When cyclohexane (C6H12) is burned in excess oxygen to produce carbon dioxide ga

Question

When cyclohexane (C6H12) is burned in excess oxygen to produce carbon dioxide gas and liquid water, it releases 3919kJ of heat per mole of cyclohexane burned.

A) Write the balanced chemical equation that corresponds to this reaction.

B) If 15g cyclohexane is burned in a calorimeter with a heat capacity of 230kJ/K, what temperature change do you expect (assuming that all the heat is deposited in the calorimeter)?

C) How much heat is associated with the production of 5.5g water?

D) What is the (Delta H(f)) of cyclohexane, given that the (delta H(f)) of H20(g) is -242 kJ, the (delta H(f)) of CO2(g) is -393.5kJ, the reaction CO2(s)=CO2(g) has a (delta H) of 25.2kJ and the reaction H20(l)=H20(g) has a (delta H) of 44kJ.

Explanation / Answer

C6H12 + 9O2 --> 6CO2 + 6H20 dH = -3919 KJ......... When one mole (84 grams) C6H12 is burned, 3919 KJ heat is evolved.. When 15g is burned, Heat = q = 15 x 3919 /84 = 699.8 = 700 KJ... Hence temperature change is T = 700 KJ /230 = 3.04 K... 6 moles of water (108g) is formed with evolution of 3919KJ.. 5.5g water is produced with evolution of heat = q1 = 5.5 x 3919 / 108 = 199.6 = 200 KJ... Delta H(f) is calculated when one mole of compound is formed from its elements... 6C + 6H2 --> C6H12 By summing up various reactions and their heats properly, you get Delta H(f) of C6H12.. I think the data you provided for this calculation is not sufficient... If you think it is sufficient, then this part of question is out of my bounds... PLZ RATE ME FOR THE REST... THANK YOU...

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