Answer:
a. 7278 K
b. 4.542 × 10⁻³¹
Explanation:
a.
Let´s consider the following reaction.
N₂(g) + O₂(g) ⇄ 2 NO(g)
The reaction is spontaneous when:
ΔG° < 0 [1]
Let's consider a second relation:
ΔG° = ΔH° - T × ΔS° [2]
Combining [1] and [2],
ΔH° - T × ΔS° < 0
ΔH° < T × ΔS°
T > ΔH°/ΔS°
T > (180.5 × 10³ J/mol)/(24.80 J/mol.K)
T > 7278 K
b.
First, we will calculate ΔG° at 25°C + 273.15 = 298 K
ΔG° = ΔH° - T × ΔS°
ΔG° = 180.5 kJ/mol - 298 K × 24.80 × 10⁻³ kJ/mol.K
ΔG° = 173.1 kJ/mol
We can calculate the equilibrium constant using the following expression.
ΔG° = - R × T × lnK
lnK = - ΔG° / R × T
lnK = - 173.1 × 10³ J/mol / (8.314 J/mol.K) × 298 K
K = 4.542 × 10⁻³¹
Answer:

Explanation:
Hello,
In this case, we can use the ideal gas equation:

So we know the temperature, pressure and volume, therefore we can easily compute the required moles as shown below:

Best regards.
Answer:
yep yep yep yep yep yep yep yep yep yep so cool yep
yep
yep
yep
yep
yep
yep
yep
yep
yep
yep
yep
yep
yep
yep
yep
yep
yel
yep
ype
yl
yrdvt
f4ef
te
g
5
ey
rw
f
t
t
e
c
t
y
r
e
s
f
t
4
e
d
g
t
r
e
f
r
r
e
e
f
r
r
r
r
e
Explanation:
nr
e
e
t
y
e
f
r
Answer:
4060
Explanation:
hope this helps
follow me for more answers
It is kept constant
There is the answer if it helped