For the reaction A + 2B ←→ C, what is the value of KC if the rate law is given by–rA = k(CA2/3/CB – KCCC)? Given that initial concentration of A is equal to that of B = 5M and the equilibrium conversion of B is found to be 0.3. k = 100.

For the reaction A + 2B ←→ C, what is the value of KC if the rate

1.	For the reaction A + 2B ←→ C, what is the value of KC if the rate law is given by–rA = k(CA2/3/CB – KCCC)? Given that initial concentration of A is equal to that of B = 5M and the equilibrium conversion of B is found to be 0.3. k = 100.
A.	Kc = 0
B.	Kc = 0.5
C.	Kc = 1
D.	Kc = 1.5
Answer» D. Kc = 1.5