Using standard thermodynamic data from Appendix D, calculate the equilibrium constant at 307 K for the...
Using standard thermodynamic data from Appendix D, calculate the equilibrium constant at 307 K for the following chemical equilibrium:
FeO(s) + CO(g) ⇄Fe(s) + CO2(g)
Homework Answers
FeO(s) + CO(g) ⇄Fe(s) + CO2(g)
G0rxn
=
G0f products -
G0f reactants
= -394.359 + 0 -(-251.46 -137.168)
= -5.731Kj/mole
= -5731J/mole
G0rxn
= -RTlnK
-5731 = -8.314*307lnK
lnK = -5731/(-8.314*307)
lnK = 2.2453
K = 9.443 >>>>>answer
Add Answer to:
Using standard thermodynamic data from Appendix D, calculate the
equilibrium constant at 307 K for the...
Using standard thermodynamic data from Appendix D, calculate the equilibrium constant at 311 K for the...
Using standard thermodynamic data from Appendix D, calculate the equilibrium constant at 311 K for the following chemical equilibrium: CO2(g) + 4H2(g) 2CH(0) + 2H20 (1) 1.16E19 The number of significant digits is set to 3; the tolerance is +/-2% Click if you would like to Show Work for this question: Open Show Work
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate...
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. H2(g) + Cl2(g)—>2HCI(g) K=
Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction....
Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. HCl(g) + NH3(g)--->NH4Cl(s) K =
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate...
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. N2(g) + 3H2(9) 2NH3(g)
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate...
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction 2502(g) + O2(0) 2503(9) AH°F (kJ/mol) AGⓇ, (kJ/mol sº (/mol K) 205.1 Oxygen 02(0) (9) O3(9) 249.2 231.7 161.1 142.7 163.2 238.9 AH°: (kJ/mol Agºr (kJ/mol) 5° (J/mol K) 31.8 0.3 0.3 278.8 3 3.0 167.8 33.0 - 15.0 Sulfur S(s, rhombic) S(s, monodinic) S(g) Sz"(aq) Sg(9) SzCl2(g) SF6(9) H2S(9) soz(9) SO3(0) 1 0....
Using data from Appendix C in the textbook, write the equilibrium-constant expression and calculate the value...
Using data from Appendix C in the textbook, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions at 298 K . A) NaHCO3(s) ⇌ NaOH(s)+CO2(g) What is the free-energy change for this reaction at 298 K? Express the free energy in kilojoules to one decimal place. B) 2HBr(g)+Cl2(g) ⇌ 2HCl(g)+Br2(g) Which is the equilibrium-constant expression for this reaction? K=P2HClPBr2P2HBrPCl2 K=P2HBrPCl2 K=P2HBrPCl2P2HClPBr2 K=PHClPBr2PHBrPCl2 C) 2SO2(g)+O2(g) ⇌ 2SO3(g) Which is the equilibrium-constant...
7 and 8 7. Using the Thermodynamic Data from Appendix 3 in your text book, calculate...
7 and 8
7. Using the Thermodynamic Data from Appendix 3 in your text book, calculate the standard reaction entropy of the following chemical reaction: N2 (g) + O2(g) 2 NO (g) 8. Using the Thermodynamic Data from Appendix 3 in your text book, calculate the standard reaction entropy of the following chemical reaction: Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H20 (1) 9. The standard reaction free energy AGº = -64.0 kJ for this...
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 641...
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 641 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ /kJ mol-1 -314.4 -45.9 -92.3 Smº /JK-mol-1 94.6 192.8 186.9 Cp.m /JK-mol-1 84.1 35.1 29.1 Do not use the Van't Hoff equation, In(K/K) = -(AHR/R) (T2-1-T1-1) The value of the thermodynamic equilibrium constant is Kp = Number
Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K...
Using any data you can find in the ALEKS Data resource,
calculate the equilibrium constant
K at 25.0°C for the following reaction.
6Cl2(g) + 2Fe2O3(s)
→ 4FeCl3(s)+ 3O2(g)
Round your answer to 2 significant digits.
O ENTROPY AND FREE ENERGY Using thermodynamic data to calculate K Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. 6 C12(g) + 2 Fe2O3(s) — 4 FeCl3(s) + 302(8) Round your answer to...
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 839...
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 839 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ 7 kJ mol-1 -314.4 -45.9 -92.3 Smº JK-1 mol-1 94.6 192.8 186.9 Cp,m 84.1 35.1 29.1 /JK-1 mol-1 Do not use the Van't Hoff equation, In(K /K1) = -(AHR/R) (T2-1 - 7,-1) The value of the thermodynamic equilibrium constant is Kp= 7.6e14
Using standard thermodynamic data from Appendix D, calculate the equilibrium constant at 311 K for the following chemical equilibrium: CO2(g) + 4H2(g) 2CH(0) + 2H20 (1) 1.16E19 The number of significant digits is set to 3; the tolerance is +/-2% Click if you would like to Show Work for this question: Open Show Work
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. H2(g) + Cl2(g)—>2HCI(g) K=
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. N2(g) + 3H2(9) 2NH3(g)
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction 2502(g) + O2(0) 2503(9) AH°F (kJ/mol) AGⓇ, (kJ/mol sº (/mol K) 205.1 Oxygen 02(0) (9) O3(9) 249.2 231.7 161.1 142.7 163.2 238.9 AH°: (kJ/mol Agºr (kJ/mol) 5° (J/mol K) 31.8 0.3 0.3 278.8 3 3.0 167.8 33.0 - 15.0 Sulfur S(s, rhombic) S(s, monodinic) S(g) Sz"(aq) Sg(9) SzCl2(g) SF6(9) H2S(9) soz(9) SO3(0) 1 0....
7 and 8
7. Using the Thermodynamic Data from Appendix 3 in your text book, calculate the standard reaction entropy of the following chemical reaction: N2 (g) + O2(g) 2 NO (g) 8. Using the Thermodynamic Data from Appendix 3 in your text book, calculate the standard reaction entropy of the following chemical reaction: Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H20 (1) 9. The standard reaction free energy AGº = -64.0 kJ for this...
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 641 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ /kJ mol-1 -314.4 -45.9 -92.3 Smº /JK-mol-1 94.6 192.8 186.9 Cp.m /JK-mol-1 84.1 35.1 29.1 Do not use the Van't Hoff equation, In(K/K) = -(AHR/R) (T2-1-T1-1) The value of the thermodynamic equilibrium constant is Kp = Number
Using any data you can find in the ALEKS Data resource,
calculate the equilibrium constant
K at 25.0°C for the following reaction.
6Cl2(g) + 2Fe2O3(s)
→ 4FeCl3(s)+ 3O2(g)
Round your answer to 2 significant digits.
O ENTROPY AND FREE ENERGY Using thermodynamic data to calculate K Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. 6 C12(g) + 2 Fe2O3(s) — 4 FeCl3(s) + 302(8) Round your answer to...
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 839 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ 7 kJ mol-1 -314.4 -45.9 -92.3 Smº JK-1 mol-1 94.6 192.8 186.9 Cp,m 84.1 35.1 29.1 /JK-1 mol-1 Do not use the Van't Hoff equation, In(K /K1) = -(AHR/R) (T2-1 - 7,-1) The value of the thermodynamic equilibrium constant is Kp= 7.6e14
Most questions answered within 3 hours.
-
If I was given the address of 134.15.0.0/16 from my ISP and I
wanted to use...
asked 27 seconds from now -
What is the pH of the solution that results of dissolving 1.74g
of sodium hydroxide in...
asked 3 minutes ago -
Given a standardized normal distribution (with μ = 0 and a σ =
1), what is...
asked 41 minutes ago -
Given the following information:
acetic acid
CH3COOH
Ka = 1.8×10-5
triethylamine
(C2H5)3N
Kb = 5.2×10-4
(1)...
asked 27 minutes ago -
Potassium permanganate(KMNO4)is has a solubility of 6.4 g/ 100 g
of water at 20ºC, and 250...
asked 24 minutes ago -
51.
As the marginal propensity to expend rises, the multiplier:
decreases.
is impossible to determine.
increases....
asked 30 minutes ago -
The Baldwin Company currently has the following balances on their
balance sheet:
Total
Liabilities
$69,309
Common...
asked 33 minutes ago -
A quiet town in Kansas has 10 people, all of whom have the same
preferences. There...
asked 38 minutes ago -
Summarize what an organization needs from a leader.
a. Analyze what might happen to an organization...
asked 41 minutes ago -
How would one critically evaluate an organizations marketing
strategies from the viewpoint of its consumers, as...
asked 40 minutes ago -
Company XYZ know that replacement times for the quartz time
pieces it produces are normally distributed...
asked 55 minutes ago -
A) Write the acid-base reaction that occurs between Na2HPO4 and
NaOH
B) Write the possible reactions...
asked 1 hour ago