Short Answer Type
Long Answer TypeShort Answer TypeCalculate the maximum work obtained when 0.75 mol of an ideal gas expands isothermally and reversibly at 27°C from a volume of 15L to 25L.
State first law of thermodynamics in different ways.
(i) Energy can neither be created nor destroyed, though it may be converted from one form into another.
(ii) The total energy of an isolated system remains constant, although there may be internal changes in the state of the system.
(iii) It is impossible to construct a perpetual motion machine i.e. a machine that can produce work without any expenditure of energy.
(iv) Total energy of a system and its surrounding such as universe remains constant in any physical or chemical process.
If water vapour is assumed to be a perfect gas,
molar enthalpy change for vapourisation of 1 mol of water at 1bar and 100°C is 41kJ mol–1. Calculate the internal energy change, when
(i) 1 mol of water is vaporised at 1 bar pressure and 100°C.
Long Answer TypeDerive mathematical form of First law of Thermodynamics.
Or
Derive the relationship between heat, internal energy and work.
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