Answer:
(a) q positive; w negative.
(b) ΔE = -126 J
(c) E and ΔE
Explanation:
<em>(a) Determine whether the amounts of heat (q) and work (w) exchanged should have positive or negative signs. heat (q) positive negative work (w) positive negative</em>
By convention, when the system absorbs heat from the surroundings, its sign is positive, that is, q = 196 J.
By convention, when the system exerts work on the surroundings, its sign is negative, that is, w = -322 J.
<em>(b) Calculate the change in internal energy (ΔE) of the gas. J</em>
The change in internal energy (ΔE) can be calculated using the following expression.
ΔE = q + w
ΔE = 196 J + (-322 J) = -126 J
<em>(c) Determine whether one or more of the following is a state function:
</em>
<em>
internal energy (E) of a system,
</em>
<em>change in internal energy (ΔE) of a system,
</em>
<em>heat (q) absorbed or released by a system,
</em>
<em>work (w) done on or by a system.</em>
<em />
E and ΔE are state functions (they only depend on the states of the gas), whereas q and w depend on the trajectory.
