27. For the reaction below, what will be true for the NH]-0.30 M, [H:]-0.15 M, a

Question

27. For the reaction below, what will be true for the NH]-0.30 M, [H:]-0.15 M, and IN]-020 M system if (A) The system is at equilibrium. (B) The amount of product will increase over time. (C) The amount of product will decrease over time (D) The reaction will progress until all reactants are consumed 28. The reaction is investigated (essume an ideal gas mixture) Initially there are 4.0 moles of HO and 2.0 moles of Na in a 2.0 L container. If the concentration of N O at equilibrium is 0.30 M, what is the molar concentration of H:0 at equilibrium? (A) 1.9M (B) 1.7M (C) 0.30M (D) 0.15 M 29. For the reaction, K, is 0.01 at 2000 "C. After this system has established equilibrium, 0.015 moles of N are added. How does the addition of N, affect the concentrations of boO2 and NO once equilibrium is established again? (A) The concentration of O decreases and the (B) The concentration of O, does not change and the (C) The concentration of O; increases and the (D) The concentration of O; decreases and the concentration of NO does not change concentration of NO increases concentration of NO decreases concentration of NO increases 30. The equilibrium system is an exothermic reaction. Which change will result in a increase in the concentration of SO; when equilibrium is re-established? (A) a decrease in volume of the container (B) an increase in temperature (O) the removal of S0-g) (D) a decrease in pressure 31. What are the Brensted-Lowry bases in the reaction? (A) HCl and HF (C) F and Chr (B) Fr and HF (D) Ch and HCl

Explanation / Answer

27)

Qc = [NH3]^2 / [N2][H2]^3

= (0.30)^2 / (0.20 * 0.15^3)

= 133

Since Qc is greater than Kc, backward reaction will favour

So, the reactant will increase and product will decresae

Answer: C

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