In the figure shown, AD, CE, and FB intersect at point F.
1 answer:
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Answer:
Partial pressure of nitrogen gas is 0.98 bar.
Explanation:
According to the Dalton's law, the total pressure of the gas is equal to the sum of the partial pressure of the mixture of gases.
where,
= total pressure = 3.9 bar
= partial pressure of nitrogen gas
= partial pressure of oxygen gas
= partial pressure of argon gases
= Mole fraction of nitrogen gas = 0.25
= Mole fraction of oxygen gas = 0.65
= Mole fraction of argon gases = 0.10
Partial pressure of nitrogen gas :
Partial pressure of oxygen gas :
Partial pressure of argon gas :
Answer:
ΔG° = -118x10³ J/mol
Explanation:
The two half-reactions in the cell are:
Oxidation half-reaction:
Co(s) → Co²⁺(aq) + 2e⁻; E° = -0,28V
Reduction half-reaction:
Cu²⁺(aq)+2e⁻ → Cu(s); E° = 0,34V
The E° of the cell is defined as:
Replacing:
0,34V - (-0,28V) = 0,62V
It is possible to obtain the keq from E°cell with Nernst equation thus:
nE°cell/0,0592 = log (keq)
Where:
E°cell is standard electrode potential (0.62 V)
n is number of electrons transferred (2 electrons, from the half-reactions)
Replacing:
0,62V×2/0,0592 = log (keq)
20,946 = log keq
keq = 8,83x10²⁰≈ 5,88x10²⁰
ΔG° is defined as:
ΔG° = -RT ln Keq
Where R is gas constant (8,314472 J/molK) and T is temperature (298K):
ΔG° = -8,314472 J/molK×298K ln5,88x10²⁰
<em>ΔG° = -118x10³ J/mol</em>
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I hope it helps!