Question

Methane burns in the presence of oxygen to form carbon dioxide and water. 1st attempt A sealed chamber contains 7.00 gCH_4 and 11.5 gO_2 . The mixture is ignited producing CO_2 and H_2O. How many grams of CO_2 are produced?

Answer 1

To find the grams of carbon dioxide produced, we need to determine the number of moles of methane available in the chamber and then use the mole ratio from the balanced equation. Given that the chamber contains 7.00 g of CH4, we can calculate the number of moles by dividing the mass by the molar mass.

Step-by-step explanation:

The balanced equation for the combustion of methane is:

CH4 + 2O2 → CO2 + 2H2O

From the balanced equation, we can see that 1 mole of methane reacts with 2 moles of oxygen to produce 1 mole of carbon dioxide and 2 moles of water.

To find the grams of carbon dioxide produced, we need to determine the number of moles of methane available in the chamber and then use the mole ratio from the balanced equation.

Given that the chamber contains 7.00 g of CH4, we can calculate the number of moles by dividing the mass by the molar mass.

Molar mass of CH4 = 12.01 g/mol (C) + 4(1.01 g/mol) (H) = 16.05 g/mol

Number of moles of CH4 = 7.00 g / 16.05 g/mol = 0.436 mol

According to the balanced equation, we have a 1:1 mole ratio between CH4 and CO2. Therefore, the number of moles of CO2 produced is also 0.436 mol.

To find the mass of CO2 produced, we multiply the number of moles by the molar mass of CO2 (44.01 g/mol).

Mass of CO2 produced = 0.436 mol * 44.01 g/mol = 19.15 g

Therefore, 19.15 grams of CO2 are produced.