The equilibrium constant is given for one of the reactions below. Determine the

Question

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. H_2(g) + Br_2(g) rightarrow 2 HBr(g) K_c = 3.8 times 10^4 2 HBr(g) rightarrow H_2(g) + Br_2(g) K_e = ? 6.4 times 10^-4 1.6 times 10^3 5.3 times 10^-5 1.9 times 10^4 2.4 times 10^-6 Determine the value of K_c for the following reaction if the equilibrium concentrations are as followed 0.13 M, [HI]_eq = 5.6 times 10^-6 M, [Cl_2]_eq = 0.0019 M. 2 HCl(g) + I_2(s) rightarrow 2HI(g) + Cl_2(g) 8.2 times 10^-18 3.5 times 10^-32 1.4 times 10^-19 2.9 times 10^31 1.2 times 10^17 Calculate the value of [N_2]_eq if [H_2]_eq = 2.0 M, [NH_3]_eq = 0.5 M, and K_c = 2 N_2(g) + 3H_2(g) 2 NH_3(g) 0.031 M 62.5 M 0.40 M 0.052 M 0.005 M Consider the following reaction at equilibrium. What effect will adding more SO_3 have the system? SO_2(g) + NO_2(g) SO_3(g) + NO(g) The reaction will shift to decrease the pressure The reaction will shift in the direction of reactants. The reaction will shift in the direction of products. The equilibrium constant will decrease. No change will occur since SO_3 is not included in the equilibrium expression. What is the conjugate base of H_2PO_4^-? HPO_4^2- OH^- H_3PO_4 H_3O^+ PO_4^3- The stronger the acid, then which of the following is TRUE? The stronger the conjugate base The weaker the conjugate base The weaker the conjugate acid The stronger the conjugate acid. None of the above.

Explanation / Answer

14) e) 2.6*10^-5

15) b) 3.5 *10^-32

16) a) 0.031M

17) a) HPO4^2-

18) b) weaker than conjugate base

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