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For a process Delta S("total") = 0 and D...

For a process `Delta S_("total") = 0` and `Delta G = 0` was obtained. What does it mean?

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The process is in equilibrium
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For a process DeltaS_(total) = 0 and Delta G = 0 was obtained. What does it mean?

How many of the following statement(s) is/are true for free expansion of ideal gas in an insulated container ? 1. It is a Reversible process. 2. Delta H=0 , for this process. 3. Delta E=0 , for this process. 4. Delta(PV)=0 5. Delta T = 0 , for this process. 6. Delta S_("surrounding")=0 , for this process. 7. Delta S_("system")=0 , for this process. 8. Delta S_("total") = 0 , for this process.

Statement-1: For a process to be spontaneous, Delta G as well as Delta S has to be less than zero. Statement-2 : For spontaneous change, Delta S_("total") gt 0

In a reversible process, Delta S_(sys) + Delta S_(surr) is

If a process has Delta H = 548.3 kJ and Delta S = 32 J/mole at 298 K then will the process be spontaneous at this temperature ?

What does Delta G = 0 represent ?

If Delta H gt 0 and Delta S gt 0 , the reaction proceeds spontaneously when :-

A : For an isolated system Delta G = - TDeltaS_("total") R: For an isolated system q = 0.

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