Problem 3 For the reaction 2C6H5COOH(s) + 13 O2(g) → 12CO2(g)+6 H₂O(g), Δευθ =-772.7 kJ mol¹ at 298 K. Calculate A, He

Problem 4The following chemical reaction can be used to convert furfural (C5H4O2) into methyl-tetrahydrofuran (C5H10O, methyl-THF):4 H2(g) + C5H4O2(l) −−→ C5H10O(l) + H2O(l) (2) 4a. Use the following information to calculate ∆H◦rxn and ∆U◦rxn for the above reaction (all at 298 K): C5H4O2(l) + 5 O2(g) −−→ 5CO2(g) + 2 H2O(l) (∆H◦1 = −2344 kJ/mol)C5H10O(l) + 7 O2(g) −−→ 5CO2(g) + 5 H2O(l) (∆H◦2 = −3122 kJ/mol)H2(g) + 12O2(g) −−→ H2O(l) (∆H◦3 = −286 kJ/mol)4b. The above reaction is of interest for renewable fuel production. Furfural can be readily obtained from renewable sources by dry distillation of biomass (wood, etc) but is poorly stable on exposure to air. Conversion to methyl-THF results in a more stable compound that is suitable as a motor fuel. Suppose the reaction is to be run on a large scale in a chemical plant. Will it require heating or cooling in order to maintain a constant reaction temperature? Briefly justify your answer.

Problem 2 The chemical reaction for photosynthesis is represented by the following unbalanced equation: CO2 + H₂O + hv→ C6H12O6+ O2 a) Balance the equation. b) If the reaction requires an input of energy (sunlight) to proceed, is the reaction endothermic or exothermic? c) Calculate the heat of reaction AH to see how much energy is required, given the standard enthalpy for glucose C6H12O6 is -1273.3 kJ/mol. Answer: 2,803 kJ/mol d) If an average tree produces 260 lbs. of oxygen per year, how many kilograms of carbon dioxide does it take up? Answer: 162.2 kg CO₂ e) What wavelength is necessary to drive this reaction if it takes one photon to dissociate one molecule? Answer: 0.0425 µm

What is the energy change of the reaction when 13.0g of NO₂ reacts by the below reaction? 2NO₂ → N₂ +20₂ AH = +225kJ - A) +15.9kJ B) +31.8KJ Question 45 of 50 C) +63.6kJ D) -63.6kJ E) 2900kJ