10. Consider this reversible reaction. All substances are gases and are in an in

Question

10. Consider this reversible reaction. All substances are gases and are in an insulated closed chamber with a constant volume and are at equilibrium. 2H2O + 2C12-4HC1+ O2 ??. +113 kJ What will be the effect of increasing the temperature? (A) More C12 will be produced. (B) More HCI will be produced. (C) The volume of each of the gases will increase. (D) More water will be formed (E) There will be no change. 11. Into an empty vessel COCI2(g) is introduced at 1.0 atm pressure whereupon it dissociates until equilibrium is established: If x represents the partial pressure of CO2(g) at equilibrium, what is the value of the equilibrium constant, Kp? (D 12. A mixture of 2.0 mol of CO(g) and 2.0 mol of H20(g) was allowed to come to equilibrium in a IL flask at a high temperature. If Kc-4.0, what is the molar concentration of H2(g) in the equilibrium mixture? 1.0 (B) 0.67 (C) 0.75 13. In this reaction, which substances are bases according to the Bronsted Lowry definition? HC2H302+H20-H30++C2H302- (A) (B) HC2H302 and H20 HC2H302 and C2H302 (C) H20 and C2H302- (D) H30+ and C2H302 14. SnC14 accepts two electron pairs and acts as (A) B) (C) a Brensted acid. a Lewis acid. an Arrhenius base. (D) a Lewis base. 15. HCl is a strong acid. What is the pH of 200 mL of 0.002 M HCI? (A) 2.0 (D) 4.0 (B) 2.7 (C) 34 16. Assuming complete ionization, the pH of a 0.0005 M solution of Ca(OH)2 is approximately (B) seven. (A) three. (C) eleven. (D) thirteen.

Explanation / Answer

Ans 10

Option B is the correct answer

The given equation is endothermic reaction

Heat is absorbed by the reaction.

From the Le Chatelier's principle

Increasing the temperature of the reaction, more products will form.

More HCl will be produced

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