The potential of standard hydrogen electrode is zero. This implies that

Δ G_{f}^{0} (H^{+}, a q .) = 0

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Δ H_{f}^{0} (H^{+}, a q .) = 0

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Δ G_{f}^{0} (H^{+}, a q .) < 0

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Δ G_{f}^{0} (H^{+}, a q .) > 0

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Solution

The correct option is A $Δ G_{f}^{0} (H^{+}, a q .) = 0$
Using relation , $Δ G^{0} = - n F E_{c e l l}^{0}$
As $E_{c e l l}^{0} = 0$
$\Rightarrow Δ G^{0} = 0$

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Similar questions

The standard hydrogen electrode has zero electrode potential because:

The standard hydrogen electrode potential is zero because:

a) hydrogen oxidized easily

b) electrode potential is considered as zero

c) hydrogen atom has only one electron

d) all of this

[Pls explain answer]

Q. The standard hydrogen electrode potential is zero, because

Q. A standard hydrogen electrode has a zero potential because:

Can I say that standard electrode potential of any metal electrode is equal to the potential difference or e.m.f between that metal electrode and hydrogen electrode at standard conditions ?

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The potential of standard hydrogen electrode is zero. This implies that

The correct option is A ΔG0f(H+,aq.)=0Using relation , ΔG0=−nFE0cell As E0cell=0 ⇒ΔG0=0

The correct option is A $Δ G_{f}^{0} (H^{+}, a q .) = 0$
Using relation , $Δ G^{0} = - n F E_{c e l l}^{0}$
As $E_{c e l l}^{0} = 0$
$\Rightarrow Δ G^{0} = 0$