A reaction at 4.62 atm produces 22.1 L of a gas and evolves 83.3 kJ of heat (exo

Question

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: 72.95 1.768 g of an unknown hydrocarbon (105.6 g/mol) burns in bomb calorimeter in excess oxygen. The heat capacity of the calorimeter,CV,-5539 kJ/°C and AT-6.874 °C. Find AE for this hydrocarbon in kJ/mol. Hint given in feedback. Answer: Calculate ?? per g and then convert to ?? per mole. Is ?? (-) or (+)? Using the technique of the previous problem ?? 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, 3 moles of oxygen gas are consumed and 6 moles of CO2 gas and 6 moles of H20 liquid are produced. Find AH per mole of this hydrocarbon (in kJ) at 298 K. 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) +2.502(9)-2CO2(g)+ 3H200) Answer:

Explanation / Answer

Solution :-

Work= pressure*volume= (4.62 atm)*(22.1L)= 102.102
1L*atm= 101.325 Joules
(101.102 L*atm)(101.325Joules)=10244.16J*(1kJ/1000J)=10.244kJ

E=q+w
E=-83.3+(-10.244kJ)= -93.544kJ

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