The combustion of glucose is represented by the following balanced equation: C6H12O6+6 O2→6 H2O+6 CO2. The reaction uses 1 gram of both C6H12O6 and O2. What is the percent yield if 0.45 g of H2O is produced? a 0.558% b 100% c 0.31% d 80%

Answer : The correct option is, (d) 80 %

Solution : Given,

Mass of = 1 g

Mass of = 1 g

Molar mass of = 180 g/mole

Molar mass of = 32 g/mole

Molar mass of = 18 g/mole

First we have to calculate the moles of and .

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

From the balanced reaction we conclude that

As, 6 mole of react with 1 mole of

So, 0.0312 moles of react with moles of

From this we conclude that, is an excess reagent because the given moles are greater than the required moles and is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of

From the reaction, we conclude that

As, 6 mole of react to give 6 mole of

So, 0.0312 mole of react to give 0.0312 mole of

Now we have to calculate the mass of

Theoretical yield of = 0.562 g

Experimental yield of = 0.45 g

Now we have to calculate the percent yield of the reaction.

Therefore, the percent yield of reaction is, 80 %

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explanation:

b is the correct answer

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