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9. If the reaction in Question #8 is endothermic, what happens when the following changes are made to the system? (State your answers as a shift, choose: to Product, to Reactants, No Change) a) Temperature increased. b) Temperature decreased. c) H2S concentration increased. d) H2 concentration increased. e) A catalyst is added.

9. If the reaction in Question #8 is endothermic, what happens when the following changes are made to the system? (State your answers as a shift, choose: to Product, to Reactants, No Change) a) Temperature increased. b) Temperature decreased. c) H2S concentration increased. d) H2 concentration increased. e) A catalyst is added.

Chemistry
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...
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#9 a-d

7. Using what you learned in Question #6, find K for both of the previou: reactions using the concentrations given below: a) [N2O3] = 2.1x10-6 M, [N0] = 0.076 M, [NO2] = 5.8x10-3 M b) [Co2+] = 0.82 M, [CI ] = 0.88 M, [CoCl4²-] = 0.50 M 8. At high temperatures (in this case 800°C), hydrogen sulfide exists in an equilibrium with hydrogen gas and disulfur (S2 molecules, instead of the normal S8 rings found in the solid): 2 H2S(g) = 2 H2(g) + S2(g) If the equilibrium constant is K = 1.7×10-7, and the equilibrium concentrations are [H2S] = 1.0 M, and [H2] = 4.9×10-3 M, what is the concentration of disulfur (S2)? 9. If the reaction in Question #8 is endothermic, what happens when the following changes are made to the system? (State your answers as a shift, choose: to Product, to Reactants, No Change) a) Temperature increased. b) Temperature decreased. c) H2S concentration increased. d) H2 concentration increased. e) A catalyst is added. 10. Write the formula for sodium chloride, without making any mistakes.
Transcribed Image Text:7. Using what you learned in Question #6, find K for both of the previou: reactions using the concentrations given below: a) [N2O3] = 2.1x10-6 M, [N0] = 0.076 M, [NO2] = 5.8x10-3 M b) [Co2+] = 0.82 M, [CI ] = 0.88 M, [CoCl4²-] = 0.50 M 8. At high temperatures (in this case 800°C), hydrogen sulfide exists in an equilibrium with hydrogen gas and disulfur (S2 molecules, instead of the normal S8 rings found in the solid): 2 H2S(g) = 2 H2(g) + S2(g) If the equilibrium constant is K = 1.7×10-7, and the equilibrium concentrations are [H2S] = 1.0 M, and [H2] = 4.9×10-3 M, what is the concentration of disulfur (S2)? 9. If the reaction in Question #8 is endothermic, what happens when the following changes are made to the system? (State your answers as a shift, choose: to Product, to Reactants, No Change) a) Temperature increased. b) Temperature decreased. c) H2S concentration increased. d) H2 concentration increased. e) A catalyst is added. 10. Write the formula for sodium chloride, without making any mistakes.
Expert Solution
Step 1

At equilibrium all the observable factors such as pressure, concentration, etc. remains constant. Hence if we change these factors at this stage, system will shift it's direction in order to nullify that particular effect. 

Here the reaction is as follows.

2H2Sg⇔2H2g+S2g

This is endothermic.

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