The equilibrium constant Kp for the reaction below at 700°C is 0.76 atm.
CCl4(g) C(s) + 2 Cl2(g)
Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700°C
See your posts below. You should get the hang of how this is done.
To determine the initial pressure of carbon tetrachloride (CCl4), we need to use the equilibrium constant (Kp) and the stoichiometric coefficients of the balanced equation. Here's how to do it step by step:
1. Write the balanced equation for the given reaction:
CCl4(g) C(s) + 2 Cl2(g)
2. Set up the expression for the equilibrium constant (Kp) using the partial pressures in atm:
Kp = (P(C) * P(Cl2)^2) / P(CCl4)
3. Substitute the given value of Kp into the equation:
0.76 = (P(C) * P(Cl2)^2) / P(CCl4)
4. Let's assume that initially, there is only carbon tetrachloride present, and no carbon or chlorine. Therefore, the initial pressure of carbon tetrachloride (P(CCl4)_initial) is equal to the total equilibrium pressure of 1.20 atm.
5. Substitute the values into the equation:
0.76 = (P(C) * P(Cl2)^2) / 1.20
6. We need to solve for the pressure of carbon (P(C)). Rearrange the equation to solve for P(C) by multiplying both sides of the equation by 1.20:
0.76 * 1.20 = P(C) * P(Cl2)^2
7. Substitute the given value of Kp into the equation, and take the square root of both sides:
(0.76 * 1.20)^0.5 = P(C) * P(Cl2)
8. Since the question asks for the initial pressure of carbon tetrachloride, we can ignore the pressure of chlorine (P(Cl2)) for now. Therefore, the initial pressure of carbon tetrachloride is equal to P(C):
P(C) = (0.76 * 1.20)^0.5
9. Calculate the value:
P(C) = 0.983 atm
Therefore, the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700°C is approximately 0.983 atm.