4.5 moles each of hydrogen and iodine heated in a sealed 10 litre vessel. At equilibrium, 3 moles of HI was found. The equilibrium constant for. H2(g)+I2(g) leftharpoons 2HI(g) is

Question

4.5 moles each of hydrogen and iodine heated in a sealed 10 litre vessel. At equilibrium, 3 moles of HI was found. The equilibrium constant for. H2(g)+I2(g) leftharpoons 2HI(g) is (A) 1 (B) 10 (C) 5 (D) 0.33

Tardigrade Admin · Accepted Answer

Total mole at equilibrium =(1-α)+2α =1 +α H2 +I2 leftharpoons 2HI Initial cone. undersetx4.5 underset x4.5 underset 2x0 From question 2x = 3 x= (3/2) =1.5 So cone, at equilibrium 4.5 - 1.5 of H2 = 4.5 - 1.5 of I2 and 3 of HI K= ([HI]2/[I2][H2])=(3×3/3×3)=1

Q. $4.5$ moles each of hydrogen and iodine heated in a sealed $10$ litre vessel. At equilibrium, $3$ moles of $H I$ was found. The equilibrium constant for. $H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$ is

$1$

$10$

$5$

$0.33$

Q. 4.5 moles each of hydrogen and iodine heated in a sealed 10 litre vessel. At equilibrium, 3 moles of HI was found. The equilibrium constant for. H2​(g)+I2​(g)⇌2HI(g) is

1

10

5

0.33

Total mole at equilibrium =(1−α)+2α=1+α H2​+I2​⇌2HI Initial cone. x4.5​x4.5​2x0​ From question 2x=3 x=23​=1.5 So cone, at equilibrium 4.5−1.5 of H2​ =4.5−1.5 of I2​ and 3 of HI K=[I2​][H2​][HI]2​=3×33×3​=1

Q. $4.5$ moles each of hydrogen and iodine heated in a sealed $10$ litre vessel. At equilibrium, $3$ moles of $H I$ was found. The equilibrium constant for. $H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$ is

$1$

$10$

$5$

$0.33$