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Consider the following equilibria:   Equilibrium I: H2O(g) + C(s)                                     H2(g) + CO(g);             ΔH = +131 kJ mol-1 2-   (   Equilibrium II: Cr2O4- aq)  + 2H+(aq)                                    Cr2O7   (aq)  + H2O(l)     Use Le Chatelier’s principle to predict and explain the effect of:   increasing the pressure on Equilibrium I. increasing the temperature on Equilibrium I. increasing [H+] on Equilibrium II. the presence of a catalyst on Equilibrium II.

Consider the following equilibria:   Equilibrium I: H2O(g) + C(s)                                     H2(g) + CO(g);             ΔH = +131 kJ mol-1 2-   (   Equilibrium II: Cr2O4- aq)  + 2H+(aq)                                    Cr2O7   (aq)  + H2O(l)     Use Le Chatelier’s principle to predict and explain the effect of:   increasing the pressure on Equilibrium I. increasing the temperature on Equilibrium I. increasing [H+] on Equilibrium II. the presence of a catalyst on Equilibrium II.

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 12ALQ: In Section 17.3 of your text, it is mentioned that equilibrium is reached in a closed system. What...
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  1. Consider the following equilibria:

 

Equilibrium I: H2O(g) + C(s)                                     H2(g) + CO(g);             ΔH = +131 kJ mol-1

2-

 

(
 

Equilibrium II: Cr2O4- aq)  + 2H+(aq)                                    Cr2O7

 

(aq)  + H2O(l)

 

 

Use Le Chatelier’s principle to predict and explain the effect of:

 

  1. increasing the pressure on Equilibrium I.
  2. increasing the temperature on Equilibrium I.
  • increasing [H+] on Equilibrium II.
  1. the presence of a catalyst on Equilibrium II.
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