4. Using the information in the data table provided,
a.Predict what physical state PCl3 is in at 298 K.
b. Estimate the boiling point of PCl3. You may assume that deltaH and deltaS do not vary with temperature (usually a reasonable assumption).
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4. Using the information in the data table provided,
a.Predict what physical state PCl3 is in...
3. Calculate deltaS and deltaG and the equilibrium constant 298 K for each of these reactions,...
3. Calculate deltaS and deltaG and the equilibrium constant 298
K for each of these reactions, and indicate whether they are
spontaneous under standard conditionsa.
H2 (g) + F2 (g) --> 2HF (g)
b. C2H5OH (g) --> C2H4 (g) + H2O (g) (Calculate deltaH for
this one as well )
c.2HCl (g) + Br2 (g) → 2HBr(g) + Cl2 (g)
d. PCl3 (g) + 3 H2 (g) --> PH3 (g) + 3 HCl (g) (Calculate H
for this one as...
5. Calculate deltaG under the following conditions. a.C2H5OH (g) --> C2H4 (g) + H2O (g) Pressure...
5. Calculate deltaG under the following conditions.
a.C2H5OH (g) --> C2H4 (g) + H2O (g) Pressure of all
gasses=0.200 atm, T=200oC
b. C2H5OH (g) --> C2H4 (g) + H2O (g) Pressure of all
gasses=0.200 atm, T=400oC
c.PCl3 (g) + 3 H2 (g) --> PH3 (g) + 3 HCl (g) PPH3=3.00 atm
PPCl3=1.00 atm PH2=0.250 atm PHCl=0.250 atm T=298 K
d. PCl3 (g) + 3 H2 (g) --> PH3 (g) + 3 HCl (g) PPH3=3.00 atm
PPCl3=1.00 atm PH2=0.250 atm PHCl=0.250...
4. Only ideal processes can be thermodynamically "reversible." Why can rear proce y can real process...
4. Only ideal processes can be thermodynamically "reversible." Why can rear proce y can real processes not be? 5. Consider the following reactions. (Note: if this were an exam we would give you an excerpt on tabular data from Appendix 4 (Table A4.3). 2Fe(s) + 3Cla(s) 2FeCl(s) N2H4(8) + H2(g) + 2NH3(g) (a) Would you expect the entropy change for the above reaction to be >0, <0, or no (small)? Justify your answer. (d) Would you expect the entropy change...
3. Calculate deltaS and deltaG and the equilibrium constant 298
K for each of these reactions, and indicate whether they are
spontaneous under standard conditionsa.
H2 (g) + F2 (g) --> 2HF (g)
b. C2H5OH (g) --> C2H4 (g) + H2O (g) (Calculate deltaH for
this one as well )
c.2HCl (g) + Br2 (g) → 2HBr(g) + Cl2 (g)
d. PCl3 (g) + 3 H2 (g) --> PH3 (g) + 3 HCl (g) (Calculate H
for this one as...
5. Calculate deltaG under the following conditions.
a.C2H5OH (g) --> C2H4 (g) + H2O (g) Pressure of all
gasses=0.200 atm, T=200oC
b. C2H5OH (g) --> C2H4 (g) + H2O (g) Pressure of all
gasses=0.200 atm, T=400oC
c.PCl3 (g) + 3 H2 (g) --> PH3 (g) + 3 HCl (g) PPH3=3.00 atm
PPCl3=1.00 atm PH2=0.250 atm PHCl=0.250 atm T=298 K
d. PCl3 (g) + 3 H2 (g) --> PH3 (g) + 3 HCl (g) PPH3=3.00 atm
PPCl3=1.00 atm PH2=0.250 atm PHCl=0.250...
4. Only ideal processes can be thermodynamically "reversible." Why can rear proce y can real processes not be? 5. Consider the following reactions. (Note: if this were an exam we would give you an excerpt on tabular data from Appendix 4 (Table A4.3). 2Fe(s) + 3Cla(s) 2FeCl(s) N2H4(8) + H2(g) + 2NH3(g) (a) Would you expect the entropy change for the above reaction to be >0, <0, or no (small)? Justify your answer. (d) Would you expect the entropy change...
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