Entropy, denoted by the symbol S, is the thermodynamic property describing the amount of molecular randomness or disorder in a system. It is a state thermodynamic function, meaning that its value does not depend on the path used to arrive at a specific set of conditions. Each system with a specified temperature, pressure, and composition has a unique entropy value.
The entropy change, ΔS, is the difference in entropy between two states of a system, such as between the reactants and products of a reaction or between a flask before and after adding a mixture of gas.
Part B
Calculate the standard-state entropy for the following reaction:
1 Al2O3(s) + 3 H2(g) → 2 Al(s) + 3 H2O(l)
(If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table.
Srxn = Sproducts - Sreactants
Srxn = 2*28 + 3*189 - (51 + 3*131) = 179 J/moK
Srxn = 179 J/moK
Calculate the standard-state entropy for the following reaction: 1 Al2O3(s) + 3 H2(g) ? 2 Al(s) + 3 H2O(l) (If applica...
Calculate the standard-state entropy for the following reaction: 1 Al2O3(s) + 3 H2(g) ? 2 Al(s) + 3 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. S? J/(K?mol) Al(s) 28.0 H2O(l) 189 Al2O3(s) 51.0 H2(g) 131
Calculate the standard-state entropy for the following reaction: 1 Al2O3(s) + 3 H2(g) ⟶ 2 Al(s) + 3 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) Al(s) 28.0 H2O(l) 189 Al2O3(s) 51.0 H2(g) 131
Calculate the standard-state entropy for the following reaction: 1 CH4(g) + 2 O2(g) ⟶ 1 CO2(g) + 2 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) CO2(g) 214 H2O(l) 189 CH4(g) 186 O2(g) 205
Calculate the standard-state entropy for the following reaction: 6 CO2(g) + 6 H2O(l) ⟶ 1 C6H12O6(s) + 6 O2(g) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) C6H12O6(s) 212 O2(g) 205 CO2(g) 214 H2O(l) 189
1) Calculate the standard-state entropy for the following reaction:2 NiS(s)+ 3 O2(g)→ 2 SO2(g)+ 2 NiO(s)(If applicable, coefficients of one have been included for clarity.)The standard entropy values are given in the table.Formula S J/(K*mol)SO2(g) 248NiO(s) 38.0NiS(s) 53.0O2(g) 205Express your answer in joules per kelvin to three significant figures.
Model - Entropy as a State Function Entropy, S, as with all other state functions like internal energy, E, and enthalpy, H, is a function of the state of a system. Because measuring the absolute state of a system more difficult than measuring the changes in its states, it is the change in entropy, ΔS, in which we will be interested. This means the only aspects that will interest us will be the difference in the final and initial entropies...
Calculate the standard-state entropy for the following reaction: 2NiS(s) + 3O2(g) -> 2SO2(g) + 2NiO(s) The standard entropy values are given in the table. Formula S - J/K SO2(g) 248 NiO(s) 38.0 NiS(s) 53.0 O2(g) 205
9. Consider the reaction Fe,0,(3) + 3 H2(g) —2 Fe(s) + 3 H2O(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K. ANSWER: Submit Answer Retry Entire Group 9 more group attempts remaining Consider the reaction 2502(g) + O2(g) —2503(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K. ANSWER: Submit Answer Retry Entire Group 9 more group attempts remaining
1) Consider the reaction: P4O10(s) + 6H2O(l)------>4H3PO4(aq) Using standard absolute entropies at 298K, calculate the entropy change for the systemwhen 1.53 moles ofP4O10(s) react at standard conditions. S°system = J/K 1b) Consider the reaction: 2H2O2(l)--------->2H2O(l) +O2(g) Using standard absolute entropies at 298K, calculate the entropy change for the systemwhen 1.87 moles ofH2O2(l) react at standard conditions. S°system = J/K
Given that: 2Al(s)+(3/2)O2(g)--->Al2O3(s) change in H(rxn)= -1601 kJ/mol 2Fe(s)+(3/2)O2(g)--->Fe2O3(s) change in H(rxn)= -821 kJ/mol Calculate the standard enthalpy change for the following reaction: 2Al(s)+Fe2O3(s)--->2Fe(s)+Al2O3(s) _______kJ