a) Determine the enthalpy change for the reaction.
\(2NO_{2(g)} \rightarrow N_2O_{4(g)}\) at 70 $^\circ$C, using the following information:
\(NO_{2(g)}: \Delta H_{f298} = +33.18 \text{ kJmol}^{-1} \quad C_p = 37.20 \text{ Jmol}^{-1}K^{-1}\)
\(N_2O_{4(g)}: \Delta H_{f298} = +9.16 \text{ kJmol}^{-1} \quad C_p = 77.28 \text{ Jmol}^{-1}K^{-1}\)
b) Bromine is 18 % dissociated at 2000 K and 1 bar. Calculate --
i. Equilibrium Constant, K.
ii. Standard Gibbs Free Energy, $\Delta G_r\theta$
iii. K at 2500 $^\circ$C, given that $\Delta H_r\theta = +112 \text{ kJ/mol}$.
[10 marks]
[15 marks]
[5 marks]
[10 marks]
