For a certain change, value of Delta U is -2.37 kJ. During the change, the system absorbs 650 joules. How much work did the system do?

Question

For a certain change, value of Delta U is -2.37 kJ. During the change, the system absorbs 650 joules. How much work did the system do?

Please help! I get 3.02 but is not correct!!

Answer 1

To find the work done by the system, you'll need to use the first law of thermodynamics, which states that the change in internal energy (ΔU) of a system is equal to the heat absorbed by the system (q) minus the work done by the system (w).

ΔU = q - w

Given that ΔU is -2.37 kJ and q is 650 J (remember to convert it to kJ), you can plug these values into the equation:

-2.37 kJ = 0.65 kJ - w

To solve for w, rearrange the equation:

w = 0.65 kJ - (-2.37 kJ)
w = 0.65 kJ + 2.37 kJ

Now, add the values:

w = 3.02 kJ

So the work done by the system is 3.02 kilojoules (kJ).

Therefore, your answer of 3.02 kJ is correct. Make sure to double-check your calculations or any rounding errors that might have led to the incorrect result you mentioned earlier.

For a certain change, value of Delta U is -2.37 kJ. During the change, the system absorbs 650 joules. How much work did the system do?

its -3.02

To find the work done by the system, you'll need to use the first law of thermodynamics, which states that the change in internal energy (ΔU) of a system is equal to the heat absorbed by the system (q) minus the work done by the system (w).