$H_2$ evolved at STP on complete reaction of 27 g of Aluminium with excess of aqueous NaOH would be

Q. $H_2$ evolved at STP on complete reaction of 27 g of Aluminium with excess of aqueous NaOH would be

Q. A mixture of aluminium and zinc weighing $1.67$ g was completely dissolved in acid and evolved $1.69$ litres of $H_2$ at NTP. The weight of aluminium in the original mixture is:

Q. $0.9$ g of Aluminium reacts with dil. $HCl$ to give $H_2$. The volume of $H_2$ evolved at STP is:

Q. $0.18\text{g}$ of $Al$ reacts with $dil.HCl$ to give $H_2$. The volume of $H_2$ evolved at STP is:
(Atomic weight of $Al=27$)

Q. A mixture of aluminium and zinc weighing 1.67 grams was completely dissolved in acid and 1.69 litres of hydrogen gas was evolved. The hydrogen gas was measured at STP conditions. What was the mass percent of aluminium in original mixture?