For the reversible reaction A(g) –> <– B(G) which K values would indicate …?
which K values would indicate that there is more B than A at equilibrium?
K=9×10^-5
K =2000
K = 0.7
K=4×10^8
Answer:
This is the Best answer for For the reversible reaction A(g) –> <– B(G) which K values would indicate …?
K= 2000 and K=4 x 10^8
K=products/reactants=B/A
So if I let A=2 and B=1, K=1/2=0.5 **A number of less than 1 indicates reactants are more than the products.
If I let A=1 and B=2, K=2/1=2 **A number greater than 1 indicates products are greater than the products.