Ask a New Question

Question

The standard molar heat of fusion of ice is 6020 J/mol. Calculate q, w, and (delta) E for melting 1.00 mol of ice at 0 deg. C and 1.00 atm pressure.
13 years ago

Answers

DrBob222
E = q+w
q = 6020 J/mol x 1 mol = ?
w = -pdV.
p is 101.325
Look up te density of ice and calculate the volume of a mol at zero C. Then calculate the volume of a mol of water at zero C. The differecne is dV. I found densities ice/H2O here.
http://en.wikipedia.org/wiki/Ice
13 years ago

Related Questions

1.What is the molar heat of vaporization of water, given the following thermochemical equations?... The standard molar enthalpy of fusion and the standard molar enthalpy of vaporization of benzene are... The standard molar heat of vaporiza- tion for water is 40.79 kJ/mol. How much energy would be requ... the standard molar enthalpy and entropy of the denaturation of a certain protein are 512 kj/mol and... calculate the standard molar entropy change for the combustion of methane gas using S naught values... Given the standard molar entropies measured at 25 C and 1 ATM pressure calculate delta S for the rea... The standard molar heat of vaporization for water is 40.79 kJ/mol. How much energy would be requir... What is the latent heat of fusion of ice to water? Help pls!!!!! What is the molar heat of the formation of sodium aside? Determine the standard molar enthalpy of combustion of octane using Hess's law
Ask a New Question
Archives Contact Us Privacy Policy Terms of Use