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What [Cl-], in moles per liter, would be required to force the oxidation of chloride ions...

What [Cl-], in moles per liter, would be required to force the oxidation of chloride ions according to the nonspontaneous reaction equation below at 25.0 °C, when the [Br-] = 1.00x10-5 M and [Cl2] = 1.00 M? Enter your answer to the thousandths place.

Br2(l) + 2Cl-(aq) ⟶ Cl2(g) + 2Br-(aq) E°cell = -0.292 V

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