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Questions and Answers
Which expression correctly represents the equilibrium constant for the heterogeneous reaction: $aA(s) + bB(g) \rightleftharpoons cC(g) + dD(s)$?
Which expression correctly represents the equilibrium constant for the heterogeneous reaction: $aA(s) + bB(g) \rightleftharpoons cC(g) + dD(s)$?
- $K = \frac{[A]^a[B]^b}{[C]^c[D]^d}$
- $K = \frac{[C]^c[D]^d}{[A]^a[B]^b}$
- $K = \frac{[C]^c[D]^d}{[B]^b}$ (correct)
- $K = [C]^c[D]^d$
- $K = \frac{[C]^c}{[B]^b}$
For the reaction $CO_2(aq) + H_2O(l) \rightleftharpoons H_2CO_3(aq)$ at equilibrium, which statement accurately describes the rates of the forward and reverse reactions?
For the reaction $CO_2(aq) + H_2O(l) \rightleftharpoons H_2CO_3(aq)$ at equilibrium, which statement accurately describes the rates of the forward and reverse reactions?
- The rate of the reverse reaction is faster than the rate of the forward reaction.
- The reaction stops completely.
- The rate of the forward reaction is faster than the rate of the reverse reaction.
- The rate of the forward reaction equals the rate of the reverse reaction. (correct)
Given the reaction $2NOBr(g) \rightleftharpoons 2NO(g) + Br_2(g)$, with $\Delta H_{rxn}° = 30 \frac{kJ}{mol}$, which change will shift the equilibrium to the left?
Given the reaction $2NOBr(g) \rightleftharpoons 2NO(g) + Br_2(g)$, with $\Delta H_{rxn}° = 30 \frac{kJ}{mol}$, which change will shift the equilibrium to the left?
- Remove some NO.
- Add more NOBr. (correct)
- Increase the temperature.
- Remove some $Br_2$.
- Increase the container volume.
For the reaction $2A(aq) + B(aq) \rightleftharpoons 3C(aq)$, the equilibrium constant $K_c = 100$. If the reaction quotient $Q_c = 50$, what will occur to reach equilibrium?
For the reaction $2A(aq) + B(aq) \rightleftharpoons 3C(aq)$, the equilibrium constant $K_c = 100$. If the reaction quotient $Q_c = 50$, what will occur to reach equilibrium?
Consider the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$. If the concentration of $SO_2$ is increased at equilibrium, what change will occur to the equilibrium position?
Consider the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$. If the concentration of $SO_2$ is increased at equilibrium, what change will occur to the equilibrium position?
For the reaction $X(aq) + Y(aq) \rightleftharpoons 2Z(aq)$, the initial concentrations are $[X] = 0.3 M$, $[Y] = 0.3 M$, and $[Z] = 0 M$. Given that the equilibrium constant $K_c = 250$, which of the following is closest to the equilibrium concentration of Z?
For the reaction $X(aq) + Y(aq) \rightleftharpoons 2Z(aq)$, the initial concentrations are $[X] = 0.3 M$, $[Y] = 0.3 M$, and $[Z] = 0 M$. Given that the equilibrium constant $K_c = 250$, which of the following is closest to the equilibrium concentration of Z?
For the reaction $2X(aq) + Y(aq) \rightleftharpoons Z(s)$, the concentrations at the start are $[X] = 0.1 M$, $[Y] = 0.2 M$, and $[Z] = 0.3 M$. What is the value of the reaction quotient, $Q_c$?
For the reaction $2X(aq) + Y(aq) \rightleftharpoons Z(s)$, the concentrations at the start are $[X] = 0.1 M$, $[Y] = 0.2 M$, and $[Z] = 0.3 M$. What is the value of the reaction quotient, $Q_c$?
For the reaction $CO(g) + H_2O(g) \rightleftharpoons CO_2(g) + H_2(g)$, if $K_p = 0.1$ at a temperature of 300 K, what is the correct setup to calculate $K_c$ for this reaction?
For the reaction $CO(g) + H_2O(g) \rightleftharpoons CO_2(g) + H_2(g)$, if $K_p = 0.1$ at a temperature of 300 K, what is the correct setup to calculate $K_c$ for this reaction?
At 400°C, $K = 64$ for the equilibrium $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$. If 3.00 mol of $H_2$ and 3.00 mol of $I_2$ are introduced into an empty 4.0 L vessel, what is the approximate equilibrium concentration of $HI$ at 400°C?
At 400°C, $K = 64$ for the equilibrium $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$. If 3.00 mol of $H_2$ and 3.00 mol of $I_2$ are introduced into an empty 4.0 L vessel, what is the approximate equilibrium concentration of $HI$ at 400°C?
At 700 K, the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$ has an equilibrium constant $K = 4.3 \times 10^6$, and the current concentrations are: $[SO_2] = 0.10 M$, $[SO_3] = 10. M$, $[O_2] = 0.10 M$. Which statement accurately describes the system?
At 700 K, the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$ has an equilibrium constant $K = 4.3 \times 10^6$, and the current concentrations are: $[SO_2] = 0.10 M$, $[SO_3] = 10. M$, $[O_2] = 0.10 M$. Which statement accurately describes the system?
Flashcards
Equilibrium Constant Expression (Kc)
Equilibrium Constant Expression (Kc)
Expression representing the ratio of products to reactants at equilibrium, considering only gaseous and aqueous species. Solids and liquids have constant activity and are excluded.
Equilibrium Condition
Equilibrium Condition
At equilibrium, the forward and reverse reaction rates are equal, indicating a dynamic state where the net change in concentrations is zero.
Qc vs Kc
Qc vs Kc
Kc is the equilibrium constant calculated from concentrations, while Qc is the reaction quotient calculated from initial concentrations. Comparing Qc to Kc predicts the direction a reversible reaction will shift to reach equilibrium.
Le Chatelier's Principle: Increase SO2
Le Chatelier's Principle: Increase SO2
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Volume Change on Equilibrium
Volume Change on Equilibrium
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Temperature Effects on Equilibrium
Temperature Effects on Equilibrium
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Study Notes
- Active & Collaborative Learning Worksheet
Equilibrium Constant Expression
- For a heterogeneous equilibrium aA(s) + bB(g) = cC(g) + dD(s), the equilibrium constant expression is [C]c[D]d/[B]b.
- Solid and liquid concentrations are not included in the equilibrium constant expression.
Equilibrium
- At equilibrium for the reaction CO2(aq) + H2O(l) = H2CO3(aq), the rate of the forward reaction equals the rate of the reverse reaction.
Equilibrium Shift
- For the reaction 2NOBr(g) = 2NO(g) + Br2(g) with ΔH°rxn = 30 kJ/mol, equilibrium will shift to the left if the temperature is decreased.
Reaction Direction
- For the reaction 2A(aq) + B(aq) = 3C(aq), with Kc = 100 and Qc = 50, the reaction will proceed in the forward direction to reach equilibrium.
- When Qc < Kc, the reaction proceeds in the forward direction.
Equilibrium Position
- Given the reaction 2SO2(g) + O2(g) = 2SO3(g), if the concentration of SO2 is increased by adding more SO2, the equilibrium position shifts to the right, increasing the concentration of SO3.
Equilibrium Concentrations
- For the reaction X(aq) + Y(aq) = 2Z(aq), with initial concentrations [X] = 0.3 M, [Y] = 0.3 M, and [Z] = 0 M, and Kc = 250, we need to calculate the equilibrium concentrations using an ICE table.
Reaction Quotient
- For the reaction 2X(aq) + Y(aq) = Z(s), with initial concentrations [X] = 0.1 M, [Y] = 0.2 M, and [Z] = 0.3 M, the reaction quotient Qc can be calculated.
Kp and Kc Relationship
- For the reaction CO(g) + H2O(g) = CO2(g) + H2(g), if Kp = 0.1 atm at a temperature of 300 K, then Kc can be calculated using the relationship Kp = Kc(RT)^Δn, where Δn is the change in the number of moles of gas.
Equilibrium Concentration of HI
- At 400°C, K = 64 for the equilibrium H2(g) + I2(g) = 2HI(g). with 3.00 mol H2 and 3.00 mol I2 introduced into an empty 4.0 L vessel, the equilibrium concentration of HI at 400°C can be found using an ICE table.
Reaction Quotient vs. Equilibrium
- At 700 K, the reaction 2SO2(g) + O2(g) = 2SO3(g) has the equilibrium constant K = 4.3 × 10^6, with [SO2] = 0.10 M; [SO3] = 10. M; [O2] = 0.10 M, Q < K, the reaction proceeds from left to right to reach equilibrium
- If Q > K, the reaction proceeds from right to left to reach equilibrium, and if Q = K, the reaction is currently at equilibrium.
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