Question

In the reaction, $2Al(s) + 6HCl(aq) \rightarrow 2Al^{3+} (aq) + 6Cl^- (aq) + 3H_2(g)$
(a) 11.2 L H₂(g) at STP is produced for every mole HCl(aq) consumed
(b) 6 L HCl(aq) is consumed for every 3 L H₂(g) produced
(c) 33.6 L H₂(g) is produced regardless of temperature and pressure for every mole Al that reacts
(d) 67.2 H₂(g) at STP is produced for every mole Al that reacts.

Answer 1

answer is only (a)

we cannot measure the amount of gas for an aquous HCl so option (b) is wrong

(c) is wrong because the amount of gas produced differ in tamparature and pressure condition

(d) is wrong because only 33.6 L of H₂₂gas is produced for every mole of Al

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