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Thermodynamics
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
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
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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.
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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.
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What is a state function?
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