Calculate the standard entropy change for the reaction
P4(g)+5O2(g)→P4O10(s)
using the data from the following table:
Substance | ΔH∘f (kJ/mol) | ΔG∘f (kJ/mol) | S∘ [J/(K⋅mol)] |
P4(g) | 58.9 | 24.5 | 279.9 |
O2(g) | 0 | 0 | 205.0 |
P4O10(s) | −2984 | −2698 | 228.9 |
Solution :-
Formula to calculate the entropy chnage of the reaction using the standard entropy values is as follows
Delta S rxn = Sum delta S product - Sum of delta S reactant
delta S rxn = [1*P4O10(s)] - [(1*P4(g))+(5*O2(g))]
now lets put the entropy (S) values in the formula
Delta S rxn = [1*228.9] - [(1*279)+(5*205.0)]
Delta S rxn = -1075.1 J/ K
Thereefore the standard entropy change of the reaction = -1075.1 J/K
Calculate the standard entropy change for the reaction P4(g)+5O2(g)→P4O10(s) using the data from the following table:...
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> this is right :) thank you
weloveyoulaila xo Thu, Mar 31, 2022 7:30 PM