(Solved): can you help with these questions. and show the steps  2) The oxidation of hydrazine, \( \mathr ...

2) The oxidation of hydrazine, \( \mathrm{N}_{2} \mathrm{H}_{4} \) by hydrogen peroxide forms nitrogen gas and water vapour. The standard enthalpies of formation, \( \Delta \mathrm{H}^{\circ} \mathrm{f}\left(\mathrm{kJmole}^{-1}\right) \) at \( 25^{\circ} \mathrm{C} \) for hydrazine, hydrogen peroxide and water vapour are \( +50.63,-187.8 \) and \( -241.8 \) respectively. i) Write the equation involved for above reaction. (2 marks) ii) What is the temperature rise if the heat released from the oxidation of \( 2.0 \mathrm{~g} \) hydrazine by \( 10.0 \mathrm{~g} \) of hydrogen peroxide is used to warm up \( 1 \mathrm{dm}^{3} \) of water? Given: \( \mathrm{c}=4.2 \mathrm{~J} \mathrm{~g}^{-1}{ }^{\circ} \mathrm{C}^{-1} \) (8 marks) 3) Calculate the heat of the following unbalanced equation using the heat of formation \( \left(\Delta \mathrm{H}_{f}\right. \) ') at \( 298 \mathrm{~K}, 1 \mathrm{~atm} \). from the given table. a. \( \mathrm{Fe}(s)+\mathrm{CO}_{2}(\mathrm{~g}) \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(\mathrm{g}) \) (2 marks) Heats of Formation: \[ \begin{array}{l} \mathrm{CO}_{2}(\mathrm{~g})=-393.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})=-824.2 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{CO}(\mathrm{g})=-110.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{array} \] b. \( \mathrm{C}_{3} \mathrm{H}_{8} \) (l) \( +\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \) (2 marks) Heats of Formation: \[ \begin{array}{l} \mathrm{C}_{3} \mathrm{H}_{8}(\mathrm{l})=-103.8 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{CO}_{2}(\mathrm{~g})=-393.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{H}_{2} \mathrm{O}(\mathrm{g})=-242.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{array} \]