stuck on a thermo-dtnamics lab... please help.... Molar solubility of CuCl in Mo
ID: 901557 • Letter: S
Question
stuck on a thermo-dtnamics lab... please help....
Molar solubility of CuCl in Mol at 25 deg C =
Cu+ = 4.276x10^-4
Cl- = 4.276x10^-4
balanced equation = CuCl (s) <-----> Cu+(aq) + Cl-(aq)
equilibrium expression is Ksp= [Cu+][Cl-]... Ksp = 1.82x10^-7
Molar solubility of CuCl in mol at 100 deg C =
Cu+ = 2.320x10^-3
Cl-= 2.320x10^-3
equilibrium expression is Ksp = [Cu+][Cl-] = 5.38x10^-6
so i need help with the following...
1. calculate delta G of the reaction using Ksp, in kJ/mol at 25 deg C.
2. utilizing new Ksp (100 deg C)(5.38x10^-6), calculate value of standard free energy of the rxn at 100 deg C.
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additionally...
MnO2(s) + 2 CO (g) -----> Mn(s) + 2 CO2(g)
MnO2 (s) = delta H = -520.9, delta G = -466.1, s = 53.1
CO (g) = delta H = -110.5, delta G = -137.2, s = 197.5
Mn (s) = delta H = 0, delta G = 0, s=31.8
CO2 (g) = delta H = -393.5, delta G = -394.4, s = 213.7
1. calculate delta G at 25 deg C
2. calculate delta G at 125 deg C
3. why wont delta G tables work for number 2
4. Calculate K at 298 K for the reaction
5. Calculate delta G at 298K if MnO2 = 0.150 mol, Mn = 0.850 mol, CO = .250 mol, and Co2 = 0.500 M in a 1.25 L flask.
please show with work and units, as to help me understand for the upcoming actual lab in class tomorrow... thank you in advance... I really appreciate it. I apologise for many questions in one post, but Chegg limits and my lack of a credit card (high school) limit my abilities to post questions.
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stuck on a thermo-dtnamics lab... please help.... Molar solubility of CuCl in Mo
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