Chemical Equilibrium And Reactions Test! Trivia Quiz

28 Questions | By Bandon1 | Updated: Mar 21, 2022 | Attempts: 228

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Questions and Answers

1.

The equilibrium constant can be a negative number.
- A.
  
  True
- B.
  
  False
2.

Select the KC equilibrium expression for the following homogeneous gas phase reaction: 2 SO3(g) 2 SO2(g) + O2(g)
- A.
  
  Kc = [SO3] / ([SO2][O2])
- B.
  
  Kc = [SO3]2 / ([SO2]2[O2])
- C.
  
  Kc = [SO2]2 [O2] / [SO3]2
- D.
  
  Kc = [SO2] [O2] / [SO3]
3.

For the following hypothetical equilibrium A (aq) + 2 B (aq) D C (aq) in a solution, what is the value of the equilibrium constant if the concentrations at equilibrium are [A] = 0.500 M, [B] = 0.400 M, and [C] = 0.300 M ?
- A.
  
  3.75
- B.
  
  .267
- C.
  
  .231
- D.
  
  3.00
4.

Consider the Reaction below: 56A + 48B + 3829C <-> 422D + 394EF, the K value is 3 * 10^78, what conclusion can be made?
- A.
  
  The reaction favors the products
- B.
  
  The reaction favors the reactants
- C.
  
  The reaction is at equilibrium
- D.
  
  None of the above
5.

Fill in the blank. The equilibrium constant is a ________ that ________ change for a reaction at a specific T. It is a _______ of a _________ chemical equation at a specific T
- A.
  
  Constant, doesn't, property, balanced
- B.
  
  Constant, does, property, balanced
- C.
  
  Constant, does, function balanced
- D.
  
  Constant, doesn't, function, balanced
6.

Each term is raised to a number that is equivalent to the number of the substance in the balanced equation. This is known as ....
- A.
  
  Law of Mass Action
- B.
  
  Equilibrium Constant
- C.
  
  Equilibrium Constant Expression
- D.
  
  Rate Constant
7.

For the equilibrium CO2(g) + N2(g) D CO(g) + N2O(g), the forward and reverse rate constants at 1200 K are 9.1 x 10-11 M –1 s–1 and 1.5 x 105 M –1 s–1, respectively. What is the value of the equilibrium constant for this reaction?
- A.
  
  6.1 * 10^-16
- B.
  
  7.1 x 10^4
- C.
  
  1.6 x 10 ^15
- D.
  
  1.4 x 10^-5
8.

Kc are used for?
- A.
  
  Homogenous reactions
- B.
  
  Homogenous Gas-phase reaction
- C.
  
  Heterogeneous Reactions
- D.
  
  None of the above.
9.

Kp can be used for both gas-phase and concentration phases since both have the same setup.
- A.
  
  True
- B.
  
  False
10.

Calculate the change in moles in the following reaction: 2A + 4B <-> C + 5B
- A.
  
  0
- B.
  
  -1
- C.
  
  -2
- D.
  
  2
- E.
  
  1
11.

• In a one-liter container, 0.0310 moles of NO2 are in equilibrium with 0.00452 moles of N2O4 at 100 o C according to the following reaction. 2NO2 (g) ⇌ N2O4(g) What’s the Kc of the reaction?
- A.
  
  4.7
- B.
  
  .146
- C.
  
  6.86
- D.
  
  10.5
12.

Kc of a reaction is 4.70 at 100 o C. What’s its Kp? [R = 0.0821 atm K−1 (mol/L)−1]
- A.
  
  .15
- B.
  
  .57
- C.
  
  39
- D.
  
  470
13.

You multiply the reaction A+B <-> C by 2, the K constant will then be doubled.
- A.
  
  True
- B.
  
  False
14.

Suppose the equilibrium constant of the reaction H2 + ½ O2 = H2O is 50. What is the equilibrium constant of the reaction 2H2 + O2 = 2H2O at the same temperature?
- A.
  
  2500
- B.
  
  100
- C.
  
  50
- D.
  
  25
15.

Suppose the equilibrium constant of the reaction N2 + 3H2 = 2NH3 is 100. What is the equilibrium constant of the reaction NH3 = 1/2 N2 + 3/2 H2 at the same temperature?
- A.
  
  .1
- B.
  
  .001
- C.
  
  1
- D.
  
  10
16.

Suppose that reaction A can be written as Rxn_B x 2 + (Reverse of Rxn_C). KA, KB, and KC are the equilibrium constants of reaction A, B, and C, respectively. What is the relationship between KA, KB, and KC?
- A.
  
  KA = (KB) 2 / KC
- B.
  
  KA = (KB) 2 + KC
- C.
  
  KA = KBx2 – KC
- D.
  
  None of the above
17.

Which of the following is not a factor that doesn't change the balance of a chemical equation.
- A.
  
  Mole Change
- B.
  
  Volume
- C.
  
  Temperature
- D.
  
  Pressure
18.

Suppose we take a snapshot of a reaction at some t. A = [1], B = [1], and C = [2]. The reaction is A + B <-> 2C, is the reaction in equilibrium?
- A.
  
  Yes
- B.
  
  No
- C.
  
  Not enough information is given.
- D.
  
  None of the above
19.

K>Q favors?
- A.
  
  Products
- B.
  
  Equilibrium
- C.
  
  Reactants
- D.
  
  None of the answers
20.

In a one-liter container, 0.0310 moles of NO2 are in equilibrium with 0.00452 moles of N2O4 at 100 oC according to the following reaction. Kc of the reaction is 4.70. If the volume of the container is shrunken by half to 0.500 liter while maintaining the same temperature, what is Qc (reaction quotient) right after the volume change? 2NO2 (g) ⇌ N2O4(g)
- A.
  
  2.35
- B.
  
  4.70
- C.
  
  9.40
- D.
  
  11.6
21.

Which of the following is not an effect of changing Q
- A.
  
  Adding more heat
- B.
  
  Adding a product
- C.
  
  Adding the pressure
- D.
  
  Adding more volume
22.

Consider the Reaction: A + B <-> C + D Add more C, the reaction will
- A.
  
  Shift left
- B.
  
  Shift Right
- C.
  
  Shift towards less moles
- D.
  
  Shifts towards more moles
23.

Consider the reaction, A + B <-> C + D The reaction is exothermic, the reaction is then cooled. The reaction shifts?
- A.
  
  Right
- B.
  
  Left
- C.
  
  Towards less moles
- D.
  
  Toward more moles
24.

If CaCO3, a large solid salt, is added to a reaction, CaCO3 is a product in the reaction, what effect does the addition have to the equilibrium constant?
- A.
  
  The reaction will favor the products
- B.
  
  The reaction will favor the reactants
- C.
  
  There will be no effect
- D.
  
  The reaction will be in equilibrium
25.

What do you think the temperature will affect the ammonia synthesis? N2(g) + 3H2(g) ⇌ 2NH3(g) ΔH = −92.4 kJ·mol−1
- A.
  
  Low temperature will help produce more ammonia.
- B.
  
  High temperature will help produce more ammonia.
- C.
  
  Temperature does not affect the ammonia yield.
- D.
  
  None of the above