A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step l:

Question

A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step l: HAg) + 2 NO(g) N2O(g) + H2O(g) (slow) Step 2: N20(g) + Hdg)- N2(g) + H20(g) (fast) Which of the following statements is NOT true? a· The energy profile for this reaction probably has two maxima. b. The reaction rate is probably second order in NO. C. The reaction rate is probably first order in H2. d. N20 is an intermediate. e· The activation energy for step 2 is probably less than that of step 1. A chemical equilibrium 2 AB has a forward rate constant, kf-10 M-1 s-1, and a reverse rate constant, k 5 s. If the system has a concentration of [A]-0.10 M at equilibrium, what is the concentration of B at equilibrium? a. 20 b. 2 c. 0.2 d. 0.02 e. 200 Which of the following statements regarding the equilibrium constant is NOT true? a. when K >> 1 , the concentration of products is much greater than the concentrations of reactants at equilibrium. When K 1, the products and reactants come to equilibrium rapidly. b. c. d, e. The initial rate data for the reaction 2N205(g) 4N02(g) + Odg) is shown in the following table. Determine the value of the rate constant for this reaction ,04 Rate (M/s) 450 22.5 xperiment 2.56 x 10 a. 4.09 s b. 0.176 s c. 0.0569 s d. 0.225 s e. 80.1 s For the equilibrium, 2 PH,(g)P2(g) + 3 Hag), the equilibrium partial pressures are Pu, 0.022 atm, P 0.289 atm, and Pu,0.867 atm at 873 K. Calculate Kp a. 0.0585 d. 2.50×10-3 e. 389 c. 0.0441 If the reaction quotient Q has a smaller value than the related equilibrium constant K, . a. the reaction is at equilibrium. b. the reaction will continue to make more products. c, the reaction will consume products and make reactants. d. the reaction will release heat to achieve equilibrium. e. the value of K will decrease until it is equal to Q.

Explanation / Answer

2) Kf/Kb = [B]/[A^2]

10/5 = [B]/(0.10)^2

[B] = 0.02

3) Answer E

4) If concentration of N2O5 reduces by 20 times, the rate of reaction also reduced by 20 times. Hence it is first order

rate = K[N2O5]

K = rate/[N2O5] = (450-22.5)/(1.58*10^3-1.28*10^2) = 0.176 s^-1

Answer : B

5) 2PH3 === P2 + 3H2

Kp = [P2][H2]^3/[PH3]^2

Kp = (0.289)(0.867)^3/(0.022)^2

Kp = 389 (answer E)

6) answer B

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