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The heat of combustion of butane is -2877 kJ/mol. Use this to find the heat of formation of butane. 

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Patrick Suarez
Patrick SuarezLv10
21 Nov 2020

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Related questions

The heat of combustion for two moles of butane is -5755 Kj Calculate the heat of formation of butane given that Heat of formation of water = -285.3 kJ/mol and heat of formation of CO2 = -393.5 Kj/mole

A student wishes to raise the temperature of 5.00 kg of water by 35.4 degrees C Assuming that there is no loss of heat to environment, how many grams of butane need to react with oxygen Specific heat of water = 4.18J/g C

Given that the heat of combustion for butane is −2657⋅kJ⋅mol−1, what is the heat of combustion for butane in J⋅g−1?

250 mL of water is heated from 3 oC to 90 oC on a butane stove. Assume all the heat from combustion is used to warm the water.

C4H10(g) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(l)

Standard Enthalpies of Formation (ΔHof):

C4H10(g) = -124.8 kJ/mol

CO2(g) = -393.5 kJ/mol

H2O(l) = -285.8 kJ/mol

a. What is the total amount of heat required for the process?

b. What is the molar heat of combustion for butane?

c. What is the mass of butane needed for this process?

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