Question

X+Y=X3Y4 .Above reaction is carried out by taking 6 moles each of X and Y,then which is incorrect
1) X is the limiting reagent
2)1.5 moles of X3Y4 is formed
3)1.5moles of excess reagent is left behind
4) 75% of excess reagent reacted.

EXPLAIN IT.
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Answer 1

Limiting reagent

Explanation:

• For the given reaction, $X + Y = X_{3}Y_{4}$

• The balanced chemical reaction is $3X + 4Y = X_{3}Y_{4}$

Now, for finding limiting reagent,

• 3 mol of X forms 1 mol $X_{3}Y_{4}$
• 6 mol of X forms 2 mol $X_{3}Y_{4}$

On the other hand

• 4 mol of Y forms 1 mol $X_{3}Y_{4}$
• 6 mol of X forms 1.5 mol $X_{3}Y_{4}$

• From this, we infer that, Y is the limiting reagent and 1.5 mol of  $X_{3}Y_{4}$ is formed, and during the reaction, 4.5mol of X is used; thus, 1.5 mol of excess reagent(X) are left, and thus 75% of X is reacted only.

• hence, the incorrect statement is 1) X is the limiting reagent