Question

com and for t Consider the reaction: Fe,04(s) + 4H2)3Fe(s) +4H20() Using standard thermodynamic data at 298K, calculate the free energy change when 2.34 moles of Fe,04(8) react at standard conditions kJ rxn Retry Entire Group 3 more group attempts remaining

Answer 1

Given:

Gof(Fe3O4(s)) = -1015.4 KJ/mol

Gof(H2(g)) = 0.0 KJ/mol

Gof(Fe(s)) = 0.0 KJ/mol

Gof(H2O(g)) = -228.572 KJ/mol

Balanced chemical equation is:

Fe3O4(s) + 4 H2(g) ---> 3 Fe(s) + 4 H2O(g)

?Go rxn = 3*Gof(Fe(s)) + 4*Gof(H2O(g)) - 1*Gof( Fe3O4(s)) - 4*Gof(H2(g))

?Go rxn = 3*(0.0) + 4*(-228.572) - 1*(-1015.4) - 4*(0.0)

?Go rxn = 101.112 KJ/mol

This is ?Go rxn for 1 mol

so,

for 2.34 mol of Fe3O4,

?Go rxn = 2.34 mol * 101.112 KJ/mol

= 237 KJ

Answer: 237 KJ