For the reaction 2H+(aq)+BrO4−(aq)+2Ce3+(aq)\rightarrow \mathrm{BrO}_{3}^{-}(\mathrm{aq})+2 \mathrm{Ce}^{4+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}), \quad E_{\mathrm{cell}}^{\circ}=−0.017V, answer the following questions:(a) Can a solution be prepared at 298 K that has [BrO4−]=[Ce4+]=0.675M,[BrO3−]=[Ce3+]=0.600 \mathrm{M}and\mathrm{pH}=1 ?$(b) If not, in which direction will a reaction occur?

Question

For the reaction 2H+(aq)+BrO4−​(aq)+2Ce3+(aq)\rightarrow \mathrm{BrO}_{3}^{-}(\mathrm{aq})+2 \mathrm{Ce}^{4+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}), \quad E_{\mathrm{cell}}^{\circ}=−0.017V, answer the following questions:(a) Can a solution be prepared at 298 K that has [BrO4−​]=[Ce4+]=0.675M,[BrO3−​]=[Ce3+]=0.600 \mathrm{M}and\mathrm{pH}=1 ?$(b) If not, in which direction will a reaction occur?

Filo · Accepted Answer

Step by Step Solution:
Step 1. Identify the given reaction: 2 H⁺(aq) + BrO₄⁻(aq) + 2 Ce³⁺(aq) → BrO₃⁻(aq) + 2 Ce⁴⁺(aq) + H₂O(l)

Step 2. Determine the standard cell potential: E°cell = -0.017 V

Step 3. Calculate the reaction quotient, Qc, using the given concentrations: Qc = [BrO₄⁻][Ce³⁺]²/[H⁺]²

Step 4. Determine the reaction quotient, Qc, using the given concentrations for the products and reactants to check if the reaction is at equilibrium or not: Qc = [BrO₃⁻][Ce⁴⁺]² /[H⁺]²[Ce³⁺]²

Step 5. Compare Qc and Kc to determine if the reaction is at equilibrium or not. If Qc  Kc, the reaction will shift to the left to reach equilibrium. If Qc = Kc, the reaction is at equilibrium: Kc = 1.6 × 10⁻¹⁴ (at 298 K)

Step 6. Answer part (a): Evaluate whether the given concentrations and pH values result in Qc being smaller, larger, or equal to Kc. If Qc is smaller than Kc, the reaction will shift to the right to reach equilibrium, and therefore a solution with the given concentrations and pH can be prepared. If Qc is not smaller than Kc, a solution with the given concentrations and pH cannot be prepared.

Step 7. Answer part (b): If Qc is not smaller than Kc, the reaction will shift to the left to reach equilibrium. The concentrations of Ce⁴⁺ and BrO₃⁻ will decrease, while the concentrations of Ce³⁺, BrO₄⁻, and H⁺ will increase until Qc = Kc is reached.

Final Answer:
a) No, a solution cannot be prepared at 298 K with the given concentrations and pH. b) The reaction will shift to the left to reach equilibrium.

Question Text	For the reaction $2 H^{+} (aq) + BrO_{4}^{-} (aq) + 2 Ce^{3 +} (aq)$ \rightarrow \mathrm{BrO}_{3}^{-}(\mathrm{aq})+2 \mathrm{Ce}^{4+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}), \quad E_{\mathrm{cell}}^{\circ}= $- 0.017 V,$ answer the following questions:(a) Can a solution be prepared at 298 K that has $[BrO_{4}^{-}] = [Ce^{4 +}] = 0.675 M, [BrO_{3}^{-}] = [Ce^{3 +}] =$ 0.600 \mathrm{M} $an d$ \mathrm{pH}=1 ?$(b) If not, in which direction will a reaction occur?
Topic	All topics
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1

Text solutionVerified

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