For the reaction: , ΔH=467.9 kJ/mol and ΔS=0.56 kJ/mol K. Calculate the temperature at which the ΔG° becomes zero. What will be the direction of reaction above this temperature?

For the reaction: , ΔH=467.9 kJ/mol and ΔS=0.56 kJ/mol K. Calculate

1.	For the reaction: , ΔH=467.9 kJ/mol and ΔS=0.56 kJ/mol K. Calculate the temperature at which the ΔG° becomes zero. What will be the direction of reaction above this temperature?
Answer» e reaction, Given,We have to Calculate the TEMPERATURE at which the becomes ZERO, so put \DELTA G\QUAD =\quad 0W.K.T. 0 = 467.9 - T(0.56)T = 835.5 (at which the becomes zero)Above this temperature T = 835.5, becomes positive and so the direction of reaction is reversed."