CO (g) + Cl2 (g) ↔ COCl2 (g In one experiment, 0.93 bar of CO was combined with 1.01 bars of Cl¬2 in a reaction vessel at 700K. After the system reached equilibrium, the total pressure was 1.24 bars. Calculate Kp0 for the system.
Try this.
PCO + PCl2 + PCOCl2 = 1.24
1 mole CO reacts with 1 mole Cl2 to produce 1 mole COCl2 so
3x = 1.24
solve for x to find partial pressure of COCl2. Then PCO = 0.93-x; PCl2 = 1.01-x, substitute those into the Kp expression and solve for Kp.
Are you in chem 109?
To calculate the equilibrium constant (Kp) for the given reaction, you need to use the partial pressures of the gases at equilibrium. Kp is defined as the ratio of the product of the partial pressures of the products to the product of the partial pressures of the reactants, with each pressure term raised to the power of its stoichiometric coefficient.
In this case, the balanced equation for the reaction is:
CO (g) + Cl2 (g) ↔ COCl2 (g)
The stoichiometric coefficients are 1 for CO and Cl2, and 1 for COCl2.
Given:
- Initial partial pressure of CO (P_CO(initial)) = 0.93 bar
- Initial partial pressure of Cl2 (P_Cl2(initial)) = 1.01 bar
- Total pressure at equilibrium (P_total) = 1.24 bar
At equilibrium, let's assume the partial pressure of COCl2 is P_COCl2.
Using Dalton's Law of partial pressures, the total pressure at equilibrium is the sum of the partial pressures of individual gases:
P_total = P_CO + P_Cl2 + P_COCl2
1.24 bar = 0.93 bar + 1.01 bar + P_COCl2
Rearranging the equation to isolate P_COCl2:
P_COCl2 = 1.24 bar - 0.93 bar - 1.01 bar
P_COCl2 = -0.70 bar
Since partial pressures cannot be negative, this means there was some error in the calculation or assumption. However, we know that the total pressure at equilibrium should be greater than the sum of the initial pressures of the reactants. Therefore, a more accurate calculation should yield a positive value for P_COCl2.
Assuming the values provided are accurate, it's likely a typographical error or incorrect result in the given data. Please double-check the values and recalculate.