Given the thermochemical data, \(\mathrm{A}+\mathrm{B} \longrightarrow 2
\mathrm{C} \quad \Delta H_{1}=600 \mathrm{~kJ} / \mathrm{mol}\)
\(\begin{array}{ll}2 \mathrm{C}+\mathrm{D} \longrightarrow 2 \mathrm{E} &
\Delta H_{1}=210 \mathrm{~kJ} / \mathrm{mol}\end{array}\) Determine the
enthalpy change for each of the following:
a) \(4 \mathrm{E} \longrightarrow 4 \mathrm{C}+2 \mathrm{D}\)
d) \(2 C+2 E \longrightarrow 2 A+2 B+D\)
b) \(\mathrm{A}+\mathrm{B}+\mathrm{D} \longrightarrow 2 \mathrm{E}\)
e) \(\mathrm{E} \longrightarrow \frac{1}{2} \mathrm{~A}+\frac{1}{2}
\mathrm{~B}+\frac{1}{2} \mathrm{D}\)
c) \(\mathrm{C} \longrightarrow \frac{1}{2} \mathrm{~A}+\frac{1}{2}
\mathrm{~B}\)