Question

For the reaction given below, select the correct statement.
$2Al\left(s\right)+6HCl\left(aq\right)\to 2{Al}^{3+}\left(aq\right)+6{Cl}^{-}\left(aq\right)+3H_2$

• A. $11.2$ litres of $H_2$ at STP is produced for every mole of $HCl$ (aq) used.
• B. $6$ litres $HCl\left(aq\right)$ is consumed for every $3$ litres of $H_2\left(g\right)$ produced.
• C. $33.6$ litres of $H_2\left(g\right)$ is produced regard less of temperature and pressure for every mole of $Al$ that reacts.
• D. $67.2$ litres of $H_2\left(g\right)$ at STP is produced for every mole of $Al$ that reacts.

Answer 1

Answer: (A)

$11.2$ litres of $H_2$ at STP is produced for every mole of $HCl$ (aq) used.

From the balanced chemical reaction, it can be seen that 6 moles of HCl produce 3 moles of hydrogen. Hence, 1 mole of HCl will produce 0.5 moles of hydrogen which will occupy volume of 11.2 L at STP. Thus, the option A is correct and the option B is incorrect.
1 mole of Al will produce 1.5 moles of hydrogen which will occupy a volume of 33.6 L under STP conditions only. Hence, the options C and D are incorrect.