$2 \cdot 5 \mathrm{~kJ}$ of work is done on the system and it releases $1500 \mathrm{~J}$ of heat. What is…

$2 \cdot 5 \mathrm{~kJ}$ of work is done on the system and it releases $1500 \mathrm{~J}$ of heat. What is the change in internal energy?
  1. $1000 \mathrm{~J}$
  2. $4000 \mathrm{~J}$
  3. $2500 \mathrm{~J}$
  4. $1500 \mathrm{~J}$

Solution

$\Delta U=q+w = -1500 + 2500 = 1000 ~J$

Asked in: MHT CET 2020 (20 Oct Shift 2)

Practice more Chemical Thermodynamics questions on Aicharya