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The following questions refer to the following reaction at constant 25°C and 1 atm.2Fe(s) + (3/2)O2(g) + 3H2O(l)  2Fe(OH)3(s) H = –789 kJ/molSubstance S° (J/mol K)Fe(OH)3(s) 107Fe(s) 27O2(g) 205H2O(l) 70a. Determine Ssurr for the reaction (in kJ/mol K)b. Determine Suniv for the reaction (in kJ/mol K)2.65c. What is the G for this reaction?d. Calculate the equilibrium constant


The following questions refer to the following reaction at constant 25°C and 1 atm.
2Fe(s) + (3/2)O2(g) + 3H2O(l)  2Fe(OH)3(s) H = –789 kJ/mol
Substance S° (J/mol K)
Fe(OH)3(s) 107
Fe(s) 27
O2(g) 205
H2O(l) 70

a. Determine Ssurr for the reaction (in kJ/mol K)

b. Determine Suniv for the reaction (in kJ/mol K)2.65

c. What is the G for this reaction?

d. Calculate the equilibrium constant

Step 1

Enthalpy of a reaction refers to the amount of heat which is absorbed or released by a system  at a constant pressure during a chemical reaction and is denoted by the symbol ∆H. Positive sign of ∆H indicates that the heat is absorbed by the system while the negative sign indicates that the heat is released by the system. The  total enthalpy change for a given chemical reaction is given by the equation :

In the above equation i and j are the number of products and reactants respectively in the given chemical equation.

Step 2

Entropy of a system is defined as the randomness of a system. Larger or more positive the value of entropy more is the randomness of the system or more disordered is the system. In a chemical reaction the entropy is given by the sum of the entropies of products multiplied the number of moles corresponding to each product in the given chemical equation minus the sum of the entropies of reactants multiplied by their corresponding number of moles in the given chemical reaction equation.

Step 3

Gibbs free energy refers to the energy associated with a chemical reaction that can be used for p...


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