Respuesta :
Answer: The internal energy change for the reaction is -2850 J
Explanation:
- Sign convention of heat:
When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.
- Sign convention of work:
Work done for expansion process is taken as negative and work done for compression is taken as positive.
According to the First law of thermodynamics,
[tex]\Delta U=q+w[/tex]
where,
[tex]\Delta U[/tex] = internal energy
q = heat absorbed or released = -2290 J
w = work done = -560 J
Putting values in above equation, we get:
[tex]\Delta U=(-2290)+(-560)\\\\\Delta U=-2850J[/tex]
Hence, the internal energy change for the reaction is -2850 J
The internal energy change for this reaction is 1- –2850 J
Given that,
- A sample of octane burns releasing 2290 J of heat to the surroundings, and the gases produced expands against a piston to do 560 joules of work.
The calculation is as follows:
=-2290 - 560
= -2850J
Find out more information about the heat here:
https://brainly.com/question/1429452?referrer=searchResults
