Use the equilibrium constant expressions to calculate the value of K when the following concentrations are present at equilibrium. Then determine if the reaction favors the reactants or the products. For the reaction number 1 above at equilibrium [NH3]= 0.0100 M; [N2] = 0.0200 M; [H2]=0.0200M

Li2CO3(s) ⇆ 2Li+(aq) + CO3-2(aq)

At equilibrium [Li+] = 0.20 M [CO3-2]=0.10 M [Li2CO3] = 6.0M

6) For the reaction, CS2(g) + 3Cl2(g) ⇆ CCl4(g) + S2Cl2(g) , the equilibrium concentrations in moles per Liter for are [CS2] = 0.3 M [Cl2] = 0.9 M [ S2Cl2] = 0.9 M and [CCl4] = 0.9 M

Calculate the equilibrium constant.

If some of the concentrations were instead [CS2] = 0.5 M [Cl2] = 2.0 M [ S2Cl2] = 0.5 M, what would be the equilibrium concentration of CCl4?

7) Ammonia is synthesized from nitrogen and hydrogen in the following reaction:

N2(g)+3H2(g) ⇆ 2NH3(g)

At 500 ºC, the equilibrium constant for this reaction is 0.080. Given that [NH3] = 0.0596M,
[N2] =0.600M, and [H2] = 0.420 M, find Q and predict how the reaction will proceed.

8) At 1000ºC, K =1.0x10-13 for the decomposition of hydrofluoric acid (HF), as described in the reaction 2HF(g) ⇆ H2(g) + F2(g).

If [HF] = 23.0 M, [H2] = 0.540 M, and [F2] = 0.380 M, determine the value of Q and predict how the reaction will proceed.