Question

The molar mass of carbon dioxide (CO2) is 44.01 g/mol. The molar mass of water (H2O) is 18.01 g/mol. A reaction uses 528 g of CO2. How many moles of water are used in this reaction?

Answer 1

12 moles

Step-by-step explanation:

The reaction will form carbonic acid:

CO₂ + H₂O ⇒ H₂CO₃

For 528 g of CO₂, the number of moles (n) will be:

n = mass/molar mass

n = 528/44.01

n = 12 moles of CO₂

The stoichiometry is 1 mol of CO₂ reacts with 1 mol of H₂O, so 12 moles of CO₂ need 12 moles of H₂O.

Answer 2

The reaction that results from this is:

H2O + CO2 --> H2CO3

Ratio between water and CO2 is 1:1. So we can say that for every Mole of CO2, we need 1 Mole of water to produce 1 Mole of H2CO3. Thus as n=m/M we can find n = 528/44.01 = 11.997 ~ 12Mol.

Therefore, we need 12 moles of water.