In isobaric process, pressure is constant and volume increase from $V_1$ to $V_2$ due to the absorption of heat. According to the first law of thermodynamics, $\Delta U=q+W$
At constant pressure, $q_p=\Delta U-W$
$q_p=\Delta U-p\Delta V$
$q_p=U_2-U_1-\left(-p\left(V_2-V_1\right)\right)$
$q_p=\left(U_2+p{V}_2\right)-\left(U_1+p{V}_1\right)$
$q_p=H_2-H_1$
$q_p=\Delta H...\left(i\right)$
As we know, $\Delta H=\Delta U+p\Delta V$
$\Delta H=\Delta U+W$
Putting the value of $\Delta H$ in (1)
$q_p=\Delta U+W$
Other corrected options are as follows:
$•$ For adiabatic process, $\Delta U=W$
$•$ For an isochoric process, $\Delta U=q_v$
$•$ For an isothermal process $q=-W$