For a hypothetical reaction A(g)+3B(g)⇌2C(g)ΔH=–100kJ and ΔS=–200JK−1 Then the temperature at which the reaction will be in equilibrium.
500K
480 K
520 K
510 K
At equilibrium ΔG=0;ΔH−TΔS=0;∴T=ΔHΔS
For the reaction at 298 K,
2A + B → C
ΔH = 400 kJ mol–1 and ΔS = 0.2 kJ K–1 mol–1
At what temperature will the reaction become spontaneous considering ΔH and ΔS to be constant over the temperature range?