Given the following reaction: CH4+ 2O2 -> CO2 + 2H2O, How many grams of CO2 will be produced from 15.0 g of CH4 and 114 g of O2? round to 3 significant figures

Question

Given the following reaction: CH4+ 2O2 -> CO2 + 2H2O, How many grams of CO2 will be produced from 15.0 g of CH4 and 114 g of O2? round to 3 significant figures

Answer 1

We see that O2 is in excess, so we can use our balanced equation to go from g of CH₄ to g of CO₂

1. check that equation is balanced (yes, balanced)
2. Use molar mass to go from g of CH₄ to mol of CH₄
3. 15.0 g CH₄ (1 mol CH₄/16.05 g CH₄) = 0.9346 mol CH₄
4. Use mole ratios to go from moles CH₄ to moles CO₂
5. Mole ratio is 1:1, so it is 0.9346 mol CO₂
6. Use molar mass to go from moles CO₂ to grams of CO₂
7. 0.9346 mol CO₂*(44.01 g CO₂ / 1 mol CO₂) = 41.1 g CO₂

Answer 2

15 g of CH4 only consumes 60 g of O2, so the O2 is way over excess. From 15 g of CH4, it will produce 15/16 x 44 g of CO2, namely, 41.25 grams of CO2, ROUND up to 41.3 g