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Consider the reaction: 12(g) + Cl2(g)—>21CI(g) Using standard thermodynamic data at 298K, calculate the free energy...
Consider the reaction: 12(g) + Cl2(g)—>21CI(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.950 moles of L2(g) react at standard conditions. AGºrxn = kJ Iodine AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 12(s) 0 0 116.1 12(9) 62.4 19.3 260.7 23.0 16.0 137 12(aq) I(g) 106.8 70.3 180.8 1 (9) -197.0 -55.0 -52.0 106.0 I'(aq) ICI(9) 17.8 -5.5 247.6 Chlorine Cl(9) AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) 121.7 105.7 165.2 0 0 223.1 -23.0...
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...
help with these please N2(g) + O2(g) 2NO(g) Using the standard thermodynamic data in the tables...
help with these please
N2(g) + O2(g) 2NO(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: CH (9) +202(g) →CO2(g) + 2H2O(g) de manera en cas de este mai mare de mise en contact tenda Using standard thermodynamic data at 298K, calculate the free energy change when 1.62 moles of CH4(g) react at standard conditions. AGºrx Nz9) +202(g) +2NO2(g) Using standard thermodynamic data at 298K, calculate the free...
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) ...
help with this please Ca(OH)2(aq) + 2 HCl(aq) +CaCl2(8) + 2 H2O(1) Using the standard thermodynamic...
help with this please
Ca(OH)2(aq) + 2 HCl(aq) +CaCl2(8) + 2 H2O(1) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: N2(g) + O2(g) +2NO(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: 2CO(g) + O2(g) +2002(9) - der e en manos de 20, ali ne more than one so mi dicogna undan Using standard thermodynamic data...
I know that this is the answer, but how do I cancel out equations to reach...
I know that this is the answer, but how do I cancel
out equations to reach it ?
Calculate the enthalpy change to be expected for the dissolution of NaOH ((s) and (aq) mean solid and aqueous) using Hess's Law: NaOH(s) NaOH(aq) Use the enthalpy change for NaOH-HCI pair that your class measured in this experiment, and the data from the following table: Reaction* AH(kJ/mol %H2(g) + 2Cl2(g) → HCl(g) - 92.31 Na(s) + 1202(g) + 12H2(g) → NaOH(s) -...
Thermodynamic properties of pure substances Standard thermodynamic quantities for selected substances at 25 ° C listed...
Thermodynamic properties of pure
substances
Standard thermodynamic quantities for selected substances at 25
°
C listed alphabetically by most important atom.
substance
Δ
Hf
°
(kJ/mol)
Δ
Gf
°
(kJ/mol)
S
°
(J/mol∙K)
Aluminum
Al3+ (aq)
---
-485.0
---
Al (s)
0
0
28.3
Al2O3 (s)
-1675.7
-1582.3
50.9
Al(OH)3 (s)
---
-1147.25
---
Bromine
Br− (aq)
---
-104.0
---
Br2 (l)
0
0
152.2
Br2 (g)
30.9
3.1
245.5
HBr (g)
-36.3
-53.4
198.7
Calcium
Ca2+ (aq)
---
-553.6...
ALEKS Chemistry O ENTROPY AND FREE ENERGY Calculating reaction free energy under nonstandard conditions A chemist...
ALEKS Chemistry O ENTROPY AND FREE ENERGY Calculating reaction free energy under nonstandard conditions A chemist fills a reaction vessel with 0.546 atm nitrogen monoxide (NO) gas, 1.48 atm chlorine (CI) gas, and 4.56 atm nitrosyl chloride (NOCI) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: 2NO(g) +C12(e) - 2NOCI(8) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. х 5...
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs...
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. 6 Cl(g)+2 Fe,O,(s)4 FeCl, (s)+30,(g) kJ/mol AGn= Thermodynamic Properties at 298 K Organic Compounds AG kJ/mol /(mol-K) дне kJ/mol Substance Name Formula дне kJ/mol Ag(s) Ag (aq) Ag20(s) Ag2S(s) AgBr(s) AgC(s) Agl(s) AgNO3(s) Al(s) Al2O3(s) AICI3(s) 0 42.6 105.8 77.107 73.4 Methane CH4(9) СHа(о) -74.6) -84.0 -103.8 -11.2 -31.1 121.3 Ethane -32.6 -40.7...
help with the following combustion reaction. shown are the tables and answer. I am confused with...
help with the following combustion reaction. shown are the
tables and answer. I am confused with the steps to get there.
2. (a) For ethanol, CH3CH2OH, AfHº = -277.7 kJ/mol at 25 °C. Using other AfHº values from Appendix A (Table 4.1) of your text, determine the enthalpy (heat) of combustion of liquid ethanol. (b) Determine the temperature change expected when 2.07 g of ethanol are burned in a bomb calorimeter whose heat capacity (as previously measured) is 9007 J/K...
Consider the reaction: 12(g) + Cl2(g)—>21CI(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.950 moles of L2(g) react at standard conditions. AGºrxn = kJ Iodine AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 12(s) 0 0 116.1 12(9) 62.4 19.3 260.7 23.0 16.0 137 12(aq) I(g) 106.8 70.3 180.8 1 (9) -197.0 -55.0 -52.0 106.0 I'(aq) ICI(9) 17.8 -5.5 247.6 Chlorine Cl(9) AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) 121.7 105.7 165.2 0 0 223.1 -23.0...
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...
help with these please
N2(g) + O2(g) 2NO(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: CH (9) +202(g) →CO2(g) + 2H2O(g) de manera en cas de este mai mare de mise en contact tenda Using standard thermodynamic data at 298K, calculate the free energy change when 1.62 moles of CH4(g) react at standard conditions. AGºrx Nz9) +202(g) +2NO2(g) Using standard thermodynamic data at 298K, calculate the free...
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) ...
help with this please
Ca(OH)2(aq) + 2 HCl(aq) +CaCl2(8) + 2 H2O(1) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: N2(g) + O2(g) +2NO(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: 2CO(g) + O2(g) +2002(9) - der e en manos de 20, ali ne more than one so mi dicogna undan Using standard thermodynamic data...
I know that this is the answer, but how do I cancel
out equations to reach it ?
Calculate the enthalpy change to be expected for the dissolution of NaOH ((s) and (aq) mean solid and aqueous) using Hess's Law: NaOH(s) NaOH(aq) Use the enthalpy change for NaOH-HCI pair that your class measured in this experiment, and the data from the following table: Reaction* AH(kJ/mol %H2(g) + 2Cl2(g) → HCl(g) - 92.31 Na(s) + 1202(g) + 12H2(g) → NaOH(s) -...
Thermodynamic properties of pure
substances
Standard thermodynamic quantities for selected substances at 25
°
C listed alphabetically by most important atom.
substance
Δ
Hf
°
(kJ/mol)
Δ
Gf
°
(kJ/mol)
S
°
(J/mol∙K)
Aluminum
Al3+ (aq)
---
-485.0
---
Al (s)
0
0
28.3
Al2O3 (s)
-1675.7
-1582.3
50.9
Al(OH)3 (s)
---
-1147.25
---
Bromine
Br− (aq)
---
-104.0
---
Br2 (l)
0
0
152.2
Br2 (g)
30.9
3.1
245.5
HBr (g)
-36.3
-53.4
198.7
Calcium
Ca2+ (aq)
---
-553.6...
ALEKS Chemistry O ENTROPY AND FREE ENERGY Calculating reaction free energy under nonstandard conditions A chemist fills a reaction vessel with 0.546 atm nitrogen monoxide (NO) gas, 1.48 atm chlorine (CI) gas, and 4.56 atm nitrosyl chloride (NOCI) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: 2NO(g) +C12(e) - 2NOCI(8) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. х 5...
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. 6 Cl(g)+2 Fe,O,(s)4 FeCl, (s)+30,(g) kJ/mol AGn= Thermodynamic Properties at 298 K Organic Compounds AG kJ/mol /(mol-K) дне kJ/mol Substance Name Formula дне kJ/mol Ag(s) Ag (aq) Ag20(s) Ag2S(s) AgBr(s) AgC(s) Agl(s) AgNO3(s) Al(s) Al2O3(s) AICI3(s) 0 42.6 105.8 77.107 73.4 Methane CH4(9) СHа(о) -74.6) -84.0 -103.8 -11.2 -31.1 121.3 Ethane -32.6 -40.7...
help with the following combustion reaction. shown are the
tables and answer. I am confused with the steps to get there.
2. (a) For ethanol, CH3CH2OH, AfHº = -277.7 kJ/mol at 25 °C. Using other AfHº values from Appendix A (Table 4.1) of your text, determine the enthalpy (heat) of combustion of liquid ethanol. (b) Determine the temperature change expected when 2.07 g of ethanol are burned in a bomb calorimeter whose heat capacity (as previously measured) is 9007 J/K...
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