Decomposition of ammonium chloride is an endothermic reaction. The equilibrium may be represented as: NH 4 Cl ( s ) leftharpoons NH 3( g )+ HCl ( g ) A 6.250 g sample of NH 4 Cl is placed in an evaculated 4.0 L container at 27° C. After equilibrium the total pressure inside the container is 0.820 bar and some solid remains in the container. Answer the followings The value of Kp for the reaction at 300 K is

Question

Decomposition of ammonium chloride is an endothermic reaction. The equilibrium may be represented as: NH 4 Cl ( s ) leftharpoons NH 3( g )+ HCl ( g ) A 6.250 g sample of NH 4 Cl is placed in an evaculated 4.0 L container at 27° C. After equilibrium the total pressure inside the container is 0.820 bar and some solid remains in the container. Answer the followings The value of Kp for the reaction at 300 K is (A) 16.2 (B) 0.168 (C) 1.68 (D) 32.4

Tardigrade Admin · Accepted Answer

P NH 3=P HCl =(0.820/2) bar ∴ Kp=P NH 3 × P HCl =0.41 × 0.41=0.168

$16.2$

$0.168$

$1.68$

$32.4$

$P_{N H_{3}} = P_{H Cl} = \frac{0.820}{2}$ bar
$∴ K_{p} = P_{N H_{3}} \times P_{H Cl} = 0.41 \times 0.41 = 0.168$

16.2

0.168

1.68

32.4

PNH3​​=PHCl​=20.820​ bar ∴Kp​=PNH3​​×PHCl​=0.41×0.41=0.168

$16.2$

$0.168$

$1.68$

$32.4$

$P_{N H_{3}} = P_{H Cl} = \frac{0.820}{2}$ bar
$∴ K_{p} = P_{N H_{3}} \times P_{H Cl} = 0.41 \times 0.41 = 0.168$