Question 2 of 8 Sub Which of the following changes will result in a change in the value of the rate constant for the reaction 2 A→ products? A) Increasing the concentration of A B) Decreasing the concentration of A C) Increasing the temperature of the reaction D) Allowing the reaction to reach equilibrium E) Increasing the pressure

For a reaction A+B 2 AB, if the initial concentration of A is 2.00 M, B is 1.80 M and AB is OM and the equilibrium concentration of AB is 0.02 M. Select all statements that are TRUE. O The concentration of A at equilibrium is 2.00 M. O To calculate the Keg for this reaction, we can use (A]=2.00 M, [B]= 1.80 M and (AB]=0.02 M to solve for it. O The concentration of B at equilibrium is 1.78 M. O The Keq will be much larger than 1 and this reaction favor the formation of the product. O The change in concentration, x, is equal to 0.02 M.

The following reaction is exothermic: 3A(g) B(g) + C(g) Gaseous argon is added to the equilibrium mixture without change in volume or temperature. Predict the effect of the possible stress mentioned directly above on the reaction mixture by selecting the correct phrase bel shift right to attain chemical equilibrium no shift to attain chemical equilibrium shift left to attain chemical equilibrium Onot enough information to answer question Previous DELL II O O O O

Catalysts increase reaction rates by _____ A) increasing the activation energy. B) increasing the enthalpy of reaction. C) decreasing the enthalpy of reaction. D) providing an alternate reaction mechanism with a lower activation energy. E) changing the value of the equilibrium constant.