CH4 + 2O2 = CO2 + 2H2O
Starting with 13.6 g of CH4, calculate the mass in grams of CO2 produced if there is enough O2 gas to react with all of the CH4
Just follow the steps in the worked example.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To calculate the mass of CO2 produced, we need to use stoichiometry, which is the relationship between the balanced chemical equation and the moles of each substance involved.
1. Calculate the molar mass of CH4:
- Carbon (C) has a molar mass of 12.01 g/mol
- Hydrogen (H) has a molar mass of 1.01 g/mol
So the molar mass of CH4 is 12.01 g/mol + (4 * 1.01 g/mol) = 16.05 g/mol.
2. Convert the mass of CH4 to moles:
Divide the given mass of CH4 by its molar mass:
13.6 g CH4 / 16.05 g/mol CH4 = 0.848 mol CH4.
3. Use the coefficients in the balanced chemical equation to determine the mole ratio between CH4 and CO2:
From the balanced equation: 1 mol CH4 reacts to produce 1 mol CO2.
Therefore, 0.848 mol CH4 will produce 0.848 mol CO2.
4. Calculate the mass of CO2 produced:
Multiply the moles of CO2 by its molar mass:
0.848 mol CO2 * 44.01 g/mol CO2 = 37.25 g CO2.
Therefore, if 13.6 g of CH4 reacts with enough O2 gas to produce CO2, the mass of CO2 produced will be 37.25 g.