Please a) Is this reaction exothermic or endothermic? Explain.b) How much heat is released when a 5.00 g sample of benzene is burned in excess oxygen under standard conditions?c) How much heat is released when 100.0 g of water is produced under standard conditions? ### Thermochemical Equation for the Burning of BenzeneBelow is the thermochemical equation for the combustion of benzene under standard conditions:\[ 2 \, \text{C}_6\text{H}_6 (l) + 15 \, \text{O}_2 (g) \rightarrow 12 \, \text{CO}_2 (g) + 6 \, \text{H}_2\text{O} (g) \]**Enthalpy Change (\( \Delta H \))**: -3267.7 kJ**Calculations:**- ___ moles of \(\text{C}_6\text{H}_6\) = -3267.7 kJ- ___ moles of \(\text{O}_2\) = -3267.7 kJ- ___ moles of \(\text{CO}_2\) = -3267.7 kJ- ___ moles of \(\text{H}_2\text{O}\) = -3267.7 kJ\[\begin{align*}\frac{-3267.7 \, \text{kJ}}{\text{mol}} & \\\frac{-3267.7 \, \text{kJ}}{\text{mol}} & \\\frac{-3267.7 \, \text{kJ}}{\text{mol}} & \\\frac{-3267.7 \, \text{kJ}}{\text{mol}} &\end{align*}\]Each component of the reaction has an energy change of -3267.7 kJ, indicating the exothermic nature of the reaction.

Given: The reaction is as follows: 2 C6H6(l) + 5O2(g) ------------------> 12CO2(g) +6 H2O(g). The heat of reaction = The molar mass of benzene = 78.11 g/mol. The molar mass of water = 18 g/mol. a). Since the heat of reaction is negative therefore the reaction is exothermic. b). When 5 g Benzene is burned it produces heat, which is calculated as follows: We know that. 2 mol of C6H6 reacts to give = -3267 kJ of heat. 2*(78.11) g of C6H6 reacts to give = -3267 kJ of heat. 156.22 g of C6H6 reacts to give = -3267 kJ of heat. 156.22 g of C6H6 reacts to give = - (3267/156.22) kJ. 5 g of C6H6 reacts to give = - (3267/156.22)*5 kJ. = 104.564 kJ. (Answer) c). When 100 g of water is produced the heat produced is calculated as follows: 6 moles of water is produced when = - 3267 kJ of heat is released. 6*(18) g of water is produced when = - 3267 kJ of heat is released. 108 g f water is produced when = - 3267 kJ of heat is released. 1 g of water is produced when = - (3267/108) kJ of heat is released. 100 g of water is produced when = - (3267/108)*100 kJ of heat is released. = - 3025 kJ of heat is released. (Answer)