Ans: Kc increase (a) is correct option
Since in exothermic reaction equilibrium constant is inversely proportional to temperature so when we decrease temperature Kc will increase.
The following exothermic reaction is at equilibrium [2SO3(g) + happen if the temperature is decreased. 2802(g)...
The reaction 2SO2 (g) + O2 (g) ↔ 2SO3 (g) is exothermic and at equilibrium. Which of the following action will shift equilibrium left? A Lower environment temperature B Add O2 to the system C Add a catalyst to slow down the reaction D Add Ne gas to the equilibrium E Increase the volume of the reaction chamber
At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g)+O2(g)<==>2SO3(g) is 2.99x10^-3. What is the value of the equilibrium constant for each of the following reactions at that temperature? a. SO2(g)+ 1/2 O2(g)<==> SO3(g) b. 2SO3(g)<==>2SO2(g)+O2(g) c. SO3(g)<==> SO2(g)+ 1/2 O2(g)
1. Consider the following reaction at equilibrium. 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g) a. What will happen if the pressure increased? b. What will happen if the concentration of FeS2(s) is decreased? 2) The following reaction is exothermic: What direction will the equilibrium shift if the following changes are made? 2 SO2(g) + O2(g) ⇌ 2 SO3(g) a) Raising the temperature b) Adding SO3 c) Removing O2 d) Decreasing the volume
The equilibrium constant, K, for the following reaction is 1.71x10-2 at 1120 K. 2803(8) 2802(g) + O2(g) Calculate Kat this temperature for the following reaction: SO2(g) + 1/2O2(g) 2 so3(g) K.
2SO2 (g) + O2 (g) <---> 2SO3 (g) The reaction is exothermic. How does the equilibrium shift at: a) increase of [O2]? b) decrease of [SO3]? c) increase in pressure? d) increase in the volume of the container? e) increase in temperature? f) addition of catalyst?
Consider the following system at equilibrium where AH° = 198 kJ, and K. = 2.90x102, at 1.15*10°K. 2SO3(g) — 2802(g) + O2(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 Kc B. is equal to Ko 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° = 198 kJ, and K. = 2.90x10-2, at 1.15*109K 2SO3(g) = 2802(g) + O2(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...
For the following endothermic reaction system at equilibrium: 2SO3(g) <---> 2SO2(g) + O2(g) Choose the changes that will shift the equilibrium position to the right. (Select all that apply.) Add Ne(g) Add SO2(g) Remove SO3(g) Decrease temperature Add a catalyst Increase temperature Decrease volume
The system, CO(g) + O2(g) 2 CO2(g), is exothermic and at equilibrium at a temperature. Predict how Kp changes and direction of the shift if the temperature is increased. Kp increases, and it shifts to the right. Kp increases, and it shifts to the left. Kp decreases, and it shifts to the left. Kp doe not change, and it does not shift to either direction. Kp decreases, and it shifts to the right.
The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 7 × 103 at a certain temperature. If at equilibrium, [SO2] = 0.0451 M and [O2] = 0.078 M, what is the equilibrium [SO3]?