Given the equilibrium CH4(g) + H₂O(g) ⇒ CO(g) + 3H₂(g) AH= +205 kJ mol-1 a) If the pressure applied to the equilibrium is increased what would be the effect on the amount hydrogen produced? b) If the concentration of steam (H2O (g)) is increased what would be the effect on the amount of hydrogen produced?

Given the equilibrium CH4(g) + H₂O(g) ⇒ CO(g) + 3H₂(g) AH= +205 kJ mol-1 a) If the pressure applied to the equilibrium is increased what would be the effect on the amount hydrogen produced? b) If the concentration of steam (H2O (g)) is increased what would be the effect on the amount of hydrogen produced?

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

Br2(g) + Cl2(g) 2BRCI(g) the equilibrium concentrations were found to be [Br,) - 3.5 x 103 M, [CI,] = 1.2 x 10 2 M, and [BrCl] = 1.4 x 10 2 M. Write the equilibrium expression, and calculate the equilibrium constant for this reaction at this temperature. K = < Prev 9 of 27 Nex
The reaction quotient for a system is 3.9 x 103. If the equilibrium constant for the system is 2 x 10-4, what will happen as the reaction mixture approaches equilibrium? O a) There will be a net gain in reactant(s). O b) There will be a net gain in product(s). O C) The equilibrium constant will increase until it equals the reaction quotient. O a) The equilibrium constant will decrease until it equals the reaction quotient. e) There will be a net gain in both product(s) and reactant(s).
Write the equilibrium expressions 6H20(g) + 6C02(g) C6H1206(s) + 602(g)
Methanol liquid burns readily in air. One way to represent this equilibrium is: 2 CH3ОН(1) + 3 02(9)+ 2 CO2(g) + 4 H20(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) CНH3ОН(1) + 3/2 02(9)+ =cO2(g) + 2 H20(g) K1 = %D 2) 2 CO2(9) + 4 H20(g) 2 CH3ОН (1) + 3 02(9) K2 = 3) СO2(g) + 2 H20(g) еснзон (1) + 3/2 02(g) K3 : %3D Drag and drop your selection from the following list to complete the answer: к1/2 1/K (1/K)!/2
Suppose a 250. mL flask is filled with 1.8 mol of CO, 0.20 mol of H2O and 1.0 mol of H2. The following reaction becomes possible: CO(g)+H,O()-CO,(z)+H.() The equilibrium constant K for this reaction is 2.64 at the temperature of the flask. Calculate the equilibrium molarity of H2O. Round your answer to two decimal places. Ом 5
Suppose a 250. mL flask is filled with 1.9 mol of Br,, 1.8 mol of BrOCl and 1.6 mol of BrCl. The following reaction becomes possible: Br, (g) + OC1, (g) = BIOC1(g) + BrC1(g) The equilibrium constant K for this reaction is 4.15 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. 0.53 M ?
Suppose a 500. mL flask is filled with 1.1 mol of NO2, 1.7 mol of NO and 0.90 mol of CO2. The following reaction becomes possible: NO, (g)+CO(g) NO(g) +CO,(s) The equilibrium constant K for this reaction is 0.292 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. м B C ol
Suppose a 250. mL flask is filled with 0.10 mol of Br,, 1.7 mol of OC1, and 0.20 mol of BrCl. The following reaction becomes possible: Br, (g) + OC1,(g) -BROC1 (g) + BrCl (g) The equilibrium constant K for this reaction is 0.343 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. | M
A 0.066 mol sample of formaldehyde vapor, CH₂O, was placed in a heated 500 mL vessel and some of it decomposed. The reaction is CH,O(g) = At equilibrium, the CH₂O(g) concentration was 0.060 mol L-¹. Calculate the value of Kc for this reaction? Kc = H₂(g) H2(g) + CO(g) i
1. Consider the following equilibrium for which AH < 0 2SO2(g) + O2(g) =2SO3(g) How will each of the following changes affect an equilibrium mixture of the three gases. (a) 02 (g) is added to the system. (b) the reaction mixture is heated. (c) the volume of the reaction vessel is doubled (d) a catalyst is added to the mixture. (e) the total pressure of the system is increased by adding a noble gas. (f) SO:(g)is removed from the system?
Please answer with the correct number of significant digits. At a certain temperature, the equilibrium constant K for the following reaction is 9.7 x 10¹¹: NO₂(g) + CO(g) NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 42. L reaction vessel is filled with 1.2 mol of NO₂ and 1.2 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. NO(g) + CO₂(9) 1 NO₂(9)+CO (9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 2 NO₂(9)+2CO(g) 1 2 NO(g) +2C0₂(9) There will be very little NO₂ and CO. There will be very little NO and CO₂. Neither of the above is true. K-O K-0 X
A student ran the following reaction in the laboratory at 600 K: CO(g) + Cl₂(g) —COCI₂(g) When he introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 2.09 atm and the initial partial pressure of Cl₂ was 1.22 atm, he found that the equilibrium partial pressure of Cl₂ was 0.405 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр