$56 g$ of $N X_{2}$ and $18 g$ of $H X_{2}$ react as $N X_{2} + 3 H X_{2} 2 NH X_{3}$ with an actual yield of $80%$ based on the limiting reagent ( $N = 14$ , $H = 1$ ). Choose the correct statement(s).

Answer: A, B, D

N X_{2}

= 2 mol needs 6 mol

H X_{2}

(available 9), so

N X_{2}

is limiting. At 80% yield extent = 1.6 mol.

NH X_{3}

= 3.2 mol = 54.4 g (A true).

H X_{2}

left = 4.2 mol = 8.4 g (B true).

N X_{2}

left = 0.4 mol = 11.2 g, so C is false. Gas moles = 11 - 2 x 1.6 = 7.8 (D true).