3. When 6.6 g of compound X (MW = 66.6g/mol) was burned in a constant-volume bom

Question

3. When 6.6 g of compound X (MW = 66.6g/mol) was burned in a constant-volume bomb calorimeter, the water temperature rose from 20.00 oC to 26.66 oC. If the mass of water surrounding the calorimeter was exactly 666 g and the heat capacity of the bomb calorimeter was 0.666 kJ/oC without water, calculate the molar heat of combustion at constant volume of compound X. The specific heat of water is 4.184 J/g·oC. (a) -103 to -104 kJ/mol; (b) -103 to -102 kJ/mol: (c) -100 to 100 kJ/mol; (d) 103 to 102 kJ/mol:; (e) >1000 kJ/mol

Explanation / Answer

Heat taken be water= mass*specific heat* temperature difference= 666*4.14*(26.66-20.00)=18363.22 joules

Moles of compound =6.6/66.6=0.099 moles

heat taken by water = 18363.33/0.099=185301.6 joules= 185.3016 KJ

heat taken be bomb calorimeter= 0.666*(26.66-20.00)=4.43 KJ

net heat= 185.3016-4.43= 180.8Kj/mol

None of the above

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