Hw 8.67 part b

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Virpal Gill 1B
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Hw 8.67 part b

Postby Virpal Gill 1B » Wed Jan 17, 2018 3:02 pm

This question states to find the enthalpy of formation of CH3OH. I understand where the values for the bond enthalpies came from but in the solutions manual it states that the energy needed to "atomize 1 mol C(gr)" is 717 kJ/mol. Is this something we are meant to know? If so, how is that value calculated?
Last edited by Virpal Gill 1B on Wed Jan 17, 2018 3:17 pm, edited 1 time in total.

Sammy Thatipelli 1B
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Re: Hw 8.67 part b

Postby Sammy Thatipelli 1B » Wed Jan 17, 2018 3:09 pm

This number comes from the fact that standard heat of atomization is the amount of heat energy required to produce one mole of gaseous atoms from the element in its standard state. because it is a single carbon and not part of the bond, we use the value for atomizing Carbon, which is a set value given as 717 kJ/mol

Jennie Fox 1D
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Re: Hw 8.67 part b

Postby Jennie Fox 1D » Wed Jan 17, 2018 5:45 pm

717 kJ/mol would have to be given. It can be found in the appendix at the end of the book.

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