Question

If 1.00 g of reactant a is mixed with 2.00 g of reactant b, what is the theoretical yield of product d, in grams (g)? the molar mass of a = 94.0 g/mol, b = 118 g/mol , and d = 125 g/mol.

Answer 1

The chemical reaction is as follows:

`a+b\rightarrow d`

Mass of reactant a is 1 g and molar mass is 94 g/mol. Converting mass into number of moles as follows:

`n=(m)/(M)=(1g)/(94 g/mol)=0.0106 mol`

Now, 1 mole of reactant a gives 1 mole of product d thus, 0.0106 mol of reactant a gives 0.0106 mol of product d.

Molar mass of product d is 125 g/mol, converting number of moles into mass as follows:

m=n×M=0.0106 mol×125 g/mol=1.33 g

Similarly, molar mass of reactant b is 118 g/mol and mass is 2 g, converting mass into number of moles,

`n=(m)/(M)=(2g)/(118 g/mol)=0.017 mol`

1 mol of reactant b gives 1 mol of product d thus, 0.017 mol will give 0.017 mol of product d.

Converting number of moles into mass as follows:

m=n×M=0.017 mol×125 g/mol=2.12 g

Here, reactant that produces lesser product is limiting reactant and the amount of product it forms is theoretical yield.

Therefore, theoretical yield is 1.33 g.