Asked by Nabi
The combustion reaction of propane (C3H8), a gas used for heating, is shown in the following thermochemical equation: C3H8+ 502 -->3CO2+4H2O deltaH = -2221kJ Calculate how much propane gas must be burned to obtain one amount of heat of 8 x 107 J, if the process has a yield of 60%
Answers
Answered by
DrBob222
If the yield were 100%, you would need this.
44 g C3H8 (1 mol) will produce 2221 kJ of heat, so you will need
44 g x (8 x 10^4 kJ/2221 kJ) = 1585 g to produce 8 x 10^7 J. For a reaction that is only 60% efficient, you will need
% yield = (actual yield/theoretical yield)*100
60 = (1585/X)*100 = ? where X = amount of C3H8 that must be used initially to produce 8E4 kJ @ 60% efficiency.
44 g C3H8 (1 mol) will produce 2221 kJ of heat, so you will need
44 g x (8 x 10^4 kJ/2221 kJ) = 1585 g to produce 8 x 10^7 J. For a reaction that is only 60% efficient, you will need
% yield = (actual yield/theoretical yield)*100
60 = (1585/X)*100 = ? where X = amount of C3H8 that must be used initially to produce 8E4 kJ @ 60% efficiency.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.