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 atm T=400 K
e. PCl3 (g) + 3 H2 (g) --> PH3 (g) + 3 HCl (g) PPH3=2.50 atm PPCl3=1.50 atm PH2=0.250 atm PHCl=0.250 atm T=400 K
Compare your answer to parts a and b to your answer to parts c and d. Is the effect of the temperature change the same? If not, why would this happen
Homework Answers
Add Answer to:
5. Calculate deltaG under the following conditions.
a.C2H5OH (g) --> C2H4 (g) + H2O (g) Pressure...
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...
4. Using the information in the data table provided, a.Predict what physical state PCl3 is in...
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).
AH+ (kJ/mol) 30.71 Sº (1/K*mol) 245.3 AG+ (kJ/mol) 3.14 52.30 219.4 68.11 -235.1 282.7 - 168.5 0 222.96 0 0 202.7 0 130.58 0 Brz (g) CH. (g) C2H5OH (g) Cl2 (g) F2 (g) Hz (g) HBr (8)...
2. For the following example, identify the following. H2O(l) → H2O(s) question 2 options a negative...
2. For the following example, identify the following.
H2O(l) → H2O(s)
question 2 options
a negative ΔH and a negative ΔS
a positive ΔH and a negative ΔS
a negative ΔH and a positive ΔS
a positive ΔH and a positive ΔS
It is not possible to determine without more information.
3. Calculate ΔS°rxn for the following reaction. The S° for each
species is shown below the reaction.
C2H2(g) + H2(g) →
C2H4(g)
S°(J/mol∙K) 200.9 130.7 219.3
Question 4 options:...
Calculate Grxn at 298 K under the conditions shown below for the following reaction.
Calculate Grxn at 298 K under the conditions shown below for the following reaction. 2 H2S(g) + 3 O2(g) 2 SO2(g) + 2 H2O(g) G°rxn = ? G°f (kJ/mol) -33.4 -300.1 -228.6 P(H2S) = 1.4 atm, P(O2) = 0.5atm P(SO2) = 2.2atm and P(H2O) = 0.8 atm
For which of the following reactions is AS™ > 0. Choose all that apply 2NO(g) +...
For which of the following reactions is AS™ > 0. Choose all that apply 2NO(g) + 2H2(g) + N2(g) + 2H2O(1) H2(g) + C2H4(9) + CH (9) D NHI(s)+ NH4(g) + HI(g) 2002(g) + N2(g) 2CO(g) + 2NO(g) 4NH3(9) +502(9)→ 4NO(g) + 6H20(g) Submit Answer Retry Entire Group 3 more group attempts remaining Which of the following transformations represent an increase in the entropy of the system. Choose all that apply 44 g Ag (liquid, 1.234x10°K) 44 g Ag (solid,...
Calculate the standard-state entropy for the following reaction: 1 Al2O3(s) + 3 H2(g) ? 2 Al(s) + 3 H2O(l) (If applicab...
Calculate the standard-state entropy for the following reaction: 1 Al2O3(s) + 3 H2(g) ? 2 Al(s) + 3 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. S? J/(K?mol) Al(s) 28.0 H2O(l) 189 Al2O3(s) 51.0 H2(g) 131
Calculate the standard-state entropy for the following reaction: 1 Al2O3(s) + 3 H2(g) ⟶ 2 Al(s) + 3 H2O(l) (If applicab...
Calculate the standard-state entropy for the following reaction: 1 Al2O3(s) + 3 H2(g) ⟶ 2 Al(s) + 3 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) Al(s) 28.0 H2O(l) 189 Al2O3(s) 51.0 H2(g) 131
For which of the following reactions is AS° >0. Choose all that apply. NH4Cl(s) + NH3(g)...
For which of the following reactions is AS° >0. Choose all that apply. NH4Cl(s) + NH3(g) + HCl(g) 2C2H6(g) + 702(g) + 4CO2(g) + 6H2O(g) 2NH3(g) + 2O2(g) → N2O(g) + 3H2O(1) N2(g) + 202(g) + 2NO2(g) C2H2(g) + 4H2O(g) + 2CO2(g) + 5H2(g) Which of the following transformations represent an increase in the entropy of the system. Choose all that apply 20 g Hg (liquid, 244K) 20 g Hg (liquid, 620K) 1 mol CO2 (0.874 atm, 440K) 1 mol...
Use the data found in the Thermodynamic Values link under Reference Materials to calculate ΔHo (KJ),...
Use the data found in the Thermodynamic Values
link under Reference Materials to calculate
ΔHo (KJ), ΔSo (J/K) and
ΔGo(KJ) and ΔGo from the
equation ΔGo ≈ ΔHo - TΔSo
at 25.0 oC for
1. 1
C2H5OH(g) + ___ O2
(g) → ___ CO2 (g) + ___
H2O (g) (Do not change
a coefficient that is shown)
2. 2 C4H10 (l) + ___
O2 (g) → ___ CO2 (g) +
___ H2O (g) (Do not
change a coefficient that is shown)
3. C2H5OH
(l) → C2H4
(g) + H2O
(g) ...
Use the data found in the Thermodynamic Values link under Reference Materials to calculate ΔHo (KJ),...
Use the data found in the Thermodynamic Values
link under Reference Materials to calculate
ΔHo (KJ), ΔSo (J/K) and
ΔGo(KJ) and ΔGo from the
equation ΔGo ≈ ΔHo - TΔSo
at 25.0 oC for
1. C2H5OH
(g) → C2H4
(g) + H2O (l)
2. 2 C4H10
(l) + ___ O2 (g) → ___
CO2 (g) + ___ H2O
(l) (Do not change a coefficient
that is shown)
3. 2 C4H10 (g) + ___ O2
(g) → ___ CO2 (g) + ___
H2O (l) (Do not change
a coefficient that...
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...
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).
AH+ (kJ/mol) 30.71 Sº (1/K*mol) 245.3 AG+ (kJ/mol) 3.14 52.30 219.4 68.11 -235.1 282.7 - 168.5 0 222.96 0 0 202.7 0 130.58 0 Brz (g) CH. (g) C2H5OH (g) Cl2 (g) F2 (g) Hz (g) HBr (8)...
2. For the following example, identify the following.
H2O(l) → H2O(s)
question 2 options
a negative ΔH and a negative ΔS
a positive ΔH and a negative ΔS
a negative ΔH and a positive ΔS
a positive ΔH and a positive ΔS
It is not possible to determine without more information.
3. Calculate ΔS°rxn for the following reaction. The S° for each
species is shown below the reaction.
C2H2(g) + H2(g) →
C2H4(g)
S°(J/mol∙K) 200.9 130.7 219.3
Question 4 options:...
For which of the following reactions is AS™ > 0. Choose all that apply 2NO(g) + 2H2(g) + N2(g) + 2H2O(1) H2(g) + C2H4(9) + CH (9) D NHI(s)+ NH4(g) + HI(g) 2002(g) + N2(g) 2CO(g) + 2NO(g) 4NH3(9) +502(9)→ 4NO(g) + 6H20(g) Submit Answer Retry Entire Group 3 more group attempts remaining Which of the following transformations represent an increase in the entropy of the system. Choose all that apply 44 g Ag (liquid, 1.234x10°K) 44 g Ag (solid,...
For which of the following reactions is AS° >0. Choose all that apply. NH4Cl(s) + NH3(g) + HCl(g) 2C2H6(g) + 702(g) + 4CO2(g) + 6H2O(g) 2NH3(g) + 2O2(g) → N2O(g) + 3H2O(1) N2(g) + 202(g) + 2NO2(g) C2H2(g) + 4H2O(g) + 2CO2(g) + 5H2(g) Which of the following transformations represent an increase in the entropy of the system. Choose all that apply 20 g Hg (liquid, 244K) 20 g Hg (liquid, 620K) 1 mol CO2 (0.874 atm, 440K) 1 mol...
Use the data found in the Thermodynamic Values
link under Reference Materials to calculate
ΔHo (KJ), ΔSo (J/K) and
ΔGo(KJ) and ΔGo from the
equation ΔGo ≈ ΔHo - TΔSo
at 25.0 oC for
1. 1
C2H5OH(g) + ___ O2
(g) → ___ CO2 (g) + ___
H2O (g) (Do not change
a coefficient that is shown)
2. 2 C4H10 (l) + ___
O2 (g) → ___ CO2 (g) +
___ H2O (g) (Do not
change a coefficient that is shown)
3. C2H5OH
(l) → C2H4
(g) + H2O
(g) ...
Use the data found in the Thermodynamic Values
link under Reference Materials to calculate
ΔHo (KJ), ΔSo (J/K) and
ΔGo(KJ) and ΔGo from the
equation ΔGo ≈ ΔHo - TΔSo
at 25.0 oC for
1. C2H5OH
(g) → C2H4
(g) + H2O (l)
2. 2 C4H10
(l) + ___ O2 (g) → ___
CO2 (g) + ___ H2O
(l) (Do not change a coefficient
that is shown)
3. 2 C4H10 (g) + ___ O2
(g) → ___ CO2 (g) + ___
H2O (l) (Do not change
a coefficient that...
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