Calculate the Entalphy of Combustion: Calorimeter constant C from part A q = -0.23 J Tf - TI = ΔT 26.47°C-20°C ΔT= 6.47°C q/°c = -0.23 J/6.47°C = 0.04J/°C The calorimeter constant C = 0.04 J/°C Mass of the Metals MgO- 40.3044 grams k- 39.10 grams HCL- 36.5 grams/100 ml of 1 mole of HCL Questions: (B.3) Using the equation in B3 and your calorimeter constant C from Part A, calculate ΔHb for the reaction involving K with HCl. Report your value in units of kJ/mole. • K+HCL → KCL+H2

Could you do question C please

A container of water is heated with 10 J of energy at constant pressure. What is the enthalpy change (AH) for this process? O >10 J +10 J -10 J O <10 J O O J

Use the References to access important values if needed for this question Ethanol, C2H0, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to bum more efficiently in internal combustion engines. The combustion enthalpy of ethanol is 1366.9 kJ/mol The combustion enthalpy of 2-methylpentane, C6H14 is 4.157x103 kJ/mol. Calculate the energy released during the complete combustion of 382 g 2-methylpentane kJ Assuming the same efficiency, would 382 g ethanol provide more, less, or the same quantity of energy as 382 g 2-methylpentane? | Submit Answer Retry Entire Group 8 more group attempts remaining