Question

In the reaction $4A+2B+3C⟶A_4{B}_2{C}_3$, the number of moles of products formed will be ______, If starting from 2 moles of A, 1.2 moles of B and $1.44$ moles of C.

• A. $0.48$
• B. $0.3$
• C. $0.6$
• D. $41$

Answer 1

The correct option is A $0.48$

$4A+2B+3C⟶A_4{B}_2{C}_3$

From the reaction-

No. of moles of element B required to react with 4 moles of element A $=2$

No. of moles of element B required to react with 2 moles of element A $=\frac{2}{4}\times 2=1\text{mole}$

Given amount of element B = 1.2 moles

No. of moles of element C required to react with 4 moles of element A $=3$

No. of moles of element C required to react with 2 moles of element A $=\frac{3}{4}\times 2=1.5\text{moles}$

Given amount of element C = 1.44 moles

$\therefore$ In the given reaction, C is limiting reagent.

Therefore,

No. of moles of product formed when 3 moles of element C react $=1\text{mole}$

No. of moles of product formed when 1.44 moles of element C react $=\frac{1}{3}\times 1.44=0.48\text{moles}$

Hence, 0.48 moles product formed.