First slide

Gaseous state

Question

In the following reaction, we start with 2 moles of N₂ and 5 moles of H₂ exerting a total pressure of 7 atm at a given temperature in a closed vessel. When 50% of N₂ is converted into ${NH}_{3} N_{2} + 3 H_{2} ⟶ 2 {NH}_{3}$ , partial pressure of NH₃ is

Difficult

A

2.8 atm
B

2 atm
C

3.2 atm
D

4 atm

Solution

$N_{2} + 3 H_{2} ⟶ 2 {NH}_{3} Taken 2 5 0 Reacted (50 % of N_{2}) 1 3 Left 1 2$
Total moles of N₂, H₂ and NH₃ = 5 mol initial mol = 7
pressure at start = 7 atm
Hence, pressure at equilibrium = 5 atm
$∴ Partial pressure of {NH}_{3} = \frac{2}{5} \times 5 = 2 atm$

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