1
answer
0
watching
155
views
18 Nov 2019
The chemical system 2NOCI(g) = 2NO(g) + CI_2 (g) is at equilibrium at 300 degree C. What would the effect on the system be it an additional 1.3 mol of NO(g) was added to the system? A) The reaction would proceed in reverse to use some of the NO that was added. B) The reaction would proceed in the forward reaction to increase the concentration of CI_2 C) There would be no additional reaction since only one product was added. D) The system would not return to an equilibrium mixture. The questions that follow are based on the reaction at equilibrium C(s) + CO2(g) 2CO(g) Delta H^+ = +172.5 kJ/mol What would be the effect on the equilibrium's position of adding 3.5 g of C(s)? A) The position of the equilibrium would not change. B) The reaction would proceed to the product side. C) The reaction would proceed to the reactant side. D) Additional information is need to answer this question. What would be the effect of increasing the temperature on the proceeding the temperature on the proceeding reaction? A) The reaction would proceed in the product side. B) The Position of the equilibrium would not change. C) The reaction would proceed to the reactant side. D) Additional information is needed to answer this question. What would be the effect of increasing the temperature on the proceeding reaction? A) The reaction would proceed in the product side. B) The position of the equilibrium would not change. C) The reaction would proceed to the reactant side. D) Additional information is needed to answer this question. What would be the effect on the preceding reaction of decreasing the volume to one-half its original value? A) the position of equilibrium will shift to the product side. B) The position of equilibrium will shift to the reactant side. C) There will be no change in the position of the equilibrium. D) Additional information is needed to determine the changes. In answering the questions that follow, consider this reaction, which at equilibrium: NH_3 (g) + HCI(g) = NH_4 CI(s). What would be the effect of venting all of the gases from the system and then closing it again? A) The final pressure would be lower than it was before it was vented. B) More NH_4 CI would react to return the pressure to its original value. C) Equilibrium cannot be restored to this system. D) More NH_4 CI would form after the system was vented.
The chemical system 2NOCI(g) = 2NO(g) + CI_2 (g) is at equilibrium at 300 degree C. What would the effect on the system be it an additional 1.3 mol of NO(g) was added to the system? A) The reaction would proceed in reverse to use some of the NO that was added. B) The reaction would proceed in the forward reaction to increase the concentration of CI_2 C) There would be no additional reaction since only one product was added. D) The system would not return to an equilibrium mixture. The questions that follow are based on the reaction at equilibrium C(s) + CO2(g) 2CO(g) Delta H^+ = +172.5 kJ/mol What would be the effect on the equilibrium's position of adding 3.5 g of C(s)? A) The position of the equilibrium would not change. B) The reaction would proceed to the product side. C) The reaction would proceed to the reactant side. D) Additional information is need to answer this question. What would be the effect of increasing the temperature on the proceeding the temperature on the proceeding reaction? A) The reaction would proceed in the product side. B) The Position of the equilibrium would not change. C) The reaction would proceed to the reactant side. D) Additional information is needed to answer this question. What would be the effect of increasing the temperature on the proceeding reaction? A) The reaction would proceed in the product side. B) The position of the equilibrium would not change. C) The reaction would proceed to the reactant side. D) Additional information is needed to answer this question. What would be the effect on the preceding reaction of decreasing the volume to one-half its original value? A) the position of equilibrium will shift to the product side. B) The position of equilibrium will shift to the reactant side. C) There will be no change in the position of the equilibrium. D) Additional information is needed to determine the changes. In answering the questions that follow, consider this reaction, which at equilibrium: NH_3 (g) + HCI(g) = NH_4 CI(s). What would be the effect of venting all of the gases from the system and then closing it again? A) The final pressure would be lower than it was before it was vented. B) More NH_4 CI would react to return the pressure to its original value. C) Equilibrium cannot be restored to this system. D) More NH_4 CI would form after the system was vented.
Nelly StrackeLv2
9 May 2019