Question 7 Not answered Marked out of 1.00 A reaction at 4.62 atm produces 22.1

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Question 7 Not answered Marked out of 1.00 A reaction at 4.62 atm produces 22.1 L of a gas and evolves 83.3 kJ of heat (exothermic). Calculate the change in internal energy of the system (in kJ) Answer Flag question Question 8 Not answered Marked out of 1.00 1.726 g of an unknown hydrocarbon (89.4 g/mol) burns in bomb calorimeter in excess oxygen. The heat capacity of the calorimeter,Vy-5.615 kur and 7-6.713 °C Find E for this hydrocarbon in kJ/mol Hint given in feedback. Flag question Answer: Calculate E per g and then convert to E per mole. IsE (-) or (+)? Question 9 Not answered Marked out of Using the technique of the previous problem E was found to be-2,000.00 kJ/mol of an unknown liquid hydrocarbon at 298 K. In another experiment it was determined that for each mole of hydrocarbon, 5 moles of oxygen gas are consumed and 8 moles of CO2 gas and 7 moles of H2O liquid are produced. Find AH per mole of this hydrocarbon (in kJ) at 298 K. 1.00 Flag question Hint given in feedback. Not used to answer question: This question is a bit awkward and unrealistic for molar amounts, but allows for random numbers. An example of a possible reaction is: C2H4(OH)2(I) +2.502(g) 2CO2(g)+ 3H20(1) Answer:

Explanation / Answer

7)

Q = -83.3 KJ (negative because heat is evolved)

W = -P*delta V

= -4.62 atm * 22.1 L

= -102.1 atm.L

= -102.1*101.33 J

= -10346 J

= -10.3 KJ

Now use:

delta U = Q+W

= -83.3 KJ -10.3 KJ

= - 93.6 KJ

Answer: - 93.6 KJ

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