The reaction C 2 H 6 g - C 2 H 4 g - H 2 g is at an equilibrium in a closed vessel at 1000 K- The enthalpy change H for the reaction is 137-0kJ mol -1- Which one of the following actions would shift the equilibrium to the right-A- Decreasing the volume of the closed reaction vesselB- Decreasing the temperature at which the reaction is performedC- Adding an inert gas to the closed reaction vesselD- Increasing the volume of the closed reaction vessel

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

Le Chatelier's Principle

The reaction ...

Question

The reaction $C_{2} H_{6} (g) ⇌ C_{2} H_{4} (g) + H_{2} (g)$ is at an equilibrium in a closed vessel at 1000 K. The enthalpy change $(△ H)$ for the reaction is 137.0 $k J m o l^{- l}$ . Which one of the following actions would shift the equilibrium to the right?

Decreasing the volume of the closed reaction vessel

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

Decreasing the temperature at which the reaction is performed

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

Adding an inert gas to the closed reaction vessel

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

Increasing the volume of the closed reaction vessel

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

Open in App

Solution

Suggest Corrections

Similar questions

C_{2} H_{6} (g) ⇌ C_{2} H_{4} (g) + H_{2} (g)

1000 K

(Δ H)

137.0

k J . m o l^{- 1}

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

C_{2} H_{4} (g) + H_{2} (g) ⇌ C_{2} H_{6} (g); △ H^{o} = - 136.8 k J m o l^{- 1}

C_{2} H_{4}

A B_{2} (g) + A (s) ⇌ B_{2} (g) + A_{2} (g)

K \to Equilibrium Constant

T \to Temperature in Kelvin

A B_{2}

The volume of a closed reaction vessel in which the equilibrium -

$2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$ sets is halved, Now -

Join BYJU'S Learning Program