To produce 12.0 grams of carbon dioxide, how many grams of water are needed?

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Without the reaction to which you are referring to, it is difficult to solve this question. I will use a representative chemical reaction to explain the process that will help you with your particular reaction.

First of all, in most of the reaction, carbon dioxide and water are typically on the same side of the equation. That is, either both are reactants or both are products.

Let's try an example reaction. In the respiration reaction, glucose breaks down into carbon dioxide and water as per the following reaction:

C6H12O6 + 6O2 -> 6CO2 + 6H2O + energy.

In this reaction, 1 mole of glucose reacts with 6 moles of oxygen to generate 6 moles of carbon dioxide and 6 moles of water, along with energy.

Let's say 12.0 g of carbon dioxide is formed and we are required to find how much oxygen is needed for it.

From the equation, 6 moles of carbon dioxide are generated when 6 moles of oxygen are consumed. In other words, for 1 mole of carbon dioxide produced, 1 mole of oxygen is consumed.

12 g of carbon dioxide is equivalent to 12/44 = 0.27 moles of carbon dioxide and will be produced on the consumption of 0.27 moles of oxygen, which is equal to 0.27 x 32 = 8.64 g.

Thus, 8.64 g of oxygen is needed to produce 12 g of carbon dioxide by this given reaction.

Hopefully, you can use this case as an example for your own particular reaction.

Good luck.

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