5.4 g of Al reacts with 14.6 g of HCl according to 2Al + 6HCl -> 2AlCl3 + 3H2 (Al = 27, H = 1, Cl = 35.5; 22.4 L mol^-1 at STP). Which of the following statements is/are correct?

The mass of aluminium left over is 1.8 g.

The volume of H2 at STP is 4.48 L.

The mass of aluminium left over is 1.8 g.

The volume of H2 at STP is 4.48 L.

The mass of AlCl3 formed is 26.7 g.

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3mc053

$5.4 g$ of Al reacts with $14.6 g$ of HCl according to $2 Al + 6 HCl 2 AlCl X_{3} + 3 H X_{2}$ (Al = 27, H = 1, Cl = 35.5; $22.4 L mo l^{- 1}$ at STP). Which of the following statements is/are correct?

n (Al) = 0.20

n (HCl) = 0.40

. Al would need

0.60

mol HCl, so HCl is limiting.

H X_{2}

= 0.40/2 = 0.20

mol

= 4.48

L. Al consumed

= 0.40/3 = 0.133

mol, left

= (0.200 - 0.133) \times 27 = 1.8

AlCl X_{3}

= 0.133 \times 133.5 = 17.8

g, whereas

26.7

g would need all Al to react.