Calculate Kc.
CH_4(g) + H_2O(g) <-> CO(g) + 3H_2(g)
Kp= 7.7 x 10^24 at 298K.
Should I use the formula Kp= Kc(RT)^Deltang
If so I have no idea where to start.
What do you mean you don't know where to start. This is just a case of substitute and solve.
7.7E24 = Kc(0.08205*298)^(4-2)
Solve for Kc.
To calculate Kc from Kp using the formula Kp = Kc(RT)^Δn, we need to know the change in the number of moles (Δn) of gas molecules as the reaction proceeds. In this case, the balanced equation shows that 1 mole of CH4(g) and 1 mole of H2O(g) react to form 1 mole of CO(g) and 3 moles of H2(g). Hence, the Δn is 1 + 3 - 1 - 1 = 2.
Now, let's go step by step to calculate Kc:
1. Convert the given Kp value to Kc using the formula Kp = Kc(RT)^Δn.
Rearranging the formula, we have:
Kc = Kp / (RT)^Δn
2. Gather the necessary values:
- Kp = 7.7 x 10^24 (given)
- R = 0.0821 L.atm/(K.mol) (ideal gas constant)
- T = 298 K (temperature in Kelvin)
- Δn = 2 (change in the number of moles of gas)
3. Substitute the values into the formula:
Kc = (7.7 x 10^24) / [(0.0821 L.atm/(K.mol)) * (298 K)]^2
4. Calculate the value of (RT)^Δn:
(0.0821 L.atm/(K.mol) * (298 K)) = 24.4102 L.atm/mol
Then, [(0.0821 L.atm/(K.mol)) * (298 K)]^2 = 596.953 L^2.atm^2/mol^2
5. Substitute the value of (RT)^Δn back into the initial equation and calculate Kc:
Kc = (7.7 x 10^24) / 596.953 L^2.atm^2/mol^2
6. Finally, calculate Kc:
Kc ≈ 1.29 x 10^22 L^2/mol^2
Therefore, Kc is approximately 1.29 x 10^22 L^2/mol^2.