Question

How much heat is needed to increase the internal energy of a gas in a piston by 3426 J if the gas does 537 J of work on the environment by expanding if the process?

Answer 1

Given:

the internal energy of the gas is

`\Delta U=3426`

The work done on the gas is

`W=537\text{ J}`

Required: heat needed to increase the internal energy

Step-by-step explanation:

from the first law of the thermodynamics

we can write,

`\Delta Q=\Delta U+W`

Plugging all the values in the above relation, we get

`\begin{gathered} \Delta Q=3426\text{ J+537 J} \\ \Delta Q=3963\text{ J} \end{gathered}`

Thus, the heat needed

`3963\text{ J}`