You visited us 1 times! Enjoying our articles? Unlock Full Access!

Effect on Kc

1 mole each o...

Question

$1$ mole each of $H_{2} (g)$ and $I_{2} (g)$ are introduced in a $1 L$ eacuated vessel at $523 K$ and equilibrium
$H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$ is established. The concentration of $H I (g)$ at equilibrium:

Change on changing pressure

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Changes on changing temperature

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Change on changing volume of the vessel

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Is same even if only

2 mol

H I (g)

were introduced in the vessel in the beginning

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is C Change on changing volume of the vessel
$H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$
(a) For changing pressure, volume has to be changed, thouged, though number of moles of $H I (g)$ do not get changed but its concentration will get changed.
(b) Temperature change will change $K_{p}$ and hence concentration.
(C) Volume change will change concentration not the number of moles.
(D) Equilibrium concentration of the reactants and product depends upon the initial concentration and the equlibrium constant.

Suggest Corrections

Similar questions

Q. At 700 K, equilibrium constant for the reaction:

H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)

is 64. If

0.5 m o l L^{- 1}

of HI(g) is present at equilibrium at 700 K, what are the concentration of

H_{2} (g)

and

I_{2} (g)

assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700 K?

Q. At

700 K

, the equilibrium constant for the reaction;

H_{2 (g)} + I_{2 (g)} ⇌ 2 H I_{(g)}

54.8

0.5 m o l l i t r e^{- 1}

H I_{(g)}

is present at equilibrium at

700 K

, what are the concentrations of

H_{2 (g)}

and

I_{2 (g)}

assuming that we initially started with

H I_{(g)}

and allowed it to reach equilibrium at

700 K

Q. At

700 K

, equilibrium constant for the reaction:

H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)

64

. If

0.5 m o l

L^{- 1}

H I (g)

is present at equilibrium at

700 K

, what are the concentration of

H_{2} (g)

and

I_{2} (g)

assuming that we initially started with

H I (g)

and allowed it to reach equilibrium at

700 K

Q. 4.5 moles each of hydrogen and iodine are heated in a sealed 10-liter vessel. At equilibrium 3.0 moles of HI were found.

The equilibrium constant for

H_{2} (g)

I_{2} (g) ⇌ 2 H I (g)

is:

4.5

moles each of hydrogen and iodine heated in a sealed ten-litre vessel. At equilibrium,

3

moles of

H I

were found.

The equilibrium constant for

H_{2} (g)

I_{2} (g) ⇌ 2 H I (g)

is:

Join BYJU'S Learning Program

1 mole each of H2(g) and I2(g) are introduced in a 1 L eacuated vessel at 523 K and equilibrium H2(g)+I2(g)⇌2HI(g) is established. The concentration of HI(g) at equilibrium:

$1$ mole each of $H_{2} (g)$ and $I_{2} (g)$ are introduced in a $1 L$ eacuated vessel at $523 K$ and equilibrium
$H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)$ is established. The concentration of $H I (g)$ at equilibrium: