Given below are two statements: One is labelled as Assertion A and the other is labelled as Reason R.
Assertion A: If $$d Q$$ and $$d W$$ represent the heat supplied to the system and the work done on the system respectively. Then according to the first law of thermodynamics $$d Q=d U-d W$$.
Reason R: First law of thermodynamics is based on law of conservation of energy.
In the light of the above statements, choose the correct answer from the options given below:
Match List I with List II
|List I||List II|
|A.||Isothermal Process||I.||Work done by the gas decreases internal energy|
|B.||Adiabatic Process||II.||No change in internal energy|
|C.||Isochoric Process||III.||The heat absorbed goes partly to increase internal energy and partly to do work|
|D.||Isobaric Process||IV.||No work is done on or by the gas|
Choose the correct answer from the options given below :
The graph between two temperature scales P and Q is shown in the figure. Between upper fixed point and lower fixed point there are 150 equal divisions of scale P and 100 divisions on scale Q. The relationship for conversion between the two scales is given by :-
According to law of equipartition of energy the molar specific heat of a diatomic gas at constant volume where the molecule has one additional vibrational mode is :-