Question

In: Chemistry

Use data from Appendix C to calculate the equilibrium constant, K, and ΔG∘ at 298 K...

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 and include the appropriate units.

Part D

Calculate the equilibrium constant, K.

Express your answer using two significant figures.

Part E

3C2H2(g)⇌C6H6(g)
Calculate ΔG∘.

Express your answer to four significant figures and include the appropriate units.

Part F

Calculate the equilibrium constant, K.

Express your answer using one significant figure.

Solutions

Expert Solution

queen_honey_blossom answered 3 years ago
Next > < Previous

Related Solutions

Given the thermodynamic data in the table below, calculate the equilibrium constant (at 298 K) for...
Given the thermodynamic data in the table below, calculate the equilibrium constant (at 298 K) for the reaction:             2SO2 (g) + O2 (g) à 2SO3 (g)                    
Calculate the equilibrium constant at 298 K for the reaction of ammonia with oxygen to form...
Calculate the equilibrium constant at 298 K for the reaction of ammonia with oxygen to form nitrogen and water. The data refer to 298 K. 4NH3(g) + 3O2(g) <> 2N2(g) + 6H2O(l) Substance NH3(g) O2(g) N2(g) H2O(l) ΔH°f (kJ/mol) -46 0 0 -285 ΔG°f (kJ/mol) -16 0 0 -237 S°(J/K·mol) 192 205 192 70 I thought Kc is just Molar concentration of Products divide by Molar concentration on Reactants which would be 12 x 16 divide by 14 x 13...
Using values from Appendix C of your textbook, calculate the value of Keq at 298 K...
Using values from Appendix C of your textbook, calculate the value of Keq at 298 K for each of the following reactions: (A) 2 NO(g) N2(g) + O2(g) (B) 3 NO(g) NO2(g) + N2O(g) (C) 2 HI(g) H2(g) + I2(g) Appendix C page screenshots are below: http://i.imgur.com/fHg7YIC.png http://i.imgur.com/nGvqHNp.png http://i.imgur.com/YPDGm2N.png
Use data from Appendix IIB in the textbook to calculate the equilibrium constants at 25?C for...
Use data from Appendix IIB in the textbook to calculate the equilibrium constants at 25?C for each of the following reactions. 2NO(g)+O2(g)?2NO2(g) . Express your answer using two significant figures.
Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K. X(s)...
Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K. X(s) + Y^2+(aq) ⇌ X^2+(aq) + Y(s)     K= 1.43 x 10^-6     E^o = ? V
Using the following thermochemical tables, calculate the indicated equilibrium constant at 298 K for the following...
Using the following thermochemical tables, calculate the indicated equilibrium constant at 298 K for the following reactions. (a) H2(g) + I2(s) -> 2HI(g) Kp = ? (b) NH3(aq) + H2O(l) = NH4+(aq) + OH-(aq) Kb = ? (c) Fe(OH)2(s) = Fe2+(aq) + 2OH-(aq) Ksp = ? Substance ΔHo (kJ/mol) ΔGo (kJ/mol) So (J/mol K) Al(s)             0                          0                   28.32 Al2O3(s)    -1669.8             -1576.5               51.0 CH3OH(l) -238.6               -166.23              126.8 CO(g)        -110.5               -137.2                197.9 CO2(g)       -393.5               -394.4                213.6 Cl2(g)            0                         0                   222.96 Cl –(aq)...
Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: Co2+(aq)...
Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: Co2+(aq) + 2I-(aq) Co(s) + I2(s) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant:
Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: I2(s)...
Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: I2(s) + Hg(l) = 2I-(aq) + Hg2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: -------
Using the data in Appendix C in the textbook and given the pressures listed, calculate ΔG...
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...
Consider the reaction: 2 NO2(g) → N2O4(g) Calculate ΔG (in kJ/mol) at 298°K if the equilibrium...
Consider the reaction: 2 NO2(g) → N2O4(g) Calculate ΔG (in kJ/mol) at 298°K if the equilibrium partial pressures of NO2 and N2O4 are 1.337 atm and 0.657 atm, respectively.
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT