Answer:
16.5 atm
Explanation:
<em>A mixture of He, N₂, and Ar has a pressure of 24.1 atm at 28.0 °C. If the partial pressure of He is 3013 torr and that of Ar is 2737 mm Hg, what is the partial pressure of N₂?</em>
The total pressure of a gaseous mixture is equal to the sum of the partial pressures.
P = pHe + pN₂ + pAr
pN₂ = P - pHe - pAr [1]
We need to express pHe and pAr in atm.
From [1],
pN₂ = 24.1 atm - 3.96 atm - 3.60 atm = 16.5 atm
<u>Answer:</u> The concentration of in the solution is
<u>Explanation:</u>
The given cell is:
Half reactions for the given cell follows:
<u>Oxidation half reaction:</u> ( × 3)
<u>Reduction half reaction:</u> ( × 2)
<u>Net reaction:</u>
Substance getting oxidized always act as anode and the one getting reduced always act as cathode.
To calculate the of the reaction, we use the equation:
Putting values in above equation, we get:
To calculate the concentration of ion for given EMF of the cell, we use the Nernst equation, which is:
where,
= electrode potential of the cell = 1.23 V
= standard electrode potential of the cell = +1.50 V
n = number of electrons exchanged = 6
Putting values in above equation, we get:
Hence, the concentration of in the solution is