What mass of carbon dioxide is produced from the complete combustion of 6.40×10−3 gg of methane?

ch4 + o2 --> co2 + 2h2o

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.

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

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