How many moles of oxygen are required to produce 37.15 g CO2?

To calculate the number of moles of oxygen required to produce 37.15 g of CO_2, we need to start with the balanced chemical equation for the combustion of carbon-based substances, such as:

C + O_2 → CO_2

This equation indicates that 1 mole of carbon reacts with 1 mole of oxygen to produce 1 mole of carbon dioxide.

Now let's calculate the number of moles of CO_2 produced using the molar mass of CO_2:

Molar mass of CO_2 = 12.01 g/mol (for C) + 2 * 16.00 g/mol (for each O) Molar mass of CO_2 = 12.01 g/mol + 32.00 g/mol Molar mass of CO_2 = 44.01 g/mol

Number of moles of CO_2 produced = Mass of CO_2 / Molar mass of CO_2 Number of moles of CO_2 = 37.15 g / 44.01 g/mol Number of moles of CO_2 = 0.844 moles (rounded to three decimal places)

The balanced chemical equation indicates that the mole ratio between O_2 and CO_2 is 1:1. So, 0.844 moles of CO_2 would be produced from 0.844 moles of O_2.

Therefore, 0.844 moles of oxygen gas (O_2) are required to produce 37.15 g of carbon dioxide (CO_2).