Calculate ∆ H for the reaction 2 NH 3 ( g ) + 1 2 O 2 ( g ) → N 2 H 4 ( l ) + H 2 O ( l ) given the following data: 2 NH 3 ( g ) + 3 N 2 O ( g ) → 4 N 2 ( g ) + 3 H 2 O ( l ) Δ H = − 1010. KJ N 2 O ( g ) + 3 H 2 ( g ) → N 2 H 4 ( l ) + H 2 O ( l ) Δ H = − 317 KJ N 2 H 4 ( l ) + O 2 ( g ) → N 2 ( g ) + 2 H 2 O ( l ) Δ H = − 623 KJ H 2 ( g ) + 1 2 O 2 ( g ) → H 2 O ( l ) Δ H = − 286 K J
Calculate ∆ H for the reaction 2 NH 3 ( g ) + 1 2 O 2 ( g ) → N 2 H 4 ( l ) + H 2 O ( l ) given the following data: 2 NH 3 ( g ) + 3 N 2 O ( g ) → 4 N 2 ( g ) + 3 H 2 O ( l ) Δ H = − 1010. KJ N 2 O ( g ) + 3 H 2 ( g ) → N 2 H 4 ( l ) + H 2 O ( l ) Δ H = − 317 KJ N 2 H 4 ( l ) + O 2 ( g ) → N 2 ( g ) + 2 H 2 O ( l ) Δ H = − 623 KJ H 2 ( g ) + 1 2 O 2 ( g ) → H 2 O ( l ) Δ H = − 286 K J
Solution Summary: The author explains that the enthalpy change of a reaction is self-determining of the route by which the chemical reaction take place.
2
NH
3
(
g
)
+
1
2
O
2
(
g
)
→
N
2
H
4
(
l
)
+
H
2
O
(
l
)
given the following data:
2
NH
3
(
g
)
+
3
N
2
O
(
g
)
→
4
N
2
(
g
)
+
3
H
2
O
(
l
)
Δ
H
=
−
1010.
KJ
N
2
O
(
g
)
+
3
H
2
(
g
)
→
N
2
H
4
(
l
)
+
H
2
O
(
l
)
Δ
H
=
−
317
KJ
N
2
H
4
(
l
)
+
O
2
(
g
)
→
N
2
(
g
)
+
2
H
2
O
(
l
)
Δ
H
=
−
623
KJ
H
2
(
g
)
+
1
2
O
2
(
g
)
→
H
2
O
(
l
)
Δ
H
=
−
286
K
J
Part 1. Aqueous 0.010M AgNO 3 is slowly added to a 50-ml solution containing both carbonate [co32-] = 0.105 M
and sulfate [soy] = 0.164 M anions. Given the ksp of Ag2CO3 and Ag₂ soy below. Answer the ff:
Ag₂ CO3 = 2 Ag+ caq) + co} (aq)
ksp = 8.10 × 10-12
Ag₂SO4 = 2Ag+(aq) + soy² (aq) ksp = 1.20 × 10-5
a) which salt will precipitate first?
(b)
What % of the first anion precipitated will remain in the solution.
by the time the second anion starts to precipitate?
(c) What is the effect of low pH (more acidic) condition on the separate of the carbonate and
sulfate anions via silver precipitation? What is the effect of high pH (more basic)? Provide appropriate
explanation per answer
Part 4. Butanoic acid (ka= 1.52× 10-5) has a partition coefficient of 3.0 (favors benzene) when distributed bet.
water and benzene. What is the formal concentration of butanoic acid in each phase when
0.10M aqueous butanoic acid is extracted w❘ 25 mL of benzene
100 mL of
a) at pit 5.00
b) at pH 9.00
Calculate activation energy (Ea) from the following kinetic data: Temp (oC) Time (s) 23.0 180. 32.1 131 40.0 101 51.8 86.0 Group of answer choices 0.0269 kJ/mole 2610 kJ/mole 27.6 kJ/mole 0.215 kJ/mole 20.8 kJ/mole
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