The equilibrium constant for the reaction A-B- C-D is 2-85 at room temperature and 1-4- 10 -2 at 698K- This shows that forward reaction is-

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

Byju's Answer

Standard XII

Chemistry

Le Chatelier's Principle for Del N Equals to 0

The equilibri...

Question

The equilibrium constant for the reaction $A + B ⇌ C + D$ is $2.85$ at room temperature and $1.4 \times 10^{- 2}$ at $698 K$ . This shows that forward reaction is:

Exothermic

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

Endothermic

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

Unpredictable

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

There is no relationship between

Δ H

and

K

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

Open in App

Solution

The correct option is D Exothermic
With increase in temperature, the value of the equilibrium constant decreases.
As temperature increases, the amount of products decreases and the amount of reactants increases.
With increase in temperature, the equilibrium shifts to left.
This is characteristic of exothermic reaction.

Suggest Corrections

Similar questions

Q. The equilibrium constant

K

for the reaction :

2 H I (g) ⇌ H_{2} (g) + I_{2} (g)

at room temperature is

2.85

and that at

698 K

1.4 \times {! 0}^{- 2}

. This implies that the forward reaction is:

Q. The equilibrium constant K for the reaction

2 H I (g) ⇌ H_{2} (g) + I_{2} (g)

at room temperature is

2.85

and that at

698 K

1.4 \times 10^{- 2}

. This implies :

Q. The equilibrium constant K for the reaction:

2 H I (g) ⇌ H_{2} (g) + I_{1} (g)

at room temp is 2.85 and that at 698 K is

1.4 \times 10^{- 2}

. This implies that the forward reaction is:

Q. The equilibrium constant

K

, for the given reaction

2 H I (g) ⇌ H_{2} (g) + I_{2} (g)

at room temperature is

2.85 K

and that at

698 K

1.4 \times 10^{- 2}

. Hence the reason that

H I

exists as a stable compound at room temperature is____________.

Q. For a given exothermic reaction

K_{p}

and

{K^{^{'}}}_{p}

are the equilibrium constants at temperature

T_{1}

and

T_{2}

respectively. Assuming that heat of reaction is constant in temperature range between 183.

T_{1}

and

T_{2}

it is readily observed that:

Join BYJU'S Learning Program

The equilibrium constant for the reaction A+B⇌C+D is 2.85 at room temperature and 1.4×10−2 at 698K. This shows that forward reaction is:

The equilibrium constant for the reaction $A + B ⇌ C + D$ is $2.85$ at room temperature and $1.4 \times 10^{- 2}$ at $698 K$ . This shows that forward reaction is: