6. The following exothermic reaction is allowed to reach equilibrium.2H2 (g) + O2(g) = 2H;O(g)What happens to the reaction when the temperature is decreased?A. Favors forward reactionB. Favors reverse reactionC. The reaction is still at equilibrium7. The following reaction is allowed to reach equilibrium.N2(g) + O2(g) = 2NO(g)What happens to the reaction when more NO(g) is added?A. Favors forward reactionB. Favors reverse reactionC. The reaction is still at equilibrium8. The following reaction is allowed to reach equilibrium.3H2 (g) + N2(g) = 2NH3(g)What happens to the reaction when the volume of the reaction vessel is decreased?A. Favors forward reactionB. Favors reverse reactionC. The reaction is still at equilibrium9. The following exothermic reaction is allowed to reach equilibrium.2H2(g) + O2(g) = 2H2O(g)What happens to the reaction when the temperature is increased?A. Favors forward reactionB. Favors reverse reactionC. The reaction is still at equilibrium

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6. The following exothermic reaction is allowed to reach equilibrium. 2H2 (g) + O2(g) = 2H2O(g) What happens to the reaction when the temperature is decreased? A. Favors forward reaction B. Favors reverse reaction C. The reaction is still at equilibrium

6. The following exothermic reaction is allowed to reach equilibrium. 2H2 (g) + O2(g) = 2H2O(g) What happens to the reaction when the temperature is decreased? A. Favors forward reaction B. Favors reverse reaction C. The reaction is still at equilibrium

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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4. A. An important reaction in the commercial production of hydrogen is CO(g) + H2O(g) --><-- H2(g) + CO2(g) How will the system at equilibrium shift in each of the five following cases? (Use arrows or write "right" , "left" , or "no shift"). a. Gaseous carbon monoxide is removed b. In rigid reaction container, a catalyst is added. c. The temperature is decreased (the reaction is exothermic). d. The reaction container volume is doubled. e. Hydrogen gas is added. B. The equation above has a Kc value of 7.5 x 102. If 2.0 moles of each reactant and product are put into the same sealed 4.0 L container, determine the concentrations of all species present at equilibrium. Please answer A with sub parts and B.
Consider the following exothermic reaction: C (s) + 2 Cl2 (g) ⇋⇋ CCl4 (g) How would the equilibrium shift if the reaction mixture is heated? Select one: a. The reaction would shift towards the products. b. The reaction would shift towards the reactants. c. The equilibrium would not be affected.
The chemical equation represents a reversible reaction. 3H2(9) + N2(9) # 2NH3(g) At equilibrium, 1 liter of a mixture of gases at 450°C contains 1.83 mol of hydrogen (H2), 0.793 mol of nitrogen (N2), and 1.72 mol of ammonia (NH3).What is the equilibrium constant for the reaction under these conditions? O A. 0.718 B. 0.609 O C. 1.39 O D. 0.159 96 5 6
Which reaction, when at equilibrium, would be unaffected by a change in pressure? A. N2(g) + O2 (g) = 2NO(g) B. 2CO(g) + O2 = 2CO2(g) C. COBr2(g) = CO(g) + Br2(g) D. N2O4(g) = 2NO2 (g)
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Choose the equilibrium expression for the following reaction. a. CH4 (9) + 2H₂S(9) ⇒ CS₂ (9) + 4H₂ (9) OK: = K= OK= K= b. 4NH3(g) + 5O2(g) — 4NO(g) + 6H₂O(g) [NO] 4 [H₂0]6 [NH,][0₂]5 [NO] [H₂ O] 2 [NH3][0₂] [NO]¹ [H₂O]6 [NH₂] 4 [NO] ¹ [H₂O]6 [NH₂] 4 [0₂]5 c. CO₂(g) + MgO(s) = MgCO3(s) OK: OK= OK: OK= K: K= OK= [CS₂] [H₂]4 [CH₂] [H₂S] [CS₂] [CH][H₂S]² [CS₂] [H₂] [CH₂] [H₂S]² [CS₂] [H₂] 4 [CH₂] [H₂S]² K= 1 [CO₂] [MgCO₂]² [CO₂][MgO] [MgCO3] [CO₂]²[MgO]² [MgO] [CO₂][MgCO3]
The equation represents a chemical reaction at equilibrium. HCI (aq) + Mg (s) + Heat MgCl2 (aq) + H2 (g) What happens to the system when the temperature is decreased? O A. The reaction shifts toward the left, and the amount of hydrogen gas decreases. B. The reaction shifts toward the right, and the amount of hydrogen gas decreases. C. The reaction shifts toward the left, and the amount of hydrogen gas increases. D. The reaction shifts toward the right, and the amount of hydrogen gas increases.
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Consider the following exothermic reaction: C (s) + 2 Cl2 (g) ⇋⇋ CCl4 (g) How would the equilibrium shift if the reaction mixture is heated? Select one: a. The reaction would shift towards the products. b. The reaction would shift towards the reactants. c. The equilibrium would not be affected.
Which way would the equilibrium shift if the temperature was decreased for this reaction (AH = -542 kJ)? H₂ (g) + F₂ (g) → 2HF (g) Shift toward reactants Shift toward products Remain the same None of the above
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