Answer to Question #189767 in Chemistry for Michael

Question #189767

Calculate the ΔGo (in kJ/mol) of the following reaction at 298 K. Express your answer in four significant figures and omit the unit.


N

H

3

(

g

)

+

H

C

l

(

g

)

N

H

4

C

l

(

s

)

Δ

G

o

f

[

N

H

3

(

g

)

]

=

16.48

k

J

m

o

l

Δ

G

o

f

[

H

C

l

(

g

)

]

=

95.30

k

J

m

o

l

Δ

G

o

f

[

N

H

4

C

l

(

s

)

]

=

202.9

k

J

m

o

l



1
Expert's answer
2021-05-06T07:39:25-0400

Solution:

Balanced chemical equation:

NH3(g) + HCl(g) → NH4Cl(s)


ΔGof[NH3(g)] = −16.48 kJ/mol

ΔGof[HCl(g)] = −95.30 kJ/mol

ΔGof[NH4Cl(s)] = −202.9 kJ/mol


ΔGor = ΔGof[NH4Cl(s)] − (ΔGof[NH3(g)] + ΔGof[HCl(g)])

ΔGor = −202.9 kJ/mol − (−16.48 kJ/mol + (−95.30 kJ/mol)) = −91.12 kJ/mol

ΔGor = −91.12 kJ/mol


Answer: ΔGor = −91.12 kJ/mol

Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!

Comments

No comments. Be the first!

Leave a comment

LATEST TUTORIALS
New on Blog
APPROVED BY CLIENTS