For tin, Sn, the heat of vaporization at its normal boiling point of 2270 °C is

Chemistry
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For tinSn, the heat of vaporization at its normal boiling point of 2270 °C is 230.1kJ/mol.


The entropy change when 2.01 moles of liquid Sn vaporizes at 2270 °C, 1 atm is  J/K.
Jun 2nd, 2015

Please let me know if you need any clarification. I'm always happy to answer your questions.

Q=T(delta s)

heat of vaporization for 1 mol=230kj

so heat of vaporization for 1 mol=230*2=460KJ

460*10^3 J=(2270+273)delta S

delta S=460*10^3/(2270+273)

delta S=180.89 J/K

so entropy change 180.89 J/K


hope you happy with my answer please don't forget to rate me and leave a review.if you have any question  let me know i'll choose the best answer for you.thank you.see you soon again...:)

Please let me know if you need any clarification. I'm always happy to answer your questions.
Jun 2nd, 2015

Correct! can u answer this one too please? 

For copperCu, the heat of fusion at its normal melting point of 1083 °C is 13.0kJ/mol.

The entropy change when 2.34 moles of solid Cu melts at 1083 °C, 1 atm is  J/K.

Jun 2nd, 2015

sure wait for while


Jun 2nd, 2015

okay

Jun 2nd, 2015

Q=T(delta s)

Q=13*2.34 KJ

so

13*2.34*10^3 J=(1083+273)(delta s)

(delta s)=13*2.34*10^3 J/(1083+273)

(delta s)=22.4 J/K

Jun 2nd, 2015

Thanks!! i really need you outside of this 

Jun 2nd, 2015

you are always welcome!

Jun 2nd, 2015

could i ask you some more?

Jun 2nd, 2015

ya why not...........

Jun 2nd, 2015

okay! 

Fe3O4(s) + 4H2(g)3Fe(s) + 4H2O(g)

Using standard thermodynamic data at 298K, calculate the entropy change for thesurroundings when 1.89 moles of Fe3O4(s) react at standard conditions.
surroundings =  J/K


2SO2(g) + O2(g)2SO3(g)

Using standard thermodynamic data at 298K, calculate the entropy change for thesurroundings when 2.15 moles of SO2(g) react at standard conditions.
   surroundings =  J/K

Jun 2nd, 2015

you can use same equation for this questions also

Q=TS

1.89*delta H=298*s

s=1.89*delta H/298


to find delta H you have to find the enthalpy change of the reaction.to do that you have to use standard thermodynamic data from book.at this time i'm unable to find that data.so find delta H and substitute it to equation..


2nd question also can be solved as same procedure...

Jun 3rd, 2015

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