Question

6Al+6Hcl->2[Al(H20)6+6Cl+3H

Answer 1

Answer:

6Al+6Hcl->2[Al(H20)6+6Cl+3H

Explanation:

In option A, the conditions of temperature and pressure are not mentioned.

Hence, the number of moles of hydrogen cannot be determined.

Hence, the option, 6 L HCl  

(

​  

aq) is consumed for every 3 L H  

2

​  

(g) produced, cannot be correct.

Thus, option A is incorrect.

For options, B and C, 2 moles of Al reacts with 3 moles of hydrogen.

Hence, 1 mole of Al will react with 1.5 moles of hydrogen.

At STP, 1.5 moles of hydrogen will occupy a volume of 1.5×22.4=33.6L

Thus, 33.6 L of hydrogen gas is produced at standard temperature and pressure only for every mole Al that reacts.

Hence, option B is correct and option C is incorrect.

In the case of option D, from the balanced chemical equation, it can be seen that 6 moles of HCl reacts with 3 moles of hydrogen.

Hence, 1 mole of HCl will react with  

6

3

​  

=0.5 moles of hydrogen.

At STP, 1 mole of hydrogen corresponds to 22.4 L.

Hence, 0.5 moles of hydrogen will correspond to  

2

22.4

​  

=11.2L.

Thus, 11.2 L of hydrogen gas at STP is produced for every mole of HCl consumed.

Thus, option D is correct.

Answer 2

Answer:

2 Al (s) + 6 HCl (aq) → 2 AlCl3 (aq) + 3 H2 (g)

This is an oxidation-reduction (redox) reaction:

6 HI + 6 e- → 6 H0

(reduction)

2 Al0 - 6 e- → 2 AlIII

(oxidation)

HCl is an oxidizing agent, Al is a reducing agent