14)14) Given the thermodynamic data in the table below, calculate the equilibrium constant (at 298K) forthe reaction:1.8M1.885-2 SO2 (g) + O2 (g) = 2 SO3 (g)aseSubstance AHf (kJ/mol) S° (J/mol K)249 88.1820110SO2 (g)02 (g)SO3 (g)-297(oldmorh a) 2205000-e ear--395256ali mor D09lonoideonodoi orits s lo suisy ontEA) 2.37 x 1024B) 1.06C) 1.95+ ()D) 3.82 x 1023E) More data are needed.Jom\4

The equilibrium constant (K) is related with standard Gibb’s free energy change as follows: Where,…

Answered: 14) 14) Given the thermodynamic data in…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 16P

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Similar questions

Tetrachloromethane (carbon tetrachloride), CCl4, has a normal boiling point of 76.7C and an enthalpy of vaporization, Hvap, of 29.82 kJ/mol. Estimate the entropy of vaporization, Svap. Estimate the free energy of vaporization, Gvap, at 25C.
Calculate the standard free-energy change and the equilibrium constant Kp for the following reaction at 25C. See Appendix C for data. CO(g)+2H2(g)CH3OH(g)
Given the following data at 25C 2NO(g)N2(g)+O2(g)K=1 10 30 2NO(g)+Br2(g)2NOBr(g)K=8 101 Calculate K for the formation of one mole of NOBr from its elements in the gaseous state.
Titanium(IV) oxide is converted to titanium carbide with carbon at a high temperature. TiO2(s) + 3 C(s) 2 CO(g) + TiC(s) (a) Calculate rG and K at 727 C. (b) Is the reaction product-favored at equilibrium at this temperature? (c) How can the reactant or product concentrations be adjusted for the reaction to proceed at 727 C?
Acetic acid, CH3CO2H, can form a dimer, (CH3CO2H)2, in the gas phase.. 2CH3CO2H(g)(CH3CO2H)2(g) The dimer is held together by to hydrogen bonds with a total strength of 66.5 kJ per mole of dimer. At 25 C, the equilibrium constant for the dimerization is 1.3103 (pressure in atm). What is ?S for the reaction?
Hydrogen gas and iodine vapor react to produce hydrogen iodide gas: H2(g)+I2(g)2HI(g) Calculate the free-energy change G for the following two conditions, at 25C. Which one is closer to equilibrium? Explain. a The partial pressures of H2(g), I2(g). and HI(g) are each 13 atm. b The partial pressures of H2(g) and I2(g) are each 13 atm; the partial pressure of HI(g) is 190 atm.
Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7 J/mol K. Calculate the equilibrium partial pressures of I2(g), H2(g), and HI(g) for the system 2HI(g)H2(g)+I2(g) at 500°C if the initial partial pressures are all 0.200 atm.
Use data given in Tables 6.2 and 18.1 to obtain the value of Kp at 1000C for the reaction C(graphite)+CO2(g)2CO(g) Carbon monoxide is known to form during combustion of carbon at high temperatures. Do the data agree with this? Explain.
Benzene can be prepared from acetylene. 3C2H2(g)C6H6(g). Determine the equilibrium constant at 25 C and at 850 C. Is the reaction spontaneous at either of these temperatures? Why is all acetylene not found as benzene?
Use data given in Tables 6.2 and 18.1 to obtain the value of Kp at 2000C for the reaction N2(g)+O2(g)2NO(g) Nitric oxide is known to form in hot flames in air, which is a mixture of N2 and O2. It is present in auto exhaust from this reaction. Are the data in agreement with this result? Explain.
Is the following reaction spontaneous as written? Explain. Do whatever calculation is needed to answer the question. CH4(g)+N2(g)HCN(g)+NH3(g)
A reaction has K = 1.9 1014 at 25C and K = 9.1 103 at 227C. Predict the signs for G, H and S for this reaction at 25C. Assume H and S do not depend on temperature.

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