Question

Consider the following reaction

2A2 + 3B2 → 2C2 + D2

If 6 mol of A2 reacts with 7.5 mol of B2, then

(a)4 mol of C2 is formed
(b)3 mol of D2 is formed
(c)0.5 mol of B2 is left in excess
(d)1 mol of A2 is left in excess

Answer 1

Answer:

The Correct Answer is (d)1 mol of A2 is left in excess.

Explanation:

We must compare the stoichiometric coefficients of the reactants and products in order to ascertain the amounts involved in the reaction.

The balanced equation reads as follows:

$2A2 + 3B2 \rightarrow 2C2 + D2$

For A2, B2, C2, and D2, the stoichiometric ratio is 2:3:2:1, correspondingly.

Given:

6 mol of A2 reacts with 7.5 mol of B2

We may determine the moles of C2 and D2 created by using the stoichiometric ratio.

For C2, the balanced equation shows that A2:C2 is a 2:2 ratio. As a result, when 6 mol of A2 interacts, 6 mol of C2 is created.

For D2, the balanced equation shows that B2:D2 is a 3:1 ratio. As a result, when 7.5 mol of B2 interacts, ($\frac{7.5}{3}$) × 1 = 2.5 mol of D2 is produced.

Therefore, the correct options are:

(a) 4 mol of C2 is formed (incorrect, it should be 6 mol)

(b) 3 mol of D2 is formed (incorrect, it should be 2.5 mol)

(c) 0.5 mol of B2 is left in excess (incorrect, it should be 2.5 mol of B2)

(d) 1 mol of A2 is left in excess (correct)

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