A mixture of 28 g of N2 and 8 g of H2 reacts in a closed vessel by N2 + 3H2 -> 2NH3 until 60% of the limiting reagent has been consumed (N = 14, H = 1). Which of the following statements is/are correct?

The average molar mass of the final mixture is 9.47 g mol^-1.

The total amount of gas after reaction is 3.8 mol.

The average molar mass of the final mixture is 9.47 g mol^-1.

The total amount of gas after reaction is 3.8 mol.

The mass of NH3 formed is 34.0 g.

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3mc052

A mixture of $28 g$ of $N X_{2}$ and $8 g$ of $H X_{2}$ reacts in a closed vessel by $N X_{2} + 3 H X_{2} 2 NH X_{3}$ until $60%$ of the limiting reagent has been consumed (N = 14, H = 1). Which of the following statements is/are correct?

n (N X_{2}) = 1.0

n (H X_{2}) = 4.0

;

N X_{2}

needs

3.0

mol

H X_{2}

, so

N X_{2}

is limiting. Reacted

N X_{2}

= 0.60

: left

N X_{2}

0.40

H X_{2}

4.0 - 1.8 = 2.2

NH X_{3}

1.20

. Total

= 3.8

mol. Mass is conserved at

36

g, so average

M = 36/3.8 = 9.47

NH X_{3}

mass

= 1.20 \times 17 = 20.4

g, not

34