Please answer all parts, explain and show work. Thank you. When I look at a tabl

Question

Please answer all parts, explain and show work. Thank you.

When I look at a table of standard entropies, I see that the amino acid glycine CH_2(NH_2)COOH_(S) has a S degree = 103.5 J/K/mol while methylamine CH_3NH_2_(g) has S degree = 243.41 J/K/mol. This seems like nonsense, as glycine has a higher heat capacity it seems it should have more entropy (remember S is -C_p DeltaT). Is there a sensible reason why they are so different? methylamine is used to make pesticides and drugs like ephedrine and methamphetamine) Urea hydrolyzes with water to make ammonia, giving it a bad smell. Using the table in your book, calculate the changes in molar entropy and Gibbs free energy (Delta S degree and Delta G degree) at standard temperature and pressure for the following reaction: (NH_2) _2CO_ (s) + H_2O_(l) rightarrow 2NH_3_ (g) + CO_2 (g) The value of Delta_f G degree(urea_(S)) in the book is wrong! It should be -196.8 kJ/mol. Using the data above, can you calculate Delta H degree as well? How does it compare to calculating Delta H degree from values in the table?

Explanation / Answer

Heat capacity has nothing to do with the entropy of the compound as entropy is actually the degree of randomness or measure of the degree of disorder of a compound.

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.