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.

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.

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aristocles aristocles · Answer 2 · 2019-10-06T04:57:08+02:00

Answer:

[tex]\delta Q = \delta E = 7.24 kJ[/tex]

Explanation:

Heat absorbed by the system is given as

[tex]\delta Q = 7.24 kJ[/tex]

now from first law of thermodynamics we know that

[tex]\delta Q = \delta E + W[/tex]

here

W = work done by the system

[tex]\delta E[/tex] = change in internal energy

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

[tex]W = 0[/tex]

so from above equation

[tex]\delta Q = \delta E = 7.24 kJ[/tex]