The enthalpy of reaction for the formation of 2.00-mol ozone from 3.00-mol O2 (g): 3 O2 (g) à 2 O3 (g) is ∆Horxn = 429 kJ at 1 atm and 25 oC. In this question, O2 (g) and O3(g) are rigid molecules and have the ideal gas behavior. Their molar heat capacities at constant pressure are independent of temperature, and follow the values shown in our lecture note (Page 56 in Chapter 2 Part 1). At -35 oC, the enthalpy of reaction for the above reaction ( 3 O2 (g) à 2 O3 (g) ) should be _______ 429 kJ. Insufficient information equal to greater than less than
The enthalpy of reaction for the formation of 2.00-mol ozone from 3.00-mol O2 (g): 3 O2 (g) à 2 O3 (g) is ∆Horxn = 429 kJ at 1 atm and 25 oC. In this question, O2 (g) and O3(g) are rigid molecules and have the ideal gas behavior. Their molar heat capacities at constant pressure are independent of temperature, and follow the values shown in our lecture note (Page 56 in Chapter 2 Part 1). At -35 oC, the enthalpy of reaction for the above reaction ( 3 O2 (g) à 2 O3 (g) ) should be _______ 429 kJ.
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The reaction given is
=> 3 O2 (g) ------> 2 O3 (g) ∆Horxn = 429 kJ at 25oC
Using appendix : The molar heat capacity of O2, CO2 = 29.38 J⋅mol−1⋅K−1
And the molar heat capacity of O3 CO3 = 40 J⋅mol−1⋅K−1
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