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The heat of combustion of acetylene, C2H2, is -1255.5kj/mol. When 0.187g of acetylene (molecular weight 26.03)...

The heat of combustion of acetylene, C2H2, is -1255.5kj/mol. When 0.187g of acetylene (molecular weight 26.03) is burned with excess oxygen in a bomb calorimeter which has a total heat capacity of 1045J/C and an initial temperature of 21.36C, what will be the final temperature of the calorimeter plus contents? equation: C2H2+5/2 O2(g)--2CO2(g)+H2O(L)

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Answer #1

Mass of acetylene = 0.187g

Molar mass of acetylene = 26.03g/mol

No of mole of acetylene burned = 0.187g/26.03g/mol = 0.007184mol

Heat released = 0.007184mol × 1255.5kJ/mol =9.0195kJ= 9019.5J

Heat capacity of calorimeter = 1045J/℃

q = ∆T × C

= (Final temperature - Initial temperature) × C

9019.5J = (Final temperature - 21.36℃ ) ×1045J/℃

= Final temperature ×1045J/℃ - 22321J

Final temperature ×1045J/℃ = 9019.5J + 22321J

Final temperature = 13341J/1045(J/℃)

= 29.99℃

  

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