Heat of Reaction Use the heat of formation method to calculate the heat of reaction at standard temperature and pressure for the following reactions. Categorize each reaction as endothermic or exothermic. Where appropriate, assume the phase of each species and clearly state the justification 1. Hydrogenation CO, +3H2 → CH3OH + H2O 2. Alkane cracking C2H6 → C2H4 + H2 3. Photosynthesis 6CO2(g) + H2O(1) → C6H12O6(aq) + 60(g) What about cellular respiration? Will it be endothermic or exothermic? Heat of Combustion Use the heat of formation method to calculate the heat of combustion and compare your value to the one given in the table. Which phase will you choose for each species? Why? 1. CH + 20 → CO2 + 2H2O 2. 2CH. + 250 → 16CO2 + 187,0 Adiabatic Flame Temperature Pure methane is combusted with air (21mol% 0, 79mol% N.) in an adiabatic process. The combustion of methane is given as: CH4 + 2O → CO + 2H2O The nitrogen is non-reactive but plays a role in the energy balance. The air is fed such that there is a 100% excess of oxygen and the methane is completely consumed. The inlet stream has a temperature of 25°C.1. What is the molar flow rate of each species, including nitrogen, in each stream? 2. What is the temperature of the outlet stream? Reactive Energy Balance Ethane is cracked to form ethylene in a high temperature process. C₂H₂ → C₂H₂ + H₂The process occurs in a continuous flow reactor. The inlet feed is pure ethane at 100°C. The outlet stream is a mixture of ethylene, hydrogen, and unreacted ethane at 850°C. If the fractional conversion of ethane is 65%, how much heat must be supplied to the process?