Assume that the following chemical reaction is at equilibrium. 2 ICl(g) Double h

Question

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) Double headarrow I_2(g) + Cl_2(g) Delta H^degree = 26.9 kJ At 25 Degree C, K_p = 2.0 times 10^5. If the temperature is decreased to 15 Degree C which statement applies? KP will increase and the reaction will proceed in the backward direction. K_p will decrease and the reaction will proceed in the backward direction. K_p will increase and the reaction will proceed in the forward direction. K_p will remain unchanged and the reaction will proceed in the forward direction. Kp will decrease and the reaction will proceed in the forward direction. Rate data have been determined at a particular temperature for the overall reaction 2NO + 2H_2, in which all reactants and products are gases. The rate law expression is. rate = k[NO][H2]^2 rate = k[NO][H2]^2 rate = k[NO]^2[H_2]^2 d rate = k[NO]^2[H2]

Explanation / Answer

19. as DH = +ve , at low temperature , Kp is lower

so that ,

answer: b

20. order .w.r.t NO

r1/r2 = (a1/a2)^n

(0.015/0.06) = (0.1/0.2)^n

n = 2

   order w..r.t H2

(0.015/0.0225) = (0.2/0.3)^n

   n = 1

rate = k [NO]^2[H2]

answer: d

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