Butane (c4 h10(g), mc031-1.jpghf = –125.6 kj/mol) reacts with oxygen to produce carbon dioxide (co2 , mc031-2.jpghf = –393.5 kj/mol ) and water (h2 o, mc031-3.jpghf = –241.82 kj/mol) according to the equation below. mc031-4.jpg what is the enthalpy of combustion (per mole) of c4h10 (g)? use mc031-5.jpg. –2,657.5 kj/mol –5315.0 kj/mol –509.7 kj/mol –254.8 kj/mol

The balanced chemical equation for the combustion of butane is:

Δ = ΣΔ-ΣΔ

                         = =[-3148kJ/mol+(-2418.2kJ/mol)]-[(-251.2kJ/mol)+0]

                      = -5315 kJ/mol

Calculating the enthalpy of combustion per mole of butane:

Therefore the heat of combustion per one mole butane is -2657.5 kJ/mol

Correct -2657.5 kJ/mol

b is the correct answer

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question: ray weighs 100 kilograms, his wrestling partner, bobby, weighs 50 kilograms. if ray moves at 4 m s , how fast will bobby have to run at him to apply an equal amount of kinetic energy?

answer: 8 m/s he needs to run twice as fast to keep up so he has some work to do

explanation:   if the mass has units of kilograms and the velocity of meters per second, the kinetic energy has units of kilograms-meters squared per second squared.

question answered by

(jacemorris04)