Write the balanced reaction using the fewest whole number coefficients to describe the reaction between gaseous hydrogen and gaseous oxygen. then use the information to solve the problem below: in one experiment, 14.0 moles of hydrogen and 10 moles of oxygen were reacted to produce 1.33 moles of h2o. calculate the % yield.

The percentage yield of water is 9.5 %

Explanation:

We are given:

Moles of hydrogen = 14 moles

Moles of oxygen = 10 moles

The chemical equation for the formation of water from hydrogen and oxygen follows:

By Stoichiometry of the reaction:

2 moles of hydrogen gas reacts with 1 mole of oxygen gas

So, 14 moles of hydrogen gas will react with = of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent

Thus, hydrogen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of hydrogen gas produces 2 moles of water

So, 14 moles of hydrogen gas will produce = of water

To calculate the percentage yield of water, we use the equation:

Experimental yield of water = 1.33 moles

Theoretical yield of water = 14 moles

Putting values in above equation, we get:

Hence, the percent yield of the water is 9.5 %.

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