Using the same unbalanced chemical reaction, what is the theorectical yeild of CO2 if 16.0g of methane reacts with excess oxygen:
CH4(g)+ O2 (g)→ CO2 (g)+ H2O(g)
mols CH4 = grams CH4/molar mass CH4 = ?
Using the coefficients in the balanced equation, covert mols CH4 to mols CO2.
Now convert mols CO2 to grams (I suppose you want it in grams) by grams = mols CO2 x molar mass CO2 = ? This is the theoretical yield in grams.
To find the theoretical yield of CO2 in this chemical reaction, we need to follow these steps:
Step 1: Write down the balanced chemical equation.
Given: CH4(g) + O2(g) → CO2(g) + H2O(g)
Step 2: Calculate the molar mass of methane (CH4).
Carbon (C) has a molar mass of 12.01 g/mol, and Hydrogen (H) has a molar mass of 1.01 g/mol.
Molar mass of methane (CH4) = (1 mol C × 12.01 g/mol) + (4 mol H × 1.01 g/mol) = 16.05 g/mol
Step 3: Calculate the number of moles of methane.
Number of moles = mass of substance ÷ molar mass
Number of moles of CH4 = 16.0 g ÷ 16.05 g/mol ≈ 0.997 mol
Step 4: Determine the stoichiometry of methane to carbon dioxide.
From the balanced equation, we can see that the stoichiometric ratio between CH4 and CO2 is 1:1. This means that for every 1 mole of methane reacted, 1 mole of CO2 is produced.
Step 5: Calculate the theoretical yield of CO2.
The theoretical yield is the maximum amount of product that can be obtained from the limiting reactant. In this case, methane is the limiting reactant, assuming an excess of oxygen.
The theoretical yield of CO2 = Number of moles of limiting reactant × Stoichiometric ratio
Theoretical yield of CO2 = 0.997 mol × 1 mol CO2/mol CH4 ≈ 0.997 mol CO2
Step 6: Convert the number of moles of CO2 to grams.
Molar mass of CO2 = (1 mol C × 12.01 g/mol) + (2 mol O × 16.00 g/mol) = 44.01 g/mol
Theoretical yield of CO2 (in grams) = Number of moles of CO2 × Molar mass of CO2
Theoretical yield of CO2 ≈ 0.997 mol × 44.01 g/mol ≈ 43.92 g
Therefore, the theoretical yield of CO2, when 16.0g of methane reacts with excess oxygen, is approximately 43.92 grams.