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.
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...
Adam tabulated the values for the average speeds on each day of
his road trip as 60.5, 63.2, 54.7, 51.6, 72.3, 70.7, 67.2, and 65.4
mph he wishes to construct a 98% confidence interval what value of
t* should Adam use to construct the confidence interval?