Use Your Knowledge Of The Collision Theory And Use The Poten
Use Your Knowledge Of The Collision Theory And Use The Potential Energ
Use your knowledge of the collision theory and use the potential energy diagram given to answer questions 1 through 5. Which letter represents the activation energy? Select one: a. A b. B c. C d. None of the above
What is represented by the letter "b"? Select one: a. Potential energy of the products b. Activated Complex c. Reverse Activation Energy d. Forward Activation Energy
What amount of energy is absorbed in the completion of the forward reaction? Select one: a. 100 kJ b. 200 kJ c. 300 kJ d. 400 kJ
Which letter would NOT be affected by the addition of a catalyst? Select one: a. A b. B c. C d. All of the above
The reaction of charcoal (carbon) and oxygen is sped up by grinding the charcoal into a fine powder. This is an example of: Select one: a. Increasing concentration to increase reaction rate b. Increasing temperature to increase reaction rate c. Increasing surface area to increase reaction rate d. All of the above
The rate of a reaction depends upon: Select one: a. The concentration of the reactants b. The temperature of the reaction c. The nature of the reactants d. All of the above
Which reactions are involved in determining equilibrium: Select one: a. Forward reaction b. Reverse reaction c. Both of the above d. Neither of the above
The rate of a reaction is dependent upon the equilibrium constant. Select one: True False
An equilibrium constant of 900 indicates: Select one: a. There are more reactants than products at equilibrium b. There are more products than reactants at equilibrium c. There are the same amount of reactants and products at equilibrium d. The reaction is not at equilibrium
The equilibrium expression for the reaction: H2(g) + I2(g) 2HI(g) would be: Select one: a. K = [HI]2 / [H2][I2] b. K = [H2][I2] / [HI]2 c. K = 2[HI] / [H2][I2] d. K = [H2][I2] / 2[HI]
The equilibrium constant for the following reaction: Ca(HCO3)2(s) CaO(s) + 2 CO2(g) + H2O(g) would be: Select one: a. K = [CaO][CO2]2[H2O] / [Ca(HCO3)2] b. K = [Ca(HCO3)2] / [CaO][CO2]2[H2O] c. K = [CO2]2[H2O] / [Ca(HCO3)2] d. K = [CO2]2[H2O]
Given the reaction: A + B C + D. The concentrations at equilibrium are [A] = 1 M, [B] = 1 M, [C] = 2 M, and [D] = 2 M. What is the value of the equilibrium constant (K)? Select one: a. 0.25 b. 1.0 c. 2.0 d. 4.0
The Haber process is a method to produce ammonia from hydrogen and nitrogen gases. The reaction is: N2(g) + 3 H2(g) 2 NH3(g). If hydrogen gas is added after the reaction has reached equilibrium, the reaction will: Select one: a. Shift to the right to produce more product b. Shift to the left to produce more reactants c. Stop. All of the nitrogen gas has been used up. d. Need more information
Given the reaction: N2(g) + 3 H2(g) 2 NH3(g). If the system is at equilibrium, what will happen if pressure is added? Select one: a. Nothing. Pressure does not affect equilibrium position. b. The reaction will shift to the right to produce more product. c. The reaction will shift to the left to produce more reactants d. All of the above
Given the following reaction: 2 HCl(aq) + Mg(s) MgCl2(aq) + H2(g) + heat. When the temperature is decreased, what changes occur? Select one: a. In order to restore equilibrium, the reaction shifts right, towards reactants. b. In order to restore equilibrium, the reaction shifts right, towards products. c. In order to restore equilibrium, the reaction shifts left, towards reactants. d. In order to restore equilibrium, the reaction shifts left, towards products.
Given the reaction: Fe3+(yellow) + SCN-(colorless) [FeSCN]2+(dark red). If Fe3+ is added to the solution: Select one: a. The solution becomes more yellow b. The solution turns darker red c. The solution becomes colorless d. No changes in color occur
Given the equation: A2(g) + B2(g) 2AB(g). [A] = 4.0 M, [B] = 2.0 M, and [AB] = 4.0 M at equilibrium. What is the value of the equilibrium constant (K)? Select one: a. 1.0 b. 2.0 c. 3.0 d. 4.0
The equilibrium constant for a given reaction = 1.0 x 10-8. What does that indicate about the reaction at equilibrium? Select one: a. The equilibrium lies far to the right, and there is a greater concentration of products than reactants b. The equilibrium lies far to the left, and there is a greater concentration of products than reactants c. The equilibrium lies far to the right, and there is a greater concentration of reactants than products. d. The equilibrium lies far to the left, and there is a greater concentration of reactants than products
Given the following reaction: XBO3(s) XO(s) + BO2(g). If the concentration of BO2 at equilibrium was 2.0 M, what is the equilibrium constant (K)? Select one: a. Not enough information is given b. 1.0 M c. 2.0 M d. 0.50 M
Given the following exothermic, equilibrium reaction: 3 H2(g) + N2(g) 2 NH3(g). Using Le Chatelier's Principle, which of the following changes would shift the equilibrium toward more production of NH3? Select one: a. Adding a catalyst b. Adding heat c. Increasing the volume of the container d. Removing NH3