The potential in an electrochemical cell, E, is related to the Gibb's free energy change (ΔG) for the overall cell redox reactio
1 answer:
You might be interested in
Answer:
The gas will occupy a volume of 1.702 liters.
Explanation:
Let suppose that the gas behaves ideally. The equation of state for ideal gas is:
(1)
Where:
- Pressure, measured in kilopascals.
- Volume, measured in liters.
- Molar quantity, measured in moles.
- Temperature, measured in Kelvin.
- Ideal gas constant, measured in kilopascal-liters per mole-Kelvin.
We can simplify the equation by constructing the following relationship:
(2)
Where:
,
- Initial and final pressure, measured in kilopascals.
,
- Initial and final volume, measured in liters.
,
- Initial and final temperature, measured in Kelvin.
If we know that ,
,
,
and
, the final volume of the gas is:
The gas will occupy a volume of 1.702 liters.
Answer:
1.65 L
Explanation:
The equation for the reaction is given as:
A + B ⇄ C
where;
numbers of moles = 0.386 mol C (g)
Volume = 7.29 L
Molar concentration of C =
= 0.053 M
A + B ⇄ C
Initial 0 0 0.530
Change +x +x - x
Equilibrium x x (0.0530 - x)
where
K is given as ; 78.2 atm-1.
So, we have:
Using quadratic formula;
where; a = 78.2 ; b = 1 ; c= - 0.0530
= or
= or
= 0.0204 or -0.0332
Going by the positive value; we have:
x = 0.0204
[A] = 0.0204
[B] = 0.0204
[C] = 0.0530 - x
= 0.0530 - 0.0204
= 0.0326
Total number of moles at equilibrium = 0.0204 + 0.0204 + 0.0326
= 0.0734
Finally, we can calculate the volume of the cylinder at equilibrium using the ideal gas; PV =nRT
if we make V the subject of the formula; we have:
where;
P (pressure) = 1 atm
n (number of moles) = 0.0734 mole
R (rate constant) = 0.0821 L-atm/mol-K
T = 273.15 K (fixed constant temperature )
V (volume) = ???
V = 1.64604
V ≅ 1.65 L