Question

A system receives 575 ) of heat and delivers 425 ) of work. Calculate the change in the internal energy. AE, of the system.​

Answer 1

Answer:

ΔE = 150 J

Explanation:

From first law of thermodynamics, we know that;

ΔE = q + w

Where;

ΔE is change in internal energy

q is total amount of heat energy going in or coming out

w is total amount of work expended or received

From the question, the system receives 575 J of heat. Thus, q = +575 J

Also, we are told that the system delivered 425 J of work. Thus, w = -425 J since work was expended.

Thus;

ΔE = 575 + (-425)

ΔE = 575 - 425

ΔE = 150 J

Answer 2

After applying the first law of thermodynamics, the change in the internal energy of the system is 150 Joules.

Given the following data:

• Quantity of heat = 575 Joules

• Work done = 425 Joules

To find the change in the internal energy of the system, we would apply the first law of thermodynamics.​

Mathematically, the first law of thermodynamics is given by the formula:

$\Delta E = Q - W$

Where;

• $\Delta E$ is the change in internal energy.

• Q is the quantity of heat absorbed.

• W is the work done.

Substituting the given parameters into the formula, we have;

$\Delta E = 575 - 425$

Change in internal energy, E = 150 Joules

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