A change in the free energy of a system at constant temperature and pressure will be- - sys G - - sys H - T- sys SAt constant temperature and pressure- - sys G 0 non-spontaneousIf both - H and - S are negative- the reaction will be spontaneous-

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Standard XII

Chemistry

Gibbs Free Energy & Spontaneity

A change in t...

Question

A change in the free energy of a system at constant temperature and pressure will be:
$Δ_{s y s} G = Δ_{s y s} H - T Δ_{s y s} S$
At constant temperature and pressure,
$Δ_{s y s} G < 0 (s p o n t a n e o u s)$
$Δ_{s y s} G = 0 (e q u i l i b r i u m)$
$Δ_{s y s} G > 0 (n o n - s p o n t a n e o u s)$
If both $Δ H$ and $Δ S$ are negative, the reaction will be spontaneous:

at high temperature

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at all temperatures

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at low temperature

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at high pressure

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Solution

The correct option is C at low temperature

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Q. A change in the free energy of a system at constant temperature and pressure will be:

Δ_{s y s} G = Δ_{s y s} H - T Δ_{s y s} S

At constant temperature and pressure

Δ_{s y s} G < 0 (s p o n t a n e o u s)

Δ_{s y s} G = 0 (e q u i l i b r i u m)

Δ_{s y s} G > 0 (n o n - s p o n t a n e o u s)

The free energy for a reaction having

Δ H = 31400 c a l

Δ S = 32 c a l K^{- 1} m o l^{- 1}

1000^{\circ} C

is?

A change in the free energy of a system at constant temperature and pressure will be:

Δ_{s y s} G = Δ_{s y s} H - T Δ_{s y s} S

At constant temperature and pressure,

Δ_{s y s} G < 0 (s p o n t a n e o u s)

Δ_{s y s} G = 0 (e q u i l i b r i u m)

Δ_{s y s} G > 0 (n o n - s p o n t a n e o u s)

A reaction has positive values of

Δ H

and

Δ S

From this you can deduce that the reaction:

A change in the free energy of a system at constant temperature and pressure will be:

Δ_{s y s} G = Δ_{s y s} H - T Δ_{s y s} S

At constant temperature and pressure,

Δ_{s y s} G < 0 (s p o n t a n e o u s)

Δ_{s y s} G = 0 (e q u i l i b r i u m)

Δ_{s y s} G > 0 (n o n - s p o n t a n e o u s)

For a system in equilibrium,

Δ G = 0

, under conditions of constant_____

A + B ⇌ 2 C + D

2 (E_{a})_{f} = (E_{a})_{b}; (E_{a})_{f}

= Activation energy for forward reaction,

(E_{a})_{b}

= Activation energy backward reaction. Formation of C will be favoured at

The $Δ H$ and $Δ S$ for a reaction at one atmospheric pressure are +30.558 kJ and 0.066 k J $k^{- 1}$ respectively. The temperature at which the free energy change will be zero and below this temperature the nature of reaction would be:

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A change in the free energy of a system at constant temperature and pressure will be:ΔsysG=ΔsysH−TΔsysSAt constant temperature and pressure,ΔsysG<0(spontaneous)ΔsysG=0(equilibrium)ΔsysG>0(non−spontaneous)If both ΔH and ΔS are negative, the reaction will be spontaneous:

The correct option is C at low temperature