N2 + O2 ----> 2NO Using standard thermodynamics data at 298 K, calculate the fre

Question

N2 + O2 ----> 2NO Using standard thermodynamics data at 298 K, calculate the free energy change when 1.640 moles of N2 react at standard conditions Delta G rxn ______ kJ
4HCl + O2 ------> 2H2O + 2Cl2 Using standard thermodynamics data at 298 K, calculate the free energy change when 2.26 moles of HCl react at standard conditions Delta G rxn ______ kJ
N2 + O2 ----> 2NO Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.64 moles of N2 react at standard conditions Delta S system ______ J/K

4HCl + O2 ------> 2H2O + 2Cl2 Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.26 moles of HCl react at standard conditions Delta S system ______ J/K
A student measures the molar solubility of iron III sulfide in a water solution to be 1.04 x 10^-18 M. The solubility product constant for this compound is ______
N2 + O2 ----> 2NO Using standard thermodynamics data at 298 K, calculate the free energy change when 1.640 moles of N2 react at standard conditions Delta G rxn ______ kJ
4HCl + O2 ------> 2H2O + 2Cl2 Using standard thermodynamics data at 298 K, calculate the free energy change when 2.26 moles of HCl react at standard conditions Delta G rxn ______ kJ
N2 + O2 ----> 2NO Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.64 moles of N2 react at standard conditions Delta S system ______ J/K

4HCl + O2 ------> 2H2O + 2Cl2 Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.26 moles of HCl react at standard conditions Delta S system ______ J/K
A student measures the molar solubility of iron III sulfide in a water solution to be 1.04 x 10^-18 M. The solubility product constant for this compound is ______
Using standard thermodynamics data at 298 K, calculate the free energy change when 1.640 moles of N2 react at standard conditions Delta G rxn ______ kJ
4HCl + O2 ------> 2H2O + 2Cl2 Using standard thermodynamics data at 298 K, calculate the free energy change when 2.26 moles of HCl react at standard conditions Delta G rxn ______ kJ Using standard thermodynamics data at 298 K, calculate the free energy change when 2.26 moles of HCl react at standard conditions Delta G rxn ______ kJ
N2 + O2 ----> 2NO Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.64 moles of N2 react at standard conditions Delta S system ______ J/K Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.64 moles of N2 react at standard conditions Delta S system ______ J/K

4HCl + O2 ------> 2H2O + 2Cl2 Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.26 moles of HCl react at standard conditions Delta S system ______ J/K 4HCl + O2 ------> 2H2O + 2Cl2 Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.26 moles of HCl react at standard conditions Delta S system ______ J/K Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.26 moles of HCl react at standard conditions Delta S system ______ J/K
A student measures the molar solubility of iron III sulfide in a water solution to be 1.04 x 10^-18 M. The solubility product constant for this compound is ______

Explanation / Answer

For,

N2 + O2 --> 2NO

dGrxn = 1.64[dG(products) - dG(reactants)]

           = 1.64(2 x 87.60)

           = 287.328 kJ

----

For,

4HCl + O2 --> 2H2O + 2Cl2

dGrxn = 2.26[dG(products) - dG(reactants)]

           = 2.26(2 x -228.6 + 4 x 95.3)

           = -171.760 kJ

----

For,

N2 + O2 --> 2NO

dSsys = 1.64[dS(products) - dS(reactants)]

           = 1.64[(2 x 210.5) - (191.6 + 205)]

           = 40.02 J/K

---

For,

4HCl + O2 --> 2H2O + 2Cl2

dSsys = 2.26[dS(products) - dS(reactants)]

           = 2.26[(2 x 188.7 + 2 x 223) - (4 x 186.6 + 205)]

           = -289.28 J/K

---

For Fe2S3

molar solubility = 1.04 x 10^-18 M

Ksp = [Fe3+]^2.[S^2-]^3

       = (2 x 1.04 x 10^-18)^2.(3 x 1.04 x 10^-18)^3

       = 1.32 x 10^-88

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