Explanation:
im not sure all I know is 1.81 x 1024
Answer:
Kc = 4.76
Explanation:
To find the concentrations of CO and H₂ at equilibrium, you have to set up an ICE (Initial, Change, Equilibrium) table.
CO (g) + 2H₂(g) ⇌ CH₃OH (g)
I 0.32 M 0.53 M 0
C -x -2x +x
E 0.32-x 0.53-2x 0.16 M
Since you know the concentration of CH₃OH at equilibrium, it would be equal to x since 0 + x = 0.16. So,
[CH₃OH] = 0.16 M
[CO] = 0.32 - 0. 16 = 0.16 M
[H₂] = 0.53 - 2(0.16) = 0.21 M
Now that you have all the concentrations at equilibrium, you can calculate the equilibrium constant.
Kc = products ÷ reactants
= [CH₃OH] ÷ [CO][H₂]²
= 0.16 ÷ (0.16)(0.21)
Kc = 4.76
The equilibrium constant at this temperature is 4.76.
Hope this helps.
