3.6 L of an ideal diatomic gas A, at P = 1.15 atm is confined in a rigid vessel and held at a constant temperature of T = 45 °C. The gas then undergoes monomolecular decay where every molecule decays A2 → 2A. What is the final pressure after this reaction? State your answer in atm without units.

A 7.00 L tank at 15.8 °C is filled with 5.07 g of sulfur tetrafluoride gas and 11.5 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: x10 sulfur tetrafluoride partial pressure: || atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm

16. The combustion of gasoline (octane) in a car engine can be represented by the following equation: 2C3H18(1) + 2502(g) a. What mass of oxygen is used up to burn a full tank of 36.00 kg of gasoline? Text --> 16CO2(g) +18H20(g) b. Why might a vehicle that is calibrated to run perfectly at sea level run poorly at higher elevations? Text Тext According to the Canadian Automobile Association, the average Canadian drives 20,000 km/yr. C. Assuming that distance, how many more kg of carbon dioxide are added to the atmosphere each year by a Toyota Tacoma (fuel economy of 12.8 L/100 km) than a Toyota Prius (4.52 L/100 km)? The density of gasoline is 0.719 kg/L.

Sample Experimental Values: Reaction 1: Both reactants are 2M Reaction 2: Both Reactants are 2M NaOH (aq) + HCl (aq) → H₂O (1) + NaCl (aq) 1 Reaction 2 NaOH (aq) + CH3COOH (aq) → H₂O (1) + NaCH3COO (aq) Temperature Change 20 C 8 C Volume of Reactants 25.0 mL NaOH 25.0 mL HCI 10.0 mL NaOH 10.0 mL CH3COOH Final Mass of Solution 50.0 g 20.0 g 2. Using the sample experimental values, answer the questions below. a. Show the calculation used to determine how much heat was produced for both reactions. Report your answer in Joules. b. How much heat was released per mole of acid? (Hint: think about the concentration of the reactants and their respective volumes used. Report answer for both reactions in kJ/mol) What is the vocabulary chemists use to describe this experimental value? 3. Based on the experimental evidence, how is the heat of neutralization related to the strength of the acid?