Chemical Equilibrium
Quiz
- Which of the following is true for a reaction at equilibrium?
- The rate of the forward reaction is greater than the rate of the reverse reaction.
- The rate of the forward reaction is less than the rate of the reverse reaction
- The rate of the forward reaction is equal to the rate of the reverse reaction.
- The concentrations of reactants and products are equal.
- What does the equilibrium constant (K) indicate about a reaction?
- The amount of reactants at equilibrium
- The amount of products at equilibrium
- The ratio of the concentrations of products to reactants at equilibrium
- The speed of the reaction
- Which of the following expressions correctly represents the equilibrium constant \( K_c \) for the reaction \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \)?
- \( K_c = \frac{[N_2][H_2]^3}{[NH_3]^2} \)
- \( K_c = \frac{[NH_3]^2}{[N_2][H_2]^3} \)
- \( K_c = \frac{[NH_3]}{[N_2][H_2]^3} \)
- \( K_c = \frac{[N_2][H_2]^3}{[NH_3]} \)
- Which of the following factors does not affect the equilibrium position of a reaction?
- Concentration of reactants
- Temperature
- Pressure
- Catalyst
- What will happen to the equilibrium position if the concentration of a reactant is increased?
- It will shift to the right
- It will shift to the left
- It will remain unchanged
- It will reach a new equilibrium at the same position
- According to Le Chatelier's principle, what is the effect of increasing the temperature on an exothermic reaction at equilibrium?
- The equilibrium will shift to the right
- The equilibrium will shift to the left
- There will be no change
- The rate of the reaction will decrease
- For the reaction \( 2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) \), what is the effect of increasing the pressure on the equilibrium position?
- It shifts to the left
- It shifts to the right
- No effect
- The reaction rate increases
- In a chemical equilibrium, the concentration of products and reactants are
- Always equal
- Always constant
- Continuously changing
- None of the above
- None of the above
- \( K_p = \frac{P_{CH_3OH}}{P_{CO}P_{H_2}^2} \)
- \( K_p = \frac{P_{CO}P_{H_2}^2}{P_{CH_3OH}} \)
- \( K_p = \frac{P_{CO}}{P_{CH_3OH}P_{H_2}^2} \)
- \( K_p = \frac{P_{CO}}{P_{CH_3OH}P_{H_2}^2} \)
- If the value of \( K_c \) is very large, what does this indicate about the reaction?
- The reactants are favored
- The products are favored
- The reaction is at equilibrium
- The reaction is very fast
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