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For the EMF of a hydrogen electrode to be zero, the pressure of hydrogen required in neutral pH at 90°C, is 10–x. Determine x:
Correct answer is '12'. Can you explain this answer?
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For the EMF of a hydrogen electrode to be zero, the pressure of hydrog...
°C is 1 atm (standard pressure). This is known as the standard hydrogen electrode (SHE) and is used as a reference for measuring the electrode potential of other half-cells in electrochemical reactions.
The half-reaction at the SHE is:
H2(g) → 2H+(aq) + 2e-
The electrode potential of the SHE is defined as 0.00 V at all temperatures and pressures. This means that any other half-cell connected to the SHE will have a potential difference relative to the SHE, which can be measured using a voltmeter.
The hydrogen pressure required for the SHE to be established at 90°C is 1 atm, which is the standard pressure. However, at higher or lower temperatures, the pressure required for the SHE may be different due to the change in the equilibrium constant of the half-reaction.
The half-reaction at the SHE is:
H2(g) → 2H+(aq) + 2e-
The electrode potential of the SHE is defined as 0.00 V at all temperatures and pressures. This means that any other half-cell connected to the SHE will have a potential difference relative to the SHE, which can be measured using a voltmeter.
The hydrogen pressure required for the SHE to be established at 90°C is 1 atm, which is the standard pressure. However, at higher or lower temperatures, the pressure required for the SHE may be different due to the change in the equilibrium constant of the half-reaction.
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For the EMF of a hydrogen electrode to be zero, the pressure of hydrog...
H+(aq) + e− → 1/2 H2(g)
Since standard potential= 0 , then(according to Nerstt equation) for the emf to be 0 :
log{ [H2]^0.5 / [H+] } = 0 or [H2]^0.5 / [H+] = 1
Now at 90 C, KW = 10^(-12) . So neutral is at 10^(-6)
On putting value in it and solving we get [H2] = 10^(-12) . Hence x=12
Since standard potential= 0 , then(according to Nerstt equation) for the emf to be 0 :
log{ [H2]^0.5 / [H+] } = 0 or [H2]^0.5 / [H+] = 1
Now at 90 C, KW = 10^(-12) . So neutral is at 10^(-6)
On putting value in it and solving we get [H2] = 10^(-12) . Hence x=12
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For the EMF of a hydrogen electrode to be zero, the pressure of hydrogen required in neutral pH at 90°C, is 10–x. Determine x:Correct answer is '12'. Can you explain this answer?
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