For the gaseous reaction C2H4 + H2 C2H6 , Δ H = −130 kJ mol−1 carried in a closed vessel, the equilibrium concentration of the C2H6 can definitely be increased by :

Question

For the gaseous reaction C2H4 + H2 <=> C2H6 , Δ H = −130 kJ mol−1 carried in a closed vessel, the equilibrium concentration of the C2H6 can definitely be increased by : (A) increasing temperature and decreasing pressure (B) decreasing temperature and increasing pressure (C) increasing temperature and pressure both (D) decreasing temperature and pressure both

Tardigrade Admin · Accepted Answer

According to Le-Chatelier principle exothermic reactions are favourable at low

temperature. The reaction in which number of moles decrease are favourable at high pressure or low volume.

C_{2} H_{4} + H_{2} ⇌ C_{2} H_{6}; Δ H = - 130 k J m o l^{- 1}

∵

the reaction is exothermic and number of moles of reactants are decreasing

∴

the reaction rate is increased by decreasing temperature and increasing pressure.

Q. For the gaseous reaction C2​H4​+H2​​C2​H6​ , ΔH=−130kJmol−1 carried in a closed vessel, the equilibrium concentration of the C2​H6​ can definitely be increased by :

increasing temperature and decreasing pressure

decreasing temperature and increasing pressure

increasing temperature and pressure both

decreasing temperature and pressure both

Q. For the gaseous reaction
$C_{2} H_{4} + H_{2} C_{2} H_{6}$ , $Δ H = - 130 k J m o l^{- 1}$ carried in a closed vessel, the equilibrium concentration of the $C_{2} H_{6}$ can definitely be increased by :