In the reaction, 2 Al ( s ) + 6 HCl ( aq ) 2 Al 3 + ( aq ) + 6 Cl

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Q.
In the reaction,

$2 Al (s) + 6 HCl (aq) \to 2 {Al}^{3 +} (aq) + 6 {Cl}^{-} (aq) + 3 H_{2} (g)$ [2026]

1 $33.6 L H_{2} (g)$ is produced regardless of temperature and pressure for every mole of Al that reacts.

2 $12 L HCl (aq)$ is consumed for every $6 L H_{2} (g)$ produced.

3 $67.2 L H_{2} (g)$ at STP is produced for every mole of Al that reacts.

4 $11.2 L H_{2} (g)$ at STP is produced for every mole of HCl consumed.

Ans.
(4)

$2 Al (s) + 6 HCl (aq) \to 2 {Al}^{3 +} (aq) + 6 {Cl}^{-} (aq) + 3 H_{2} (g)$

$Mole of H_{2} produced$

$= 2 \times mole of HCl used$

$= \frac{2}{3} \times mole of Al used$

Solution

Q.
In the reaction,

$2 Al (s) + 6 HCl (aq) \to 2 {Al}^{3 +} (aq) + 6 {Cl}^{-} (aq) + 3 H_{2} (g)$ [2026]

1 $33.6 L H_{2} (g)$ is produced regardless of temperature and pressure for every mole of Al that reacts.

2 $12 L HCl (aq)$ is consumed for every $6 L H_{2} (g)$ produced.

3 $67.2 L H_{2} (g)$ at STP is produced for every mole of Al that reacts.

4 $11.2 L H_{2} (g)$ at STP is produced for every mole of HCl consumed.

Ans.
(4)

$2 Al (s) + 6 HCl (aq) \to 2 {Al}^{3 +} (aq) + 6 {Cl}^{-} (aq) + 3 H_{2} (g)$

$Mole of H_{2} produced$

$= 2 \times mole of HCl used$

$= \frac{2}{3} \times mole of Al used$

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Solution

Q. In the reaction, 2Al(s)+6HCl(aq)→2Al3+(aq)+6Cl-(aq)+3H2(g) [2026]

1 33.6 L H2(g) is produced regardless of temperature and pressure for every mole of Al that reacts.

2 12 L HCl(aq) is consumed for every 6L H2(g) produced.

3 67.2 L H2(g) at STP is produced for every mole of Al that reacts.

4 11.2 L H2(g) at STP is produced for every mole of HCl consumed.

Ans. (4) 2Al (s)+6HCl (aq)→2Al3+(aq)+6Cl-(aq)+3H2(g) Mole of H2 produced =2×mole of HCl used =23×mole of Al used

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Q.
In the reaction,

$2 Al (s) + 6 HCl (aq) \to 2 {Al}^{3 +} (aq) + 6 {Cl}^{-} (aq) + 3 H_{2} (g)$ [2026]

1 $33.6 L H_{2} (g)$ is produced regardless of temperature and pressure for every mole of Al that reacts.

2 $12 L HCl (aq)$ is consumed for every $6 L H_{2} (g)$ produced.

3 $67.2 L H_{2} (g)$ at STP is produced for every mole of Al that reacts.

4 $11.2 L H_{2} (g)$ at STP is produced for every mole of HCl consumed.

Ans.
(4)

$2 Al (s) + 6 HCl (aq) \to 2 {Al}^{3 +} (aq) + 6 {Cl}^{-} (aq) + 3 H_{2} (g)$

$Mole of H_{2} produced$

$= 2 \times mole of HCl used$

$= \frac{2}{3} \times mole of Al used$