(15 points) Unfortunately, if we just burn our octane in the atmosphere, all of
ID: 548184 • Letter: #
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(15 points) Unfortunately, if we just burn our octane in the atmosphere, all of the energy that is released is in the form of heat which will keep one warm but not move the car anywhere (e learn in chapter 9 exactly how much energy is released). In order to capture the energy, we must burn the fuel) i turn to mechanical energy. Let's assume we have a 4L 4-cylinder engine, so closed expandable container) hold n a closed (but expandable) container so we can convert the heat to pressure and in each cylinder (the s a maximum of IL Air consists o approximately 78% nitrogen, 21% oxygen with the remaining 1% a mixture of other gasses (the percentages given are molar percentages). Assume we want to intake into the 1L cylinder contains the exact stoichiometric mi water (part b). a mixture of octane vapor and air that of air and octane to be burned completely to CO2 and How many moles of CH and oxygen will be in the container under these conditions re and room temperaturer25 C)? For this and subsequent parts of this question, assume ideal gas behaviour. Cetlhe 21% conger Yo otherExplanation / Answer
the combustion of C3H8 is C3H8 + 5O2---->3CO2+ 4H2O
1 mole of C3H8 requires 5 moles of oxygen to undergo complete combustion.
From gas law, moles, n = PV/RT, P=1atm . V =1 L, R=0.0821 L.atm/mole.L, T=298K
n= 1*1/(0.0821*298)= 0.0408 moles of mixture.
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