Answer
a) $0\;\rm J$
b) $-344\;\rm J$
Work Step by Step
We have two processes, an adiabatic process, and an isothermal process.
$\bullet$ For the adiabatic process,
$$Q=\color{red}{\bf0}\;\rm J$$
since we know that there is no heat exchange during an adiabatic process.
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$\bullet$ For the isothermal process, we know that the temperature is constant.
So,
$$\Delta E_{th}=Q+W=0$$
Hence,
$$Q=-W=-\left[-\int PdV\right]$$
$$Q= \int PdV $$
Recalling that $P=nRT/V$,
$$Q= \int_i^f \dfrac{nRT}{V}dV=nRT\ln\left[\dfrac{V_f}{V_i}\right] $$
$$Q=nRT\ln\left[\dfrac{V_f}{V_i}\right] \tag 1$$
Now we need to find $T$;
$$T=\dfrac{P_fV_f}{nR}$$
$$T=\dfrac{(3\times 1.013\times 10^5)(1000\times 10^{-6})}{(0.10)(8.31)}=\bf 366\;\rm K$$
Plugging into (1);
$$Q=(0.10)(8.31)(366)\ln\left[\dfrac{1000}{3000}\right] $$
$$Q=\color{red}{\bf -334}\;\rm J$$
