i have difficulty in this question. any help would be much appreciated.
1)CO(g)+2H2(g)->CH3OH(g)
at 225c, K is 10.2 liter^2/mol^2. what concentration of CH3OH(g)is in equilibrium with CO(g) at a concentration of 0.020 mol/liter and H2(g) at a concentration of 0.020mol/liter?
[Answered elsewhere]
To solve this problem, we will use the equilibrium constant expression and the given concentrations to find the equilibrium concentration of CH3OH(g).
The balanced equation for the reaction is:
CO(g) + 2H2(g) -> CH3OH(g)
According to the law of mass action, the equilibrium constant expression for this reaction is:
K = [CH3OH] / ([CO] * [H2]^2)
Given:
- The equilibrium constant (K) is 10.2 L^2/mol^2 at 225°C.
- The concentration of CO(g) is 0.020 mol/L.
- The concentration of H2(g) is 0.020 mol/L.
Let's substitute these values into the equilibrium constant expression:
10.2 = [CH3OH] / (0.020 * 0.020^2)
Now, we solve for [CH3OH]:
[CH3OH] = 10.2 * (0.020 * 0.020^2)
= 10.2 * (0.020 * 0.0008)
= 0.01632 mol/L
Therefore, the concentration of CH3OH(g) in equilibrium with CO(g) at a concentration of 0.020 mol/L and H2(g) at a concentration of 0.020 mol/L is 0.01632 mol/L.