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Questions and Answers
For the reversible reaction $2A(g) + B(g) \rightleftharpoons C(g)$, the equilibrium constant, Kp, is found to be significantly larger than 1. Which statement best describes this system at equilibrium?
For the reversible reaction $2A(g) + B(g) \rightleftharpoons C(g)$, the equilibrium constant, Kp, is found to be significantly larger than 1. Which statement best describes this system at equilibrium?
- The concentration of A and B will be significantly higher than C.
- The concentration of C will be significantly higher than A and B. (correct)
- The partial pressures of A, B, and C will be approximately equal.
- The reaction rate of the forward reaction is significantly slower than the reverse reaction.
Consider the gas-phase equilibrium: $X(g) + 2Y(g) \rightleftharpoons Z(g)$. If the pressure on the system is increased, which way will the equilibrium shift according to Le Chatelier's principle?
Consider the gas-phase equilibrium: $X(g) + 2Y(g) \rightleftharpoons Z(g)$. If the pressure on the system is increased, which way will the equilibrium shift according to Le Chatelier's principle?
- The equilibrium will shift to the right, favoring the product. (correct)
- The equilibrium will not shift, as pressure changes only affect reactions in solution.
- The equilibrium will oscillate back and forth.
- The equilibrium will shift to the left, favoring the reactants.
Which of the following scenarios will NOT cause a shift in the equilibrium position of a reaction?
Which of the following scenarios will NOT cause a shift in the equilibrium position of a reaction?
- Changing the temperature of the system.
- Adding an inert gas to the reaction vessel at constant volume. (correct)
- Increasing the concentration of a reactant.
- Adding a catalyst to the reaction mixture.
For the reaction $A(g) \rightleftharpoons B(g) + C(g)$, $K_c = 2.25$ at a certain temperature. If a 2.0 L flask initially contains 2.0 mol of A, what is the approximate concentration of B at equilibrium?
For the reaction $A(g) \rightleftharpoons B(g) + C(g)$, $K_c = 2.25$ at a certain temperature. If a 2.0 L flask initially contains 2.0 mol of A, what is the approximate concentration of B at equilibrium?
Consider the reaction: $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$. At a certain temperature, $K_c = 100$. If the initial concentrations are $[SO_2] = 2.0 M$, $[O_2] = 1.5 M$, and $[SO_3] = 1.0 M$, which direction will the reaction shift to reach equilibrium?
Consider the reaction: $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$. At a certain temperature, $K_c = 100$. If the initial concentrations are $[SO_2] = 2.0 M$, $[O_2] = 1.5 M$, and $[SO_3] = 1.0 M$, which direction will the reaction shift to reach equilibrium?
For an endothermic reaction, how does increasing the temperature affect the equilibrium constant (K)?
For an endothermic reaction, how does increasing the temperature affect the equilibrium constant (K)?
The reaction $A(g) + B(g) \rightleftharpoons C(g)$ has an equilibrium constant of $K = 0.25$. You introduce 1.0 mol of A and 1.0 mol of B into a 1.0 L container. What is the equilibrium concentration of C?
The reaction $A(g) + B(g) \rightleftharpoons C(g)$ has an equilibrium constant of $K = 0.25$. You introduce 1.0 mol of A and 1.0 mol of B into a 1.0 L container. What is the equilibrium concentration of C?
Which statement is correct regarding the relationship between $K_p$ and $K_c$ for the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$?
Which statement is correct regarding the relationship between $K_p$ and $K_c$ for the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$?
The equilibrium constant for the reaction $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$ is 50 at 448 °C. Starting with 2.0 atm of $H_2$ and 2.0 atm of $I_2$, what is the partial pressure of HI at equilibrium?
The equilibrium constant for the reaction $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$ is 50 at 448 °C. Starting with 2.0 atm of $H_2$ and 2.0 atm of $I_2$, what is the partial pressure of HI at equilibrium?
For the equilibrium $A(g) \rightleftharpoons B(g)$, the initial concentration of A is 1.0 M and the equilibrium concentration of B is 0.4 M. What is the value of the equilibrium constant K?
For the equilibrium $A(g) \rightleftharpoons B(g)$, the initial concentration of A is 1.0 M and the equilibrium concentration of B is 0.4 M. What is the value of the equilibrium constant K?
Flashcards
Chemical Equilibrium
Chemical Equilibrium
State where the rate of forward and reverse reactions are equal, resulting in no net change in reactant and product concentrations.
Equilibrium Constant (K)
Equilibrium Constant (K)
A quantitative measure of the extent to which a reaction proceeds to completion at a given temperature.
Kc
Kc
Equilibrium constant using molar concentrations.
Kp
Kp
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Le Chatelier's Principle
Le Chatelier's Principle
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ICE Table Method
ICE Table Method
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Approximation for Small K
Approximation for Small K
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Reaction Quotient (Q)
Reaction Quotient (Q)
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Q < K
Q < K
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Q > K
Q > K
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Study Notes
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