Question

Calculate the change in Gibbs free energy for each of the following sets of ?H?rxn, ?S?rxn, and T.

Part A ?H?rxn=? 115 kJ ; ?S?rxn= 248 J/K ; T= 295 K

Part B ?H?rxn= 115 kJ ; ?S?rxn=? 248 J/K ; T= 295 K

Part C ?H?rxn=? 115 kJ ; ?S?rxn=? 248 J/K ; T= 295 K Express your answer using two significant figures.

Part D ?H?rxn=? 115 kJ ; ?S?rxn=? 248 J/K ; T= 565 K Express your answer using two significant figures.

Part E Predict whether or not the reaction in part A will be spontaneous at the temperature indicated.

Part F Predict whether or not the reaction in part B will be spontaneous at the temperature indicated.

Part G Predict whether or not the reaction in part C will be spontaneous at the temperature indicated.

Part H Predict whether or not the reaction in part D will be spontaneous at the temperature indicated.

Answer #1

1. A.

= -115*10^3 - 295*248

= -188160 joules Or -188.160 KJ

E. is negative so the reaction is spontaneous.

B. 115*10^3 -295*(-248)

= 188160 Joules or 188.160 KJ

F. As is positive in reaction B so it is not a spontaneous reaction.

C. -115*10^3 - 295*(-248)

= -41840 Joules or -41.840 KJ

G. As is negative so reaction C is not spontaneous.

D. -115*10^3 - 565*(-248)

= -25120 Joules or -25.120 KJ

H. is negative in D so the reaction is spontaneous.

if satisfied please rate it thanks.

Calculate the change in Gibbs free energy for each of the
following sets of ΔHrxn, ΔSrxn, and
T.
Part A
ΔH∘rxn= 90. kJ , ΔSrxn= 152 J/K , T=
303 K
Express your answer using two significant figures.
ΔG =
kJ
Part B
ΔH∘rxn= 90. kJ , ΔSrxn= 152 J/K , T=
750 K
Express your answer using two significant figures.
ΔG =
kJ
Part C
ΔH∘rxn= 90. kJ , ΔSrxn=− 152 J/K , T=
303 K
Express your answer...

Calculate the change in Gibbs free energy for each of the
following sets of ΔHrxn ∘, ΔS∘rxn, and
T.
1) ΔH∘rxn=− 97 kJ , ΔS∘rxn=− 154 J/K ,
T= 310 K
Express your answer using two significant figures.
2) ΔH∘rxn=− 97 kJ , ΔS∘rxn=− 154 J/K ,
T= 856 K
3) ΔH∘rxn= 97 kJ , ΔS∘rxn=− 154 J/K ,
T= 310 K
4) ΔH∘rxn=− 97 kJ , ΔS∘rxn= 154 J/K ,
T= 408 K

1)
Calculate the amount of energy in kilojoules needed to change
207 g of water ice at −10 ∘C to steam at 125 ∘C. The following
constants may be useful:
Cm (ice)=36.57 J/(mol⋅∘C)
Cm (water)=75.40 J/(mol⋅∘C)
Cm (steam)=36.04 J/(mol⋅∘C)
ΔHfus=+6.01 kJ/mol
ΔHvap=+40.67 kJ/mol
Express your answer with the appropriate units.
2) Given the values of ΔH∘rxn, ΔS∘rxn, and
T below, determine ΔSuniv.
Part A
ΔH∘rxn= 90 kJ , ΔSrxn= 144 J/K , T=
304 K
Express your answer using two...

Given the values of ΔH∘rxn, ΔS∘rxn, and
T below, determine ΔSuniv.
Part A
ΔH∘rxn= 115 kJ , ΔS∘rxn=− 263 J/K ,
T= 301 K .
ΔSuniv=
J/K
SubmitMy AnswersGive
Up
Part B
ΔH∘rxn=− 115 kJ , ΔS∘rxn= 263 J/K ,
T= 301 K .
ΔSuniv=
J/K
SubmitMy AnswersGive
Up
Part C
ΔH∘rxn=− 115 kJ , ΔS∘rxn=− 263 J/K ,
T= 301 K .
ΔSuniv=
J/K
SubmitMy AnswersGive
Up
Part D
ΔH∘rxn=− 115 kJ , ΔS∘rxn=− 263 J/K ,
T= 557...

Given the values of ΔH∘rxn, ΔS∘rxn, and
T below, determine ΔSuniv.
Part A
ΔH∘rxn= 117 kJ , ΔS∘rxn=− 263 J/K ,
T= 291 K .
ΔSuniv=
−1.3•102
J/K
SubmitMy AnswersGive
Up
Incorrect; Try Again; 3 attempts remaining
Part B
ΔH∘rxn=− 117 kJ , ΔS∘rxn= 263 J/K ,
T= 291 K .
ΔSuniv=
J/K
SubmitMy AnswersGive
Up
Part C
ΔH∘rxn=− 117 kJ , ΔS∘rxn=− 263 J/K ,
T= 291 K.
ΔSuniv=
J/K
SubmitMy AnswersGive
Up
Part D
ΔH∘rxn=− 117 kJ ,...

Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine
ΔSuniv.
Part A
ΔH∘rxn=− 89 kJ , ΔSrxn=− 150 J/K , T= 310 K
Express your answer using two significant figures.
Part B
ΔH∘rxn=− 89 kJ , ΔSrxn=− 150 J/K , T=
758 K
Express your answer using one significant figure.
Part C
ΔH∘rxn=+ 89 kJ , ΔSrxn=− 150 J/K , T=
310 K
Express your answer using two significant figures.
Part D
ΔH∘rxn=− 89 kJ , ΔSrxn=+ 150 J/K...

A. Using given data, calculate the change in
Gibbs free energy for each of the following reactions. In each case
indicate whether the reaction is spontaneous at 298K under standard
conditions.
2H2O2(l)→2H2O(l)+O2(g)
Gibbs free energy for H2O2(l) is -120.4kJ/mol
Gibbs free energy for H2O(l) is -237.13kJ/mol
B. A certain reaction has ΔH∘ = + 35.4
kJ and ΔS∘ = 85.0 J/K . Calculate ΔG∘ for the
reaction at 298 K. Is the reaction spontaneous at
298K under standard
conditions?

Given the following information,
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State if the reaction is spontaneous or nonspontaneous followed by
the temperature at which the reaction switches spontaneity if
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CaCO3(s) --> CaO(s) + CO2(g)
Given: Δ°H = 179.2 kJ , Δ°S = 160.2 J/K

Using a Table of thermodynamic data, calculate the change in
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kJ/mol, FeO (s) = -255.2 kJ/mol, FeCl3 (s) = -334 kJ/mol, H3PO4
(aq) = -1142.6 kJ/mol
(a) 2 Fe(s) + O2(g)--->2 FeO(s) kJ
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Gxrn= ___ kJ
Express your answer using two significant figures
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E*cell=____ V
Express your answer using two significant figures.

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