Br₂, 1.9 mol of BrOCI and 1.3 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrC1 (g) The equilibrium constant K for this reaction is 1.98 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 1.5 mol of CO, 0.50 mol of H₂O and 1.2 mol of CO₂. The following reaction becomes possible: CO(g) +H₂O(g) CO₂(g) +H₂(g) The equilibrium constant K for this reaction is 0.503 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M ܢܢ X E 00 Ar