Question

Calculate δe, if the system absorbs 7.24 kj of heat from the surroundings while its volume remains constant (assume that only p−v work can be done). express your answer using three significant figures.

Answer 1

I believe the answer is 7.24 kJ.
From the equation ΔE = dW + dQ; where W is the work done on/by the system and Q is the heat the system absorbs/loses.
Therefore; ΔE = 72.4 kJ since the system has bot done any p-v work (dV= zero) and has absorbed heat.

Answer 2

`\delta Q = \delta E = 7.24 kJ`

Step-by-step explanation:

Heat absorbed by the system is given as

`\delta Q = 7.24 kJ`

now from first law of thermodynamics we know that

`\delta Q = \delta E + W`

here

W = work done by the system

`\delta E` = change in internal energy

also we know that when volume of the system remains same then work done by the system must be zero

`W = 0`

so from above equation

`\delta Q = \delta E = 7.24 kJ`