Consider the oxidation of sodium metal to sodium oxide described by the balanced equation: 4 na + o2? 2 na2o. if 2.55 mol of sodium reacts, what is the percent yield if the reaction actually gives 75.0 g of na2o?

Question

Keenan

Chemistry

9 October, 03:23

Consider the oxidation of sodium metal to sodium oxide described by the balanced equation: 4 na + o2? 2 na2o. if 2.55 mol of sodium reacts, what is the percent yield if the reaction actually gives 75.0 g of na2o?

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Azul Green · Answer 1

The balanced reaction:

4Na + O2 = 2Na2O

We use the relation of the substances and the amount of sodium to determine the theoretical yield of the reaction. This yield is the amount produced if all the reactant is consumed.

2.55 mol Na (2 mol Na2O / 4 mol Na) (61.98 g / 1 mol) = 79.02 g Na2O

Percent yield = 75.0 / 79.02 x 100 = 94.91%