Indicate which of the four cases in Table 13.3 applies to each of the following reactions. If you are unable to decide from only the information given, state why. a. PCl s ( g ) +Cl 2 ( g ) → PCl 5 ( g ) b. Δ t H ° = − 87.9 kJmol − 1 NH 4 CO 2 NH 2 ( s ) → 2 NH 3 ( g ) + CO 2 ( g ) c. NH 4 CO 2 NH 2 ( s ) → 2 NH 3 ( g ) + CO 2 ( g ) NH 4 CO 2 N H 2 ( s ) → 2 NH 3 ( g ) + CO 2 ( g )
Indicate which of the four cases in Table 13.3 applies to each of the following reactions. If you are unable to decide from only the information given, state why. a. PCl s ( g ) +Cl 2 ( g ) → PCl 5 ( g ) b. Δ t H ° = − 87.9 kJmol − 1 NH 4 CO 2 NH 2 ( s ) → 2 NH 3 ( g ) + CO 2 ( g ) c. NH 4 CO 2 NH 2 ( s ) → 2 NH 3 ( g ) + CO 2 ( g ) NH 4 CO 2 N H 2 ( s ) → 2 NH 3 ( g ) + CO 2 ( g )
Solution Summary: The author explains the Gibb's equation of thermodynamic purposed a relation between S,
Indicate which of the four cases in Table 13.3 applies to each of the following reactions. If you are unable to decide from only the information given, state why.
a.
PCl
s
(
g
)
+Cl
2
(
g
)
→
PCl
5
(
g
)
b.
Δ
t
H
°
=
−
87.9
kJmol
−
1
NH
4
CO
2
NH
2
(
s
)
→
2
NH
3
(
g
)
+
CO
2
(
g
)
c.
NH
4
CO
2
NH
2
(
s
)
→
2
NH
3
(
g
)
+
CO
2
(
g
)
NH
4
CO
2
N
H
2
(
s
)
→
2
NH
3
(
g
)
+
CO
2
(
g
)
Blocking Group are use to put 2 large sterically repulsive group ortho. Show the correct sequence toconnect the reagent to product with the highest yield possible. * see image **NOTE: The compound on the left is the starting point, and the compound on the right is the final product. Please show the steps in between to get from start to final, please. These are not two different compounds that need to be worked.
I dont understand this.
Can you please explain this prooblem to me, show me how the conjugation is added, did I add them in the correct places and if so please show me. Thanks!
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning