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..© BrainMass Inc. brainmass.com February 24, 2021, 2:31 pm ad1c9bdddf
Number of moles of CO2 formed = 1585/6006.3 = 0.2639 moles
When 8 moles of CO2 are ...
The expert determines the amount of chemicals consumed. The excess oxygen atmosphere is analyzed.