The relation $q = -w$ is $NOT$ true for which of the following processes?

Calculate $\Delta H$ for the following reaction at $25^{\circ} C$.
$NH_2CN_{(g)} + \frac{3}{2} O_{2_{(g)}} \longrightarrow N_{2_{(g)}} + CO_{2_{(g)}} + H_2O_{(l)}$
$(\Delta U = -740.5 \ kJ, R = 8.314 \ J \ K^{-1} \ mol^{-1})$

In a $1 \, L$ container,$2 \, mol$ of $CO$ and $1 \, mol$ of $O_2$ are taken. They react according to the equation: $2CO(g) + O_2(g) \rightarrow 2CO_2(g)$,$\Delta H = -560 \, kJ$. Given that $1 \, atm \cdot L = 0.1 \, kJ$,and the pressure changes from $70 \, atm$ to $40 \, atm$ at $500 \, K$,calculate the value of $\Delta U$ in $kJ$.

Which of the following expressions represents the first law of thermodynamics?

When a gas undergoes adiabatic expansion,it cools down because:

$A$ gas expands from a volume of $4 \ L$ to $14 \ L$ against a constant external pressure of $1 \ atm$ in a cylinder with a frictionless piston. During this process,the gas absorbs $800 \ J$ of heat from the surroundings. Calculate the change in internal energy $\Delta E$ in $J$. (in $.7$)