For a certain reaction,DGq = -45 kJ/mol and DHq= -90 kJ/mol at 0°C. What is the minimum temperature at which the reaction will become spontaneous, ifDHq and DSq are independent of temperature?

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T = 273 °K Using the formula, DGq = DHq –TDS -45 = -90 –273 DS DS = 0.164 Now since DHq and DSq are independent,T2= DH/DS = 45/0.164 = 273°K Required Temp = 273 + 273 = 546°K

For a certain reaction,DGq = -45 kJ/mol and DHq= -90 kJ/mol at 0°C. What is the minimum temperature at which the reaction will become spontaneous, ifDHq and DSq are independent of temperature?

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