NAME Question 5 (4 pts) How much heat is produced by the combustion of 50.0 mL o
ID: 1047018 • Letter: N
Question
NAME Question 5 (4 pts) How much heat is produced by the combustion of 50.0 mL of ethanol, CHsOH, forming carbon dioxide and liquid water? Start by writing a balanced reaction equation, then calculate the heat in kilojoules. You can find the enthalpy change for the reaction steps, DH, in chapter 5 or in Appendix G. The density of liquid ethanol is 0.789 g/mL Question 6 (5 pts) Calculate heat of formation of SO; under nonstandard state conditions, given the following equations AH 89.5 kJ AH -204.2 kJ Question 7 (5 pts) Calculate AHnn for the following reaction using Hess's Law 2NOCI(g) N2(g) +02(g) + Cl(g) given the following set of reactions Hint: To obtain the overall reaction, first determine whether the given sets of reactions are forward or reverse reactions for the overall reaction. Write out all equations following the example in the slides and in the textbook The nutritional calorie (Calorie) is equivalent to I kcal. One pound (1.00 lb) of body fat is equivalent to 4.086 x 10 kcal. Express this quantity in joules and kilojoules. Use scientific notation for your answer! Question 8 (6 pts) Energy Calculations a) b) If an athlete expends 2250 kJ/h (kilojoules per hour), how long does he have to exercise to work off 1.0 lb of body fat? The average amount of calories burned during running is 125 kcal/mile. How many miles does this athlete have to run to burn off 1.0 lb of body fat? c)Explanation / Answer
Ans 5 :
The balanced chemical equation is given as :
C2H5OH + 3O2 = 2CO2 + 3H2O
The enthalpy change associated with 1 mole = -1360 KJ/mol
The mass of 50 mL = 0.789 x 50 = 39.45
Number of moles = 39.45 / 46.07 = 0.856 mol
So the heat produced = 0.856 x 1360
= 1164.6 KJ
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