6. When heated, carbon monoxide reacts with water to produce carbon dioxide and hydrogen CO(g) + H2O(g) CO2(g) + H2(g) + heat For each of the following changes at equilibrium, indicate whether the equilibrium shifts in the directions of the products, the reactants, or does not change: (a) decreasing the temperature (b) adding more H2(g) (c) removing some CO2(g) Concentration (d) adding more H2O(g) (e) decreasing the volume of the container

6. When heated, carbon monoxide reacts with water to produce carbon dioxide and hydrogen CO(g) + H2O(g) CO2(g) + H2(g) + heat For each of the following changes at equilibrium, indicate whether the equilibrium shifts in the directions of the products, the reactants, or does not change: (a) decreasing the temperature (b) adding more H2(g) (c) removing some CO2(g) Concentration (d) adding more H2O(g) (e) decreasing the volume of the container

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

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
1 (a) N₂(g) + O₂(g) 2NO (g) AH298 + 180 kJ mol-¹ From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (b) Increasing the pressure (c) Increasing the temperature (d) Increasing the concentration of N2 (e) Adding a catalyst
8) Consider the system below. When equilibrium is restored, how will the number of each type of molecule and the concentration of each substance compare to those before the stress was introduced? Complete the following table using the words "decrease," "same," or "increase." 2 NH,(g) = N,(g) + 3 H,(g) AH = 92.4 kJ/mol Decrease Volume Decrease Temperature N, Equilibrium Concentration Н, NH, N, Equilibrium Number Н, NH,
Write the equilibrium constant expression. Solid carbon and carbon dioxide gas react and form carbon monoxide: C(s) + CO₂(g) = 2CO(g)
Suppose a 500. mL flask is filled with 0.20 mol of Br,, 1.6 mol of OCl, and 1.9 mol of BrOCl. The following reaction becomes possible: 2' Br, (g) +OCl, (g)- BROCI(g)+BrC1(g) The equilibrium constantK for this reaction is 5.57 at the temperature of the flask. Calculate the equilibrium molarity of BrOCl. Round your answer to two decimal places. O M
Consider the following equilibrium for which H = 180.74: N2(g) + O2(g) 2 NO(g) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction?(a) NO(g) is added to the system. (b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%. (d) A catalyst is added to the reaction mixture. (e) The total pressure of the system is increased by adding a noble gas. (f) O2(g) is removed from the system.
Nitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no change
Consider the following exothermic reaction system at equilibrium: N2(g) + 3H2(g) ⇒ 2NH3(g) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below: Note: Use I for increase, D for decrease, NC for no change Add N2(g) Remove H2(g) Add NH3(9) Add Ne(g) Increase the temperature (constant P) Decrease the volume (constant T) Add a catalyst Submit NH3 N₂ H2