Question

For each of the following balanced chemical equations, calculate how many moles of product(s) would be produced if 0.500 mole of the first reactant were to react completely. You will have 2 different answers for each of these (one for each product).

*Hint: Set up a mole to mole ratio both starting with 0.500 moles

1. CO2g + 4H2g -> CH4g + 2H2Ol

2. C3H8g + 5O2 -> 4H2Ol + 3CO2g​

Answer 1

Step-by-step explanation:

Use the reactant as the baseline for the molar ratios of the other reaction components. In the first reaction, setting the CO2 to 1 mole aloows us to assign relative moles to the other reaction components (ratios of that component to CO2).

Multiply those ratios times the reactant number of moles to find the moles of the other components. For example, 0.5 moles of CO2 will react with (0.5)*(4) moles of O2. It will produce (0.5)*(1) mole of V=CH4 and (0.5)*(2) moles of H2O.

1. CO2g + 4H2g -> CH4g + 2H2Ol

Ratio 1 4 1 2

moles

0.5 2 0.5 1

2. C3H8g + 5O2 -> 4H2Ol + 3CO2g​

Ratio 1 5 4 3

moles

0.5 2.5 2.0 1.5