If you don’t mind can u add the picture?? It helps me answer the question better ;)
Answer:
3 °C
Explanation:
The pressure is constant, so this looks like a case where we can use Charles’ Law:
Invert both sides of the equation.
Multiply both sides by <em>V</em>₂
<em>V</em>₁ = 13.3 L; <em>T</em>₁ = (55 + 273.15) K = 328.15 K
<em>V</em>₂ = 11.2 L; <em>T</em>₂ = ?
Answer:
Equilibrium Constant = (3.60 × 10⁶²)
Explanation:
The change in Gibb's free energy for a galvanic cell is given as
Δ = -nFE°
where n = number of electrons transferred = 5 for this reaction
F = Faraday's constant = 96500 C
E° = cell potential = +0.74 V
But the change in Gibb's free energy for galvanic cell reaction is also given as
ΔG = -RT In K
R = molar gas constant = 8.314 J/mol.K
T = absolute temperature in Kelvin = 25 + 273.15 = 298.15 K
K = Equilibrium constant.
Equating these two expressions
-nFE° = - RT In K
RT In K = nFE°
In K = (nFE°) ÷ (RT)
In K = (5 × 96500 × 0.74) ÷ (8.314 × 298.15)
In K = 144.04
K = e^(144.04)
K = (3.60 × 10⁶²)
Hope this Helps!!!
By applying the ideal gas law, PV=nRT
<span>Cadmium Permanganate
Cd - Cadmium
Mn - Manganese
O - Oxygen (-ate)
Hope this helps!
</span>
