(a) Explanation Express the complete combustion reaction with theoretical air. [ [ 0 .973CH 4 + 0.023 CO 2 + 0.014 N 2 ] + a ( O 2 + 3.76 N 2 ) ] → ( b CO 2 + c H 2 O + d N 2 ) (I) Here, Methane is CH 4 , hydrogen is H 2 , oxygen is O 2 , nitrogen is N 2 , carbon dioxide is CO 2 , water is H 2 O and number of moles of oxygen, carbon dioxide, water and nitrogen is a , b , c , and d respectively. Conclusion: Apply the conservation of mass principle to the carbon, hydrogen, oxygen, and nitrogen, respectively, results in four equations among the four unknowns: Perform carbon balance: 0.973 + 0.023 = b b = 0.996 Perform hydrogen balance: 2 c = ( 4 ) ( 0.978 ) c = 1.946 Perform oxygen balance: 2 ( 0.23 ) + 2 a = 2 ( 0.996 ) + 1.946 a = 1.946 For the complete combustion reaction with actual air [ [ 0 .973CH 4 + 0.023 CO 2 + 0.014 N 2 ] + a ( O 2 + 3.76 N 2 ) ] → b ( 9.2 CO 2 + 3.84 O 2 + 0.64 CO + 86.32 N 2 ) + c H 2 O (II) Apply the conservation of mass principle to the carbon, hydrogen, oxygen, and nitrogen, respectively, results in four equations among the four unknowns: Perform carbon balance: 0.973 + 0.023 = b ( 9.2 + 0.64 ) b = 0 (b) To determine The dew point temperature of the product.

Fundamentals of Engineering Thermodynamics

8th Edition

ISBN: 9781118832301

Author: SHAPIRO

Publisher: JOHN WILEY+SONS,INC.-CONSIGNMENT

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Chapter 13.8, Problem 35P

(a)

To determine

The percent of theoretical air.

(b)

To determine

The dew point temperature of the product.

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Chapter 13.8, Problem 34P

Chapter 13.8, Problem 36P

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Fundamentals of Engineering Thermodynamics

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