Answer: 17.6×10^-3g of CO2
Explanation:
We first look at the stoichiometry of the balanced reaction equation. One mole of methane produces one mole of carbon dioxide. Hence 16g of methane yields 44g of carbon dioxide. If we now composed this with the given 6.40×10^-3g of methane as shown in the solution attached, we obtain the answer stated above.
Answer:
The mass of CO2 = 0.0176 grams
Explanation:
Step 1: Data given
Mass of methane = 6.40 *10^-3 grams
Step 2: The balanced equation
CH4 + 2O2 → CO2 + 2H2O
Step 3: Calculate moles of CH4
Moles CH4 = mass CH4 / molar mass CH4
Moles CH4 = 6.40 *10^-3 grams / 16.04 g/mol
Moles CH4 = 3.99*10^-4 moles
Step 4: Calculate moles of CO2
For 1 mol O2 we need 2 moles O2 to produce 1 mol CO2 and 2 moles H2O
For 3.99 *10^-4 moles CH4 we'll have 3.99 *10^-4 moles of CO2
Step 5: Calculate mass of CO2
Mass CO2 = moles CO2 * molar mass CO2
Mass CO2 = 3.99 *10^-4 moles * 44.01 g/mol
Mass CO2 = 0.0176 grams
The mass of CO2 = 0.0176 grams
