- #1

Any Help

- 79

- 2

## Homework Statement

A monatomic ideal gas undergoes the thermodynamic process shown in the PV diagram. Determine whether each of the values ΔU, Q, and W for the gas is positive, negative, or zero.

## Homework Equations

ΔU=Q-W

W=integral under the curve

PV=nRT T=PV/nR

## The Attempt at a Solution

direction is negative then the integral negative then

**work is negative**ΔU depends on change in temp, and here pressure increases and volume decreases so it was Ti=P0x2V0/nR and at final it becomes Tf=2P0xV0/nR Tf=Ti then it stays the same no change in temp then

**ΔU =0**therefore 0=Q-W Q=W but W negative then

*Q also negative*Is that correct? I need only to check my answer...

and is there any other way to determine Q from Graph (without looking at W or ΔU) ?