Prob_6.7_sol - It is 4745.47K b Stoichiometric combustion...

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Thermodynamics of Materials © John Kieffer, University of Michigan (2009) 3 Problem 6.7 a) Stoichiometric combustion in pure oxygen CH 4 + 2O 2 = CO 2 + 2H 2 O H = H CO 2 + 2 H H 2 O H CH 4 The enthalpy released by the reaction is H = –802300 J/mol, which is used to heat up the reaction products. Hence, H = a T 2 T 1 ( ) + b 2 T 2 2 T 1 2 ( ) + c 1 T 1 1 T 2 , or aT + b 2 T 2 c 1 T + H aT 1 b 2 T 1 2 + c 1 T 1 = 0 , where the coefficients are a = a CO 2 + 2 a H 2 O , b = b CO 2 + 2 b H 2 O , and c = c CO 2 + 2 c H 2 O . The root of the above function, i.e., the value of T for which the function is zero, yields the adia- batic flame temperature.
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Unformatted text preview: It is 4745.47K b) Stoichiometric combustion in air CH 4 + 2O 2 + 7.52N 2 = CO 2 + 2H 2 O + 7.52N 2 ∆ H The reaction enthalpy is the same as before. We again seek the root of aT + b 2 T 2 − c 1 T + ∆ H − aT 1 − b 2 T 1 2 + c 1 T 1 ⎛ ⎝ ⎜ ⎞ ⎠ ⎟ = , where the coefficients now are a = a CO 2 + 2 a H 2 O + 7.52 a N 2 , b = b CO 2 + 2 a H 2 O + 7.52 b N 2 , and c = c CO 2 + 2 c H 2 O + 7.52 c N 2 . The adiabatic flame temperature is 2329.56K...
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