2. Consider the following system at equilibrium where H° =
108 kJ/mol, and Kc =
1.29×10-2, at 600
K.
COCl2(g) CO (g) +
Cl2(g)
When 0.19 moles of
COCl2(g) are removed
from the equilibrium system at constant temperature:
The value of Kc _________increases.decreases.remains the
same.
The value of Qc _________is greater than is equal to is
less than Kc.
The reaction must
run in the forward direction to reestablish equilibrium.
run in the reverse direction to reestablish equilibrium.
remain the same. It is already at equilibrium.
The concentration of CO will
_________increase.decrease.remain the same.
The value of Kc is constant at a fixed temperature. For this reaction the temperature is kept constant at 600 K. So The value of Kc remains unchanged.
So, When 0.19 moles of COCl2(g) are removed from the equilibrium system at constant temperature ---
The value of Kc remains the same as Kc depends only on temperature. As the temperature is fixed so Kc is also same.
As the concentration of COCl2 decreases, the reaction will proceed towards reverse direction in order to increases the concentration of COCl2. So, the concentration of products decreases. Again, Qc is the ratio of the concentration of products to the concentration of reactants. As the product concentration decreases the value of Qc is less than Kc.
The reaction must --------- run in the reverse direction to reestablish equilibrium. The reason is discussed in the above paragraph.
As the reaction goes to the reverse direction so the concentration of CO will decreases.
2. Consider the following system at equilibrium where H° = 108 kJ/mol, and Kc = 1.29×10-2,...
Consider the following system at equilibrium where Delta H° = -108 kJ, and Kc = 77.5, at 600 K. CO(g) + Cl2(g) <---> COCl2(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of Kc A. increases. B. decreases. C. remains the same. The value of Qc A. is greater than Kc. B. is equal to Kc. C. is less than Kc. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run...
Consider the following system at equilibrium where H° = -108 kJ, and Kc = 77.5 , at 600 K: CO (g) + Cl2(g) COCl2(g) If the TEMPERATURE on the equilibrium system is suddenly increased : The value of Kc A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run...
Consider the following system at equilibrium where H° = 111 kJ, and Kc = 6.30, at 723 K: 2NH3(g)--> N2(g) + 3H2(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: 1- the value of Kc A. Increases B. Decreases C. Remains the same 2- The value of Qc A. Is greater than Kc B. Is equal to Kc C. Is less than Kc 3- The reaction must: A. Run in the forward direction to reestablish equilibrium. B. Run...
Consider the following system at equilibrium where H° = 111 kJ, and Kc = 6.30, at 723 K. 2NH3(g) N2(g) + 3H2(g) When 0.22 moles of N2(g) are added to the equilibrium system at constant temperature: please double check answer to make sure its correct, thank you. The value of Kc _________increases.decreases.remains the same. The value of Qc _________is greater than is equal to is less than Kc. The reaction must ? run in the forward direction to restablish equilibrium. run in...
Consider the following system at equilibrium where delta H° = 87.9 kJ/mol, and Kc = 1.20×10-2, at 500 K. PCl5(g) ⇌ PCl3(g) + Cl2(g) When 0.15 moles of PCl5(g) are removed from the equilibrium system at constant temperature: Answer the following: The value of Kc _________ (possible answers: increases, decreases, or remains the same) The value of Qc _________(possible answers: is greater than, is equal to, or is less than) Kc. The reaction must (choose a, b, or c from...
Consider the following system at equilibrium where AHo--87.9 kJ, and Kc-83.3, at 500 K. PCl3(g) C2(gPCI5(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of KcA. increases B. decreases C. remains the same The value of Qc A. is greater than Kc B. is equal to Kc C. is less than K The reaction must:A. run in the forward direction to reestablish equilibrium B. run in the reverse direction to reestablish equilibrium C....
Consider the following system at equilibrium where H° = -87.9 kJ, and Kc = 83.3 , at 500 K: PCl3(g) + Cl2(g) PCl5(g) If the TEMPERATURE on the equilibrium system is suddenly decreased : The value of Kc A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in...
Consider the following system at equilibrium where H° = 10.4 kJ, and Kc = 1.80×10-2, at 698 K: 2HI(g) =H2(g) + I2(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction...
Consider the following system at equilibrium where AH° = -198 kJ, and K. = 34.5, at 1.15*10' K. 2802(g) + O2(g) 2803(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of K A. increases. B. decreases. C. remains the same. The value of Qc A. is greater than K. B. is equal to K C. is less than K The reaction must: A. run in the forward direction to reestablish equilibrium. B. run...
Consider the following system at equilibrium where AH° ° = 10.4 kJ, and Kc = 1.80x10-2, at 698 K. 2HI(g) H2(g) + 12(g) When 0.25 moles of H2(g) are removed from the equilibrium system at constant temperature: The value of Kc The value of Qc AK The reaction must Crun in the forward direction to restablish equilibrium. run in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. The concentration of 12 will