Chemistry, 24.03.2021 17:20, dumbdumbkylee
Equimolar amounts of Cl2(g) and CO(g) are injected into an evacuated, rigid container, where they react according to the equation below. Cl2(g)+CO(g)⇄COCl2(g) ΔHrxn=−109kJ/molrxn (a) If 7.0 g of CO(g) is consumed in the reaction with excess Cl2(g), how many moles of COCl2(g) are produced? (b) Which element is oxidized in this reaction? Justify your answer in terms of oxidation numbers.
Answers: 3
Chemistry, 22.06.2019 18:00, rodriguezscarlet1713
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Equimolar amounts of Cl2(g) and CO(g) are injected into an evacuated, rigid container, where they re...
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