three questions 19

QUESTION 1. Consider the reaction:
$2$

N



H


3




(


g


)



⟺



N


2




(


g


)



+


3



H


2




(


g


)

When B.00 x 10-1 moles of NH3(g) is introduced into a 1.00 L container, the equilibrium concentration of H2(g) to be B.00 x 10-2 M.

Calculate the equilibrium constant, Kc, for this reaction

QUESTION 2. The equilibrium constant, Kc, for the following reaction is A.0 at 350 K:
$H$

2



(


g


)




+




I


2




(


g


)



⟺


2


H


I



(


g


)

Calculate the equilibrium concentrations of the reactants and product when C.0 x 10-1 moles of each reactant is introduced into a 1.00 L vessel at 350 K.

QUESTION 3. The first order rate constant for the decomposition of an unknown compound is B.00 x 10-4 1/s.

a.) If you have a B.0 x 10-1 M solution what will be the concentration after C.00 minutes?

b.) What is the half-life of the unknown compound in seconds?