Question

1. A student ran the following reaction in the laboratory at 632 K:

2HI(g) ->H₂(g) + I₂(g)  

When she introduced 0.362 moles of HI(g) into a 1.00 liter container, she found the equilibrium concentration of I₂(g) to be 3.55×10^-2 M.  

Calculate the equilibrium constant, K_c, she obtained for this reaction.  

K_c =

2. A student ran the following reaction in the laboratory at 616 K:

CO(g) + Cl₂(g) -> COCl₂(g)

When she introduced 0.131 moles of CO(g) and 0.161 moles of Cl₂(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 6.37×10^-2 M.  

Calculate the equilibrium constant, K_c, she obtained for this reaction.  

K_c =  

Answer 1