Part A Refer to the tabulated values of ΔG∘f in Appendix IVB in
the textbook to...
Part A Refer to the tabulated values of ΔG∘f in Appendix IVB in
the textbook to calculate E∘cell for the fuel cell, which employs
the following reaction. CH3CH2OH(g)+O2(g)→HC2H3O2(g)+H2O(g) (ΔG∘f
for HC2H3O2(g) = -374.2 kJ/mol.)
Using the data in Appendix C in the textbook and given the
pressures listed, calculate ΔG for each of the following
reactions at 298 K.
Part A) N2(g)+3H2(g)→2NH3(g)
Part B) N2(g)+3H2(g)→2NH3(g)
PN2 = 2.5 atm , PH2 = 7.2 atm , PNH3 =
1.7 atm
Part C)
2N2H4(g)+2NO2(g)→3N2(g)+4H2O(g)
Part D)
2N2H4(g)+2NO2(g)→3N2(g)+4H2O(g)
PN2H4=PNO2=1.0×10−2atm, PN2 = 2.0 atm ,
PH2O = 1 atm
Part E) N2H4(g)→N2(g)+2H2(g)
Part F) N2H4(g)→N2(g)+2H2(g)
PN2H4 = 0.6 atm , PN2 = 7.2 atm , PH2 =
9.1...
Using S? values from Appendix C in the textbook, calculate ?S?
values for the following reactions. 5 significant figures
please!!!
C2H4(g)+H2(g)?C2H6(g)
N2O4(g)?2NO2(g)
Be(OH)2(s)?BeO(s)+H2O(g)
2CH3OH(g)+3O2(g)?2CO2(g)+4H2O(g)
Using the thermo. values listed in Appendix B (pg. A 5-7) of your textbook
CO(g): deltaH:-110.5(kJ/mol) deltaG:-137.2(kJ/mol) deltaS:197.5(J/mol*K)
CO2(g): deltaH: -393.5(kJ/mol). deltaG: -394.4(kJ/mol) deltaS: 213.7(J/mol*K)
CO2(aq) deltaH:-412.9(kJ/mol) deltaG: -386.2(kJ/mol) deltaS:121
H2(g): deltaH:0. delta G: 0. delta S:130.6
(a) Calculate deltaS°, deltaH° & deltaG° for the vaporization of methanol, CH3OH:
(b) Is this phase transition spontaneous at room temperature (show your work) ?
(c) If the phase transition is not spontaneous at room temperature, at what higher temperature will it...
Computing Present Values of Single Amounts and
Annuities
Refer to Tables 1 and 2 in Appendix A near the end of the book to
compute the present value for each of the following amounts.
Round answers to the nearest dollar.
a. $160,000 received 10 years hence if the annual interest rate
is:
1. 10% compounded annually.
$Answer
2. 10% compounded semiannually.
$Answer
b. $6,000 received at the end of each year for the next eight
years discounted at 8% compounded...
Using values from Appendix C of your textbook, calculate the
value of Ho, So, and Go for each of the following reactions at
standard temperature (298 K). Next calculate G if ALL of the GASSES
in the reaction have partial pressures of 0.2 atm.
(a) NaOH(s) + CO2(g) NaHCO3(s) Ho = -127.44 kJ/mol
So = -176.02 J/mol-K
Go = -74.96 kJ/mol
If all gasses have partial pressures of 0.2 atm then G =
________ kJ/mol.
(b) 2 Fe(s) + 3...
Use ?G?f values from Appendix IIB to calculate the
equilibrium constants at 25 ?C for each of the following
reactions.
a. 2NO2(g)?N2O4(g)
b. 3/2H2(g)+1/4P4(g)?PH3(g)
Use tabulated half-cell potentials to calculate ΔG∘rxn for each
of the following reactions at 25 ∘C.
Part A 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq)
Express the energy change in kilojoules to two significant
figures.
Part B O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq)
Express the energy change in kilojoules to one significant
figure.
Part C Br2(l)+2I−(aq)→2Br−(aq)+I2(s) Express
the energy change in kilojoules to two significant figures.
For the reaction CuS(s) + H2(g) H2S(g) + Cu(s) ΔG°f (CuS) =
−53.6 kJ/mol ΔG°f (H2S) = −33.6 kJ/mol ΔH°f (CuS) = −53.1 kJ/mol
ΔH°f (H2S) = − 20.6 kJ/mol a. Calculate ΔG° and ΔH° at 298 K and 1
atm pressure. b. Will this reaction proceed spontaneously at 298 K
and 1 atm pressure? c. Calculate the equilibrium constant for this
reaction at 298 K. d. Calculate ΔS° at 298 K and 1 atm pressure. e.
Calculate ΔG at...
Use data from Appendix C to calculate the equilibrium constant,
K, and ΔG∘ at 298 K for each of the following
reactions.
H2(g)+I2(g)⇌2HI(g)
Calculate ΔG∘.
Express your answer to four significant figures and include the
appropriate units.
Part A
H2(g)+I2(g)⇌2HI(g)
Calculate ΔG∘.
Express your answer to four significant figures and include the
appropriate units.
Part B
Calculate the equilibrium constant, K.
Express your answer using two significant figures.
Part C
C2H5OH(g)⇌C2H4(g)+H2O(g)
Calculate ΔG∘.
Express your answer to two significant figures...