Question

surroundings. Calculate the change internal energy (ΔE) for a system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings. 9.00 x 102 kJ 64.1 kJ -9.00 x 102 kJ -64.1 kJ -65.9 kJ

Answer 1

Answer:  -64.1 kJ.  

Explanation:

According to first law of thermodynamics:

$\Delta E=q+w$

$\Delta E$=Change in internal energy

q = heat absorbed or released

w = work done or by the system

w = work done by the system=$-P\Delta V$  {Work is done by the system is negative as the final volume is greater than initial volume}

w = -855 Joules = 0.855 kJ     (1kJ=1000J)

q = -65.0 kJ  {Heat released by the system is negative}

$\Delta E=-65.0J-(-0.855J)=-64.1kJ$

Thus the change internal energy (ΔE) for a system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings is -64.1 kJ.