If a reaction has a percentage yield of 83.0%, what mass of methane can be obtained from 1150 g of carbon?
2 C(s) + 2 H2O(l) CH4(g) + CO2(g)
*Answer in grams*
mols C = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols C to mols CH4.
?C x (1 mol CH4/2 mols C) = ? mols CH4.
Convert mols CH4 to grams by g = mols CH4 x molar mass CH4 = ? g CH4. This is for 100% yield.
But you will get only 83.0% of that so
g for 100% yield x 0.830 = ? g for 83^ yield.
To find the mass of methane obtained from 1150 g of carbon, we first need to calculate the moles of carbon using its molar mass. Then, we can use the balanced chemical equation to relate the moles of carbon to the moles of methane produced, and finally convert it to grams.
1. Calculate the moles of carbon:
The molar mass of carbon is 12.01 g/mol.
Number of moles of carbon = Mass of carbon / Molar mass of carbon
Number of moles of carbon = 1150 g / 12.01 g/mol
2. Use the balanced chemical equation to relate the moles of carbon to moles of methane:
According to the balanced chemical equation, 2 moles of carbon react to produce 1 mole of methane:
2 moles of C(s) → 1 mole of CH4(g)
3. Calculate the moles of methane:
Number of moles of methane = Number of moles of carbon × (1 mole of CH4/2 moles of C)
Number of moles of methane = (1150 g / 12.01 g/mol) × (1 mol / 2 mol)
4. Convert moles of methane to grams:
Mass of methane = Number of moles of methane × Molar mass of methane
The molar mass of methane (CH4) is 16.04 g/mol.
Mass of methane = (1150 g / 12.01 g/mol) × (1 mol / 2 mol) × 16.04 g/mol
By performing the above calculations, you can determine the mass of methane obtained from 1150 g of carbon.