(C) The spontaneity of a process is determined by the Gibbs free energy change,given by the equation $\Delta G = \Delta H - T\Delta S$. For a process

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Positive $\Delta H$ and negative $\Delta S$

(C) The spontaneity of a process is determined by the Gibbs free energy change,given by the equation $\Delta G = \Delta H - T\Delta S$. For a process to be non-spontaneous,$\Delta G$ must be positive $(> 0)$. When $\Delta H > 0$ (endothermic) and $\Delta S Therefore,the condition $\Delta H > 0$ and $\Delta S < 0$ always leads to a non-spontaneous change.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

Which of the following conditions will always lead to a non-spontaneous change?

A
Positive $\Delta H$ and positive $\Delta S$
B
Negative $\Delta H$ and negative $\Delta S$
C
Positive $\Delta H$ and negative $\Delta S$
D
Negative $\Delta H$ and positive $\Delta S$

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Thermodynamics

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Free energy and Work

$2 \, mol$ of zinc is dissolved in $HCl$ at $25 \, ^oC$. What is the work done in an open vessel?

Medium

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Assertion: Many endothermic reactions that are not spontaneous at room temperature become spontaneous at high temperature.
Reason: Entropy of the system increases with increase in temperature.

MediumAIIMS 2012

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For the reaction $A \longrightarrow B$,$\Delta H^{\circ} = 7.5 \, kJ \, mol^{-1}$ and $\Delta S^{\circ} = 25 \, J \, K^{-1} \, mol^{-1}$. The value of $\Delta G^{\circ}$ and the temperature at which the reaction reaches equilibrium are,respectively:

MediumKVPY 2010

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For the melting of $3 \ mol$ of ice at $0^o \text{C}$,$\Delta G = \dots \dots$

Easy

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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) $(R=8.3 \ J \ K^{-1} \ mol^{-1})$

MediumAP EAMCET 2025

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Which of the following conditions will always lead to a non-spontaneous change?

Similar Questions

$2 \, mol$ of zinc is dissolved in $HCl$ at $25 \, ^oC$. What is the work done in an open vessel?

Assertion: Many endothermic reactions that are not spontaneous at room temperature become spontaneous at high temperature.Reason: Entropy of the system increases with increase in temperature.

For the reaction $A \longrightarrow B$,$\Delta H^{\circ} = 7.5 \, kJ \, mol^{-1}$ and $\Delta S^{\circ} = 25 \, J \, K^{-1} \, mol^{-1}$. The value of $\Delta G^{\circ}$ and the temperature at which the reaction reaches equilibrium are,respectively:

For the melting of $3 \ mol$ of ice at $0^o \text{C}$,$\Delta G = \dots \dots$

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) $(R=8.3 \ J \ K^{-1} \ mol^{-1})$

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Assertion: Many endothermic reactions that are not spontaneous at room temperature become spontaneous at high temperature.
Reason: Entropy of the system increases with increase in temperature.