In which of the following conditions can a chemical reaction not occur?
- A$\Delta H > 0$ and $\Delta S > 0$ with $T\Delta S > \Delta H$
- B$\Delta H < 0$ and $\Delta S < 0$ with $\Delta H > T\Delta S$
- C$\Delta H > 0$ and $\Delta S < 0$
- D$\Delta H < 0$ and $\Delta S > 0$
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At $273 \ K$ the maximum work done when pressure on $10 \ g$ of hydrogen is reduced from $10 \ atm$ to $1 \ atm$ under isothermal,reversible conditions is (Assume the gas behaves ideally) $(R=8.3 \ J \ K^{-1} \ mol^{-1})$
For the reaction at $298 \ K$,$2 \ A^{+}B \rightarrow C$. $\Delta H = 400 \ kJ \ mol^{-1}$ and $\Delta S = 0.2 \ kJ \ mol^{-1} \ K^{-1}$. The reaction will become spontaneous above $...... \ K$.
If $\Delta_r H^{\ominus}$ and $\Delta_r S^{\ominus}$ are standard enthalpy change and standard entropy change respectively for a reaction,the incorrect option is
Identify the correct statement for the change in Gibbs energy $(\Delta G_{\text{system}})$ for a system at constant temperature and pressure.
Easy
View SolutionThe occurrence of a reaction is impossible if
MediumAIIMS 1982
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