The following reaction has the thermodynamic values at 298 K: ΔH° = -136.9 kJ/mol and ΔS° = -120.6 J/mol K. Calculate ΔG° at 298 K for this reaction in kJ/mol (Enter your answer to four significant figures.):

at 298 K is -101.0 kJ/mol

Explanation:

According to thermodynamic of state,

where, , , T and represent change in free energy in standard state, change in enthalpy in standard state, temperature in kelvin scale and change in entropy in standard state.

Here, , T = 298 K and

So,

              = -101.0 kJ/mol

So, at 298 K is -101.0 kJ/mol

why do the isotopes of a particular element behave differently in nuclear reactions but the same in chemical reactions? chemical reactions involve changes to electrons in an atom; isotopes do not differ in electrons, and so they react the same way during chemical changes.