need chemistry help

Question

How many moles of hydrogen carbonate need to decompose to produce 0.75x10^24 moles files of carbon dioxide if water is the only other product?

Answer 1

I will not be providing the direct answer for this question, but I will lay out the steps to solve the question.

First we need to have a balanced equation. That is almost always the first step in any chemical reaction.

We start with hydrogen carbonate or (H2CO3) and we know we make carbon dioxide (CO2) as well as water (H2O) from the question

Let's set up the reaction

H2CO3 --> CO2 + H2O

First we need to determine what isn't balanced

H? 2 on each side. Balanced

C? 1 on each side. Balanced

O? 3 on each side. Balanced.

Turns out the equation is already balanced! Nice that makes things simpler.

First I have to ask if the 0.75 x 10^24 moles is accurate. It seems more likely that it would be molecules. I'm going to continue on as if it were molecules.

To determine the number of moles created we need to divide the number of molecules formed by the number of units in a mole (6.022 * 10^23) or the following equation.

0.75* 10^ 24 molecules/ 6.022 * 10^23 molecules/mol.

From that you can determine the amount of CO2 produced. And from the amount of CO2 produced you can figure out the amount of H2CO3 needed. As the balanced equation is 1 to 1 to 1 then the stoichiometry would have the moles of product equal to the moles of reactant.

Let me know if you have any questions,

Dr. D