If 30mL of $H_{2}$ and 20mL of $O_{2}$ react to form water 5mL of $H_{2}$ is left at the end of reaction, is it correct assertion.

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Solution

Step 1:
Volume of $H_{2}$ = 30 ml
Volume of $O_{2}$ = 20 ml
Reaction between H₂ and O₂ to form water is as follows:
$H_{2} + \frac{1}{2} O_{2} ⟶ H_{2} O$
30mL 15 mL reacted
Step 2:
According to the equation:
1ml of H₂ reacts with 1/2 mL of O₂ form 1 mL of H₂O.
So, 30 mL of H₂ will react with 15 mL of O₂ to form 30 mL of water.
Step 3:
Therefore, O₂ is present in excess.
Volume of $O_{2}$ left = $20 - 15 = 5 m L$
Thus, 5 mL of O₂ will be left behind and $H_{2}$ is the limiting reagent.
So 5 mL of $H_{2}$ is left is a wrong assertion.

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Similar questions

Q. Assertion :If

30

mL of

H_{2}

and

20

mL of

O_{2}

react to form water, then

5

mL of

H_{2}

is left at the end of the reaction. Reason:

H_{2}

is the limiting reagent.

In each of the following questions, an Assertion (A) is followed by a corresponding Reason (R). Use the following keys to choose the appropriate answer.

Assertion (A): If 30 mL of $H_{2}$ and 20 mL of $O_{2}$ react to form water, 5 mL of $H_{2}$ is left at the end of the reaction.
Reason (R): $H_{2}$ is the limiting reagent.

In each of the following questions, an Assertion (A) is followed by a corresponding Reason (R). Use the following keys to choose the appropriate answer.

Assertion (A): If 30 mL of $H_{2}$ and 20 mL of $O_{2}$ react to form water, 5 mL of $H_{2}$ is left at the end of the reaction.
Reason (R): $H_{2}$ is the limiting reagent.