For complete combustion of ethene, C 2 H 4 ( g ) + 3 O 2 ( g ) → 2 CO 2 ( g ) + 2 H 2 O ( l ) the amount of heat produced as measured in bomb calorimeter is 1406 kJ mol - 1 at 300 K . The minimum value of TΔS needed to reach equilibrium is ( - ) kJ . (Nearest integer) Given: R = 8 . 3 J K - 1 mol - 1

Step-by-step solution

C 2 H 4 (   g ) + 3 O 2 (   g ) → 2 CO 2 (   g ) + 2 H 2 O ( l ) ΔU = - 1406   kJ   mol - 1 T = 300 K ΔH = ΔU + Δn g RT ΔU is the change in the internal energy of the system, which is the sum of the kinetic and potential energies of all the molecules in the system. R is the gas constant ( 8 . 314   J / ( mol   K ) and T is the temperature in Kelvin. ∆ H   =   – 1406   +   ( – 2 )   ×   8 . 3