Write an equilibrium constant expression for this reaction: Ag_2SO_4 (s) 2 Ag^+

Question

Write an equilibrium constant expression for this reaction: Ag_2SO_4 (s) 2 Ag^+ (aq) + SO_4^2- (aq) For the reaction in #1 above, the K value is 1.1 Times 10^-5 at 298K. Is the equilibrium reaction mixture reactant favored, product favored, or neither? Consider this reaction: NH_4HS (s) NH_3 (g) + H_2S (g) At a certain temperature. K = 8.5 Times 10^-3. A reaction mixture at this temperature containing solid NH_4HS has [NH_3] = 0.166 M and [H_2S] = 0.166 M. What is the reaction quotient for this reaction mixture? Is the reaction in #3 above at equilibrium? If not. in which direction will it proceed to attain equilibrium? For this reaction, K = 255 at 1000 K. If a reaction mixture initially contains a CO concentration of 0 1500 M and a CI_2 concentration of 0.175 M at 1000 K, what is the equilibrium concentration of COCI_2 at 1000K? CO(g) + Cl_2 (g) COCl_2(g) Suppose you start with 1.00 mol each of carbon monoxide and water in a 50.0 L vessel. How many moles of CO are in the equilibrium mixture at 1000 degree C if K_c at this temperature is 0.58?

Explanation / Answer

1.

K = [products]^p / [reactnats]^r

K = [Ag+]^2 [CO3-2] / [ Ag2CO3]

for solids [] = 1

so

K = [Ag+]^2 [CO3-2]

2.

if K < 1, then this is favoured toward products, in this case, toward solid Ag2CO3

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