(a)
Interpretation:
Reaction mechanism for the formation of
(a)
Explanation of Solution
Given reaction,
Write the stoichiometric equation by cancelling species that are present in both sides and add up the remaining species,
(b)
Interpretation:
Reaction mechanism for the formation of
Concept Introduction:
Equilibrium constant
Equilibrium constant
Consider the reaction where A reacts to give B.
On rearranging,
Where,
(b)
Explanation of Solution
Given reaction,
The rate of forward reaction is equals to the rate of reverse reaction at equilibrium.
Write the equilibrium constant expression for the first step,
Write the equilibrium constant expression for the second step,
(c)
Interpretation:
Reaction mechanism for the formation of
Concept Introduction:
Refer part (b)
(c)
Explanation of Solution
Given reaction,
Write the stoichiometric equation, by cancelling species that are present in both sides and add up the remaining species,
Write the overall stoichiometric equilibrium constant expression,
(d)
Interpretation:
Reaction mechanism for the formation of
Concept Introduction:
Refer part (b)
(d)
Explanation of Solution
Given reaction,
Write the stoichiometric equation, by cancelling species that are present in both sides and add up the remaining species,
Write the overall stoichiometric equilibrium constant expression,
Therefore, the result obtained in part (c) confirms the statement that the equilibrium constant can be obtained by taking the product of the rate constants for all forward steps
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Chapter 12 Solutions
Chemistry: The Molecular Science
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- Consider the elementary reactions and their rate constants. kf = 4.99 × 10–2s-1 k, = 3.67 × 10-' s-' A(g) + B(g) → C(g) + D(g) C(g) + D(g) A(g) + B(g) What is the equilibrium constant (K) of the following generic reaction? A(g) + B(g) = C(g) + D(g) Ke = Which statement correctly describes the partial pressures of the reactants and products at equilibrium? The partial pressures of the reactants are greater than the partial pressures of the products at equilibrium. The partial pressures of the products are greater than the partial pressures of the reactants at equilibrium. The partial pressures of the reactants and products are equal at equilibrium.arrow_forwardFor the reaction 12(g) +Br₂(g) →21Br(g) Ke=280 at 150 °C. Suppose that 0.520 mol IBr in a 2.00-L flask is allowed to reach equilibrium at 150 °C. Esc Type here to search WE in R ▼ What is the equilibrium concentration of I₂? Express your answer in moles per liter to three signifi IVE ΑΣΦ [12] = 0.012 Submit Previous Answers Request Answer * Incorrect; Try Again; 7 attempts remaining Part C What is the equilibrium concentration of Br₂? Express your answer in moles per liter to three significant figu ΕΧΕΙ ΑΣΦ Br₂ = 0.0120 Submit Previous Answers Request Answer ? 8 Marrow_forwardH₂O(g) + CO(g) = H₂(g) + CO₂(g) Which of the following statements are true and which are false. The rate at which equilibrium is established can be inferred from the magnitude of the equilibrium constant. indefinite period of time ¹C would still be found only in the CO molecules and not in CO₂. When Q < K the system will spontaneously shift to the left. At equilibrium, the overall composition of the reaction mixture is constant. two vessels are equivalent. 2arrow_forward
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