A)What mass of carbon dioxide is produced from the complete combustion of 7.00×10−3 g of methane?
B)What mass of oxygen is needed for the complete combustion of 7.00×10−3 g of methane?
To answer both questions, we need to use the balanced equation for the combustion of methane:
CH4 + 2O2 → CO2 + 2H2O
A) To find the mass of carbon dioxide produced from the complete combustion of methane, we can use stoichiometry.
Step 1: Calculate the molar mass of methane (CH4):
C = 1 carbon atom = 12.01 g/mol
H = 4 hydrogen atoms = 1.01 g/mol × 4 = 4.04 g/mol
Molar mass of CH4 = 12.01 g/mol + 4.04 g/mol = 16.05 g/mol
Step 2: Convert the given mass of methane to moles:
Given mass of methane = 7.00×10^(-3) g
Moles of methane = given mass / molar mass = 7.00×10^(-3) g / 16.05 g/mol
Step 3: Use the stoichiometric ratio to find moles of carbon dioxide:
From the balanced equation, the stoichiometric ratio between methane and carbon dioxide is 1:1.
Therefore, moles of carbon dioxide = moles of methane.
Step 4: Convert moles of carbon dioxide to mass:
Mass of carbon dioxide = moles of carbon dioxide × molar mass of CO2
B) To find the mass of oxygen needed for the complete combustion of methane, we can use the stoichiometry from the balanced equation.
Step 1: Calculate the molar mass of oxygen:
O = 2 oxygen atoms = 16.00 g/mol × 2 = 32.00 g/mol
Step 2: Use the stoichiometric ratio to find moles of oxygen:
From the balanced equation, the stoichiometric ratio between methane and oxygen is 1:2.
Therefore, moles of oxygen = 2 × moles of methane.
Step 3: Convert moles of oxygen to mass:
Mass of oxygen = moles of oxygen × molar mass of O2
By following these steps, you can calculate the mass of carbon dioxide produced (A) and the mass of oxygen needed (B) for the complete combustion of methane.
Here is a link that will work all of your stoichiometry problems. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
Write the balanced equation.
CH4+2O2 >> CO2 + 2H20
for each mole of carbon dioxide produced, one mole of methane, and two moles of oxygen is used.
Moles methane: .007/(16.04)