The first law of thermodynamics was given as `q=DeltaU+(-w)`, where `q` is heat given to a system and `DeltaU` represents increase in internal energy and `-w` is work done by the system. Various processes such as isothermal, adiabatic, cyclic, isobaric and isochoric process in terms of `I` law of thermodynamics leads for important results. The molar heat capacity for `1` mole of monoatomic gas is `3/2 R` at constant volume and `5/2 R` at constant pressure. Which of the following statements are correct? (1) Both work and heat appears at the boundaries of system. (2) Heat given to a system is given `+ve` sign. (3) Heat given to a system is equal to increase in internal energy under isothermal conditions (4) Heat given to a system is used to increase internal energy under isochoric conditions (5) Both work and heat are not state functions but their sum `(q+w)` is state function.A. `1,2,4,5`B. `1,3,4,5`C. `1,2,3,4`D. `2,3,4,5`