Question

1. A system releases 654 kJ of heat and does 140 kJ of work on the surroundings. What is the change in internal energy of the system?

2. How much heat is required to warm 1.30 L of water from 26.0 ∘C to 100.0 ∘C? (Assume a density of 1.0g/mL for the water.) Express your answer using two significant figures..

Answer 1

from first law of thermodynamics - tq = SU - w heat workdone Change in Internal energy Here we have - a q = -654 KT S-ve sign indicates heat is released} W = – 140 kJ work is done on of that means that I the system the surroundings / work is done by T and hence - ve plugging values in above eau- - 654 KJ = su - (- 140 kJ) SU = – 794 KJ Kindly submit seperately Different Please Questions Rate our