What is the equilibrium constant expression for the reaction? C(s) + 2H_2(g) CH_

Question

What is the equilibrium constant expression for the reaction? C(s) + 2H_2(g) CH_4(g) (A) K =[CH_4/CIH_2]^2 (B) K =[CH_4]/[H_2]^2 (C) K =[CIH_2]^2/[CH_4] (D) K =[H_2]^2/[CH_4] 22. The molecular picture represents equilibrium conditions for this gas phase reaction. What is the value of K for this reaction? (A) 9 (B) 9/4 (C) 382 (D) 6/5 23. Here is a partially completed equilibrium calculation table for the synthesis of ammonia. When this table is completed correctly, what it Y. the expression for the final pressure of hydrogen? (A) 0 (B) 2-2x (C) 2-3/2x (D) 2-3x 24.MgF_2 has 80times10^4. What is the solubility of MgF_2 in mol L^-1? (A) 2.8times10^-4 (B) 2.7times10^-3 (C) 3.4times10^-4 (D) 4.3 times 10^-3 25.For this reaction at equilibrium. Ni^2+(aq) + 6NH_3(aq) |Ni(NH_3))_6]^2 times(aq) the concentration of [Ni(NH_3))]^2 will increase if (A)Ni(NO_3)_2(s) is added. (B)a catalyst is added. (C)a soluble reagent is added that removes Ni^2+. (D)N_2 is bubbled through the solution to remove dissolved NH_3. 26 2NO_2(g) N_20_4(g). K_P = Z What is K_P for the reaction 1/2N_2O_4(g) NO_2(g)? (A) 1/z (B) 1/2Z (C) 1/squareroot Z (D) 1/Z^2

Explanation / Answer

21) While writing equilibrium constant expression, solids cannot be considered.

Kc = equilibrium concentration of products/ equilibrium concentration of reactants

= [CH4]/[H2]2

23) D

N2 + 3H2 -------->2 NH3

Initial 1 2 0

change 2x

final 1-x 2-3x

25)

Given that For MgF2, Ksp = 8.0 × 10–8

   MgF2 <-------------> Mg2+ + 2F-

s 2s s =  molar solubility of MgF2

Ksp = [Mg2+] [F-]2

Ksp = [s] [2s]2

     8.0 × 10–8 = 4s3

s = 2.7x 10-3 mol/L

Therefore,

ans = B

26) The given reaction is obtained by reversing and dividing the 1st equation with 1/2.

Therefore,

new K = 1/ (Z)1/2

ans = C

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