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. |
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Kp increases, and it shifts to the left. |
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Kp decreases, and it shifts to the left. |
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Kp doe not change, and it does not shift to either direction. |
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Kp decreases, and it shifts to the right. |
In case of exothermic reaction with increase in temperature, to keep kp constant reaction shift towards left.
The system, CO(g) + O2(g) 2 CO2(g), is exothermic and at equilibrium at a temperature. Predict...
The following endothermic reaction is at equilibrium. 2 CO(g) + O2(g) 42 CO2 (g) What is the effect of the following changes on the position of the equilibrium? a) CO2 (g) is removed no shift b) The volume of the container is decreased by a factor of 2. shifts to make more product c) The temperature is decreased. shifts to make more products d) CO (g) is added no shift e) He (g) is added and the pressure doubles shifts...
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...
ΔH is positive for the equilibrium N2 (g) + O2 (g) ↔ 2 NO (g). If we lower the temperature, (A) the equilibrium shifts to the left (more N2 + O2 gases formed) (B) the equilibrium shifts to the right (more NO gas formed) (C) Equilibrium does not shift because there are the same number of molecules on left side as on the right (D) Equilibrium does not shift because temperature does not affect the reaction rates why?
The following exothermic reaction is at equilibrium [2SO3(g) + happen if the temperature is decreased. 2802(g) + O2(g) ). Predict what will O K , increases Nothing Changes Ke decreases Kremains the same more SO2(g) is consumed
Part A N2(g)+3Br2(g)⇌2NBr3(g) K=[NBr3]2[N2][Br2]3 K=[N2][Br2]3[NBr3]2 K=[NBr3][N2][Br2] K=[NBr3]2[N2][Br2]3 Part B C(s)+O2(g)⇌CO2(g) K=[CO2][O2] K=[O2][CO2] K=[CO2][O2] K=[CO2][O2][C] When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s)+H2O(g)+heat⇌CO(g)+H2(g) Part C What effect does each of the following changes have on the equilibrium? Drag the appropriate stresses to their respective bins. add H2O, Add heat, lower temperature, remove CO Categories: Equilibrium shifts to products, Equilibrium shifts to reactants, Equilibrium doesn't shift
Predict and calculate the effect of temperature change on an equilibrium system. CO reacts with Cl, to form COC12. The equilibrium constant, Kp, for this reaction is 0.200 at 873 K. CO(g) + Cl2(g) 2 COCl2(g) The standard enthalpy change for this reaction (AHº) is -108 kJ/mol. (a) Predict the effect on the production of COCl2 when the temperature of the equilibrium system is increased. (b) Use the van't Hoff equation to estimate the equilibrium constant for this reaction at...
Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(l) ΔH° = −2220 kJ. a. The reaction will shift to the right and K increases. b. No effect will be observed. c. The reaction will shift to the right and K decreases. d. The reaction will shift to the left and K increases. e. The reaction will shift to the left and K decreases.
1 point 200,(9) is increased If the pressure on the equilibrium system 2CO(g) + O2(g) a. The quantity of CO(g) increases b. The quantity of CO2(g) increases C. The quantity of CO2(g) decreases d. The quantities in the system do not change Oo oo
1. Predict the effect on the equilibrium system in below if the reaction temperature is increased. 2 SO2(g) + O2(g) ↔ 2 SO3(g)+ heat a. Shift to the product side b. There will be no change. c. Shift to the reactant side 2. Predict the effect on the equilibrium system in below if the SO2 gas concentration is decreased. 2 SO2(g) + O2(g) ↔ 2 SO3(g) a. Shift to product side b. shift to reactant side c. no change 3....
Using Le Chatelier's Principle to predict the result of changing Nitrogen monoxide and ozone react to form nitrogen dioxide and oxygen, like this: The reaction is exothermic. Suppose a mixture of NO, O, NO2 and O2 has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. shift in...