At `500K` , for an isobaric pracess.
`DeltaS_(system)=-10(KJ)/(molK)` and `DeltaS_(surr)=12(KJ)/(mol K)`
Therefore, `DeltaG` for the entire process is

A spontaneous process has DeltaS_("sys")=xJ*K^(-1) and DeltaS_("surr") =-yJ*K^(-1) . Compare the values of x and y.

A spontaneous process has DeltaS_("sys")= x J. K^(-1) and Delta S_("surr")= - y J. K^(-1) . Compare the values of x and y.

In the reaction DeltaS_(sys)=xJ*K^(-1) and DeltaS_("surr")=-yJ*K^(-1) . The reaction will be spontaneous if ______.

For a process, DeltaS_(sys)=-15J*K^(-1) . For what value of DeltaS_("surr") will the process be non-spontaneous?

In a chemical reaction, Delta H = 150 kJ and Delta S = 100 JK^(-1) at 300 K. Therefore, Delta G will be

In a chemical reaction, Delta H = 150 kJ and Delta S = 100 JK^(-1) at 300 K. Therefore, Delta G will be

For a reversible process DeltaS_(sys)=-20J*K^(-1) . What will be the value of DeltaS_("surr") in this process?

For a reaction DeltaG^@ = -51.4 KJ/mol and Delta H^@ = 49.4 KJ/mol at 300K, then value of DeltaS^@ in J/K is

At given pressure and a temperature of 300K, DeltaS_(sys) and DeltaS_("surr") for a reaction are 8.0J*K^(-1) and 4.0J*K^(-1) respectively. DeltaG for this reaction is-