Answer:
is limiting reagent.
Theoretical yield = 262.67 g
% yield = (Experimental yield / Theoretical yield) × 100 = (252.4 / 262.67) × 100 = 96.1 %
Explanation:
The formula for the calculation of moles is shown below:
<u>
Given: For
</u>
Given mass = 135.8 g
Molar mass of = 58.44 g/mol
<u>Moles of = 135.8 g / 58.44 g/mol = 2.3238 moles
</u>
<u>Given: For
</u>
Given mass = 195.7 g
Molar mass of = 207.2 g/mol
<u>Moles of = 195.7 g / 207.2 g/mol = 0.9445 moles
</u>
According to the given reaction:
1 mole of react with 2 moles of
Also,
0.9445 mole of react with 2*0.9445 moles of
Moles of = 1.889 moles
Available moles of = 2.3238 moles (Extra)
Limiting reagent is the one which is present in small amount. <u>Thus, is limiting reagent.</u>
The formation of the product is governed by the limiting reagent. So,
1 mole of gives 1 mole of
0.9445 mole of gives 0.9445 mole of
Mole of = 0.9445 moles
Molar mass of = 278.1 g/mol
Mass of = Moles × Molar mass = 0.9445 × 278.1 g = 262.67 g
<u>
Theoretical yield = 262.67 g
</u>
Given experimental yield = 252.4 g
<u>% yield = (Experimental yield / Theoretical yield) × 100 = (252.4 / 262.67) × 100 = 96.1 %
</u>