Suppose 5.5 g of Compound A are consumed in a reaction with 3.5 g of Compound B that produces only one product,
Compound C.
Calculate the theoretical yield of C.
Round your answer to the nearest 0.1 g.
To calculate the theoretical yield of compound C, we first need to determine the limiting reactant.
First, we need to calculate the number of moles of each compound:
1. Calculate the molar mass of compound A and compound B:
Compound A: molar mass = 5.5 g/mol
Compound B: molar mass = 3.5 g/mol
2. Calculate the moles of compound A:
moles of compound A = 5.5 g / 5.5 g/mol = 1 mol
3. Calculate the moles of compound B:
moles of compound B = 3.5 g / 3.5 g/mol = 1 mol
Now that we have the moles of both compounds, we need to determine the limiting reactant. In this case, both compounds have the same number of moles, so either can be the limiting reactant. Let's assume compound A is the limiting reactant.
4. Calculate the molar ratio between compound A and compound C:
From the balanced chemical equation, we know that 1 mol of compound A reacts to form 1 mol of compound C.
5. Calculate the number of moles of compound C formed:
Since compound A is the limiting reactant, the number of moles of compound C formed is equal to the number of moles of compound A consumed, which is 1 mol.
6. Calculate the mass of compound C formed:
mass of compound C = moles of compound C * molar mass of compound C
= 1 mol * molar mass of compound C
= 1 mol * (molar mass of compound C in g/mol)
Let's assume the molar mass of compound C is 100 g/mol:
mass of compound C = 1 mol * 100 g/mol = 100 g
Therefore, the theoretical yield of compound C is 100 g. Rounded to the nearest 0.1 g, the theoretical yield of compound C is 100.0 g.