Is it only for H2/Pt that the enthalpy change is +ve; entropy change is +ve ?

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Q. Assertion :The thermodynamic factor which determines the spontaneity of a process is the free energy. For a process to be spontaneous the free energy must be -ve Reason: The change in free energy is related to the change in enthalpy and change in entropy. The change in entropy for a process must always be positive if it is spontaneous.

Q. Match the List-I with List – II

\begin{matrix} List - I & List - II (P) & Chloroform-methyl alcohol & (1) & Enthalpy change +ve (Q) & Methyl alcohol-ethyl alcohol & (2) & Enthalpy change -ve (R) & Ethyl alcohol-water & (3) & Entropy change +ve (S) & Water-nitric acid & (4) & Change in volume, Δ V = + v e (5) & Change in volume, Δ V = - v e \end{matrix}

Match each product in LIST-I with one or more reaction in LIST-II and choose the correct option.

In an irreversible process taking place at constant T and P and in which only PV work is being done, the change in free energy (dG) and change in entropy (dS) satisfy the criteria:

Q. Enthalpy change for the process,

H_{2} O (i c e) ⇌ H_{2} O (w a t e r)

6.01 K J {m o l}^{- 1}

. The entropy change of

1

mole of ice at its melting point will be:

Q. The enthalpy change for a given reaction at

298 K

- x

J {m o l}^{- 1}

. For the reaction to be spontaneous at

298 K

, the entropy change at that temperature:

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