how many grams of CO2 could be produced from 100.0 grams of CH4?

CH4 + 2O2 -> CO2 + 2H2O

To determine the number of grams of CO2 that could be produced from 100.0 grams of CH4, we need to use stoichiometry.

1. Start by writing the balanced chemical equation for the reaction:
CH4 + 2O2 -> CO2 + 2H2O

2. Calculate the molar mass of CH4 (methane) and CO2 (carbon dioxide):
The molar mass of CH4 = 12.01 g/mol (C) + 4 * 1.01 g/mol (H) = 16.04 g/mol
The molar mass of CO2 = 12.01 g/mol (C) + 2 * 16.00 g/mol (O) = 44.01 g/mol

3. Convert the mass of CH4 (given as 100.0 grams) to moles:
Moles of CH4 = mass / molar mass = 100.0 g / 16.04 g/mol = 6.2268 mol (rounded to four decimal places)

4. Use the stoichiometric coefficients from the balanced equation to determine the moles of CO2 produced:
From the equation, we can see that 1 mole of CH4 produces 1 mole of CO2.
Therefore, the moles of CO2 produced will also be 6.2268 mol.

5. Convert the moles of CO2 to grams using the molar mass of CO2:
Grams of CO2 = moles * molar mass = 6.2268 mol * 44.01 g/mol = 273.83 g (rounded to two decimal places)

Therefore, approximately 273.83 grams of CO2 could be produced from 100.0 grams of CH4.

from the balanced equation, it is a one mole cO2 per one mole methane.

molesmethane=100/16
gramsCO2=100/16 * 44 g