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Thermodynamics

Question

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For a given reaction, ΔH = 35.5 kJ mol^–1 and ΔS = 83.6 JK^–1 mol^–1. The reaction is spontaneous at (Assume that ΔH and ΔS do not vary with temperature)

T < 425 K

T > 425 K

All temperatures

T > 298 K

Solution

B.

T > 425 K

∵ ΔG = ΔH – TΔS
For a reaction to be spontaneous, ΔG = –ve
i.e., ΔH < TΔS

therefore, T> ΔH/ΔS
= 35.5 x 103J/83.6JK^-1
i.e T>425 K

Some More Questions From Thermodynamics Chapter

Classify the following into different types of systems:
(i) Tea placed in a cup
(ii) Tea placed in a tea-pot
(iii) Tea placed in a thermosflask.

Define a closed system.

Define an isolated system.

Define intensive properties.

Define extensive properties.

Why all living systems need to be 'open systems'?

Define state variables of a system.

From thermodynamic point of view, to which system the animals and plants belong?

What is a state function?

A thermodynamic state function is a quantity

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