When determining the standard reduction potential of a substance by using a standard hydrogen electrode as a reference, the stan
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Answer:
1.18 V
Explanation:
The given cell is:
Half reactions for the given cell follows:
Oxidation half reaction:
Reduction half reaction:
Multiply Oxidation half reaction by 2 and Reduction half reaction by 3
Net reaction:
Oxidation reaction occurs at anode and reduction reaction occurs at cathode.
To calculate the of the reaction, we use the equation:
Putting values in above equation, we get:
To calculate the EMF of the cell, we use the Nernst equation, which is:
where,
= electrode potential of the cell = ?V
= standard electrode potential of the cell = +1.21 V
n = number of electrons exchanged = 6
Putting values in above equation, we get:
<u>Answer:</u> The mass difference between the two is 7.38 grams.
<u>Explanation:</u>
To calculate the number of moles, we use the equation given by ideal gas follows:
where,
P = pressure = 125 psi = 8.50 atm (Conversion factor: 1 atm = 14.7 psi)
V = Volume = 855 mL = 0.855 L (Conversion factor: 1 L = 1000 mL)
T = Temperature =
R = Gas constant =
n = number of moles = ?
Putting values in above equation, we get:
To calculate the number of moles, we use the equation:
.....(1)
- <u>For air:</u>
Moles of air = 0.297 moles
Average molar mass of air = 28.8 g/mol
Putting values in equation 1, we get:
Mass of air, = 8.56 g
- <u>For helium gas:</u>
Moles of helium = 0.297 moles
Molar mass of helium = 4 g/mol
Putting values in equation 1, we get:
Mass of helium, = 1.18 g
Calculating the mass difference between the two:
Hence, the mass difference between the two is 7.38 grams.