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# What is the heat of combustion per gram of butane?

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5. The combustion of butane produces heat according to the equation
2C4H10(g) + 13O2(g) &#61614; 8CO2(g) + 10H2O(l) &#61508;H° = -5,314 kJ
What is the heat of combustion per gram of butane?
A.-32.5 kJ/g
B.-45.7 kJ/g
C.-91.5 kJ/g
D.-2,656 kJ/g
E.-15,440 kJ/g

6. The freezing of water is an example of an exothermic change.

7. Calcium oxide and water react in an exothermic reaction.
CaO(s) + H2O(l) &#61614; Ca(OH)2(s) &#61508;H° = -64.8 kJ/mol
How much heat would be liberated when 7.15 g CaO(s) is dropped into a beaker containing 152 g H2O?
A.1.97 x 10-2 kJ
B.8.26 kJ
C.508 kJ
D.547 kJ
E.555 kJ

8. How much heat is absorbed in the complete reaction of 3.00 grams of SiO2 with excess carbon in the reaction below? &#61508;H0 for the reaction is +624.6 kJ.

SiO2(g) + 3C(s) &#61614; SiC(s) + 2CO(g)
A.366 kJ
B.1.13 &#61620; 105 kJ
C.5.06 kJ
D.1.33 &#61620; 104 kJ
E.31.2 kJ

See attached file for full problem description.

https://brainmass.com/chemistry/physical-chemistry/what-is-the-heat-of-combustion-per-gram-of-butane-101236

#### Solution Preview

5. The combustion of butane produces heat according to the equation
2C4H10(g) + 13O2(g) &#61614; 8CO2(g) + 10H2O(l) &#61508;H° = -5,314 kJ
What is the heat of combustion per gram of butane?
The heat given is per mol of butane. Molecular weight of butane is:
4*12+10=58 (g/mol)
So heat per g is -5,314/58 = -91.6 ...

#### Solution Summary

The solution provides detailed explanations and answer for the problem.

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## Determining amount of chemical consumed

The combustion of butane in oxygen at 25 celsius to form water and carbon dioxide follows the chemical reaction:
2 C4H10(gas) + 13 O2(gas) = 8 CO2 (gas)
(the = is supposed to be a forward arrow)

The reaction is carried out in an excess oxygen atmosphere, and 1585 kJ heat is released. Determine the amount of butane consumed.

May use following info:
deltaH C4H10= -124.73 kJ/mol
deltaH H2O= -285.83 kJ/mol
deltaH CO2= -393.5 kJ/mol
deltaH O2= 0 kJ/mol

I am only able to solve the first half of the problem, for deltaH of the whole reaction= -6006.3 kJ/mol, now what??Thanks..

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