Following gaseous reaction is undergoing in a vessel C2H4 + H2 leftharpoons C2H6; Δ H = -32.7 kcal Which will increase the equilibrium concentration of C2H6?

Question

Following gaseous reaction is undergoing in a vessel C2H4 + H2 leftharpoons C2H6; Δ H = -32.7 kcal Which will increase the equilibrium concentration of C2H6? (A) Increase of temperature (B) By reducing temperature (C) By removing some hydrogen (D) By adding some C2H6

Tardigrade Admin · Accepted Answer

Exothermic reaction is favoured by low temperature

Q. Following gaseous reaction is undergoing in a vessel
$C_{2} H_{4} + H_{2} ⇌ C_{2} H_{6}; Δ H = - 32.7 k c a l$ Which will increase the equilibrium concentration of $C_{2} H_{6} ?$

Increase of temperature

By reducing temperature

By removing some hydrogen

By adding some $C_{2} H_{6}$

Exothermic reaction is favoured by low temperature

Q. Following gaseous reaction is undergoing in a vessel C2​H4​+H2​⇌C2​H6​;ΔH=−32.7kcal Which will increase the equilibrium concentration of C2​H6​?

Increase of temperature

By reducing temperature

By removing some hydrogen

By adding some C2​H6​

Exothermic reaction is favoured by low temperature

Q. Following gaseous reaction is undergoing in a vessel
$C_{2} H_{4} + H_{2} ⇌ C_{2} H_{6}; Δ H = - 32.7 k c a l$ Which will increase the equilibrium concentration of $C_{2} H_{6} ?$

By adding some $C_{2} H_{6}$