calculate the number of moles and mass
of methane (ch4) required to produce 11 kg of carbondoxide(co2) when combusted ?
CH4 + 2O2 ==> CO2 + 2H2O
mols CO2 = 11,000/molar mass CO2 = ?
Using the coefficients in the balanced equation, convert mols CO2 to mols CH4.
Now grams CH4 = mols CH4 x molar mass CH4
To calculate the number of moles and mass of methane required to produce 11 kg of carbon dioxide when combusted, we need to determine the balanced chemical equation for the combustion of methane.
The balanced chemical equation for the combustion of methane (CH4) is as follows:
CH4 + 2O2 -> CO2 + 2H2O
From the balanced equation, we can see that one molecule of methane produces one molecule of carbon dioxide. So, the stoichiometric ratio of methane to carbon dioxide is 1:1.
Now, we can calculate the number of moles of methane required:
Step 1: Convert the mass of carbon dioxide to moles.
11 kg of carbon dioxide is equal to 11000 grams (since 1 kg = 1000 g).
Using the molar mass of carbon dioxide (CO2) which is approximately 44 g/mol, we can calculate the number of moles.
Number of moles = mass/molar mass = 11000 g / 44 g/mol = 250 moles.
Step 2: Since the stoichiometric ratio of methane to carbon dioxide is 1:1, the number of moles of methane required is also 250 moles.
To calculate the mass of methane required:
Step 1: Convert the number of moles of methane to mass.
Using the molar mass of methane (CH4) which is approximately 16 g/mol, we can calculate the mass.
Mass = number of moles × molar mass = 250 moles × 16 g/mol = 4000 grams = 4 kg.
Therefore, to produce 11 kg of carbon dioxide when combusted, we need 250 moles (or 4 kg) of methane.