Pt,H+H2(g) Hydrogen electrode EH2/H+o=0.0Volt
H2(g)→2H(aq)++2e−
[H+]=10−7M at 25oC (for Pure water)
E=2−0.0591log(PH2[H+]2)
E=0=logPH2[H+]=0
∴[H+]2=PH2=(10−7)2
∴PH2=10−14atm
NEET UG 2016 — Chemistry Physical Chemistry
The pressure of H2 required to make the potential of hydrogen electrode zero in pure water at 298 K is:
Held on 30 Apr 2016 · Verified 9 Jul 2026.
10−14atm
10−12atm
10−10atm
10−4atm
Sign in to track your attempts and accuracy.
Sign in to keep a private note on this question. Nothing you write is ever public.
The unit of rate constant for a first-order reaction is:
For the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), ΔH = -198 kJ. Which condition favours forward reaction?
$\begin{aligned} &\text { Consider the following compounds: }\\ &\mathrm{\underline{K}O}_2, \mathrm{H}_2 \mathrm{\underline{O}}_2 \text { and } \mathrm{H}_2 \mathrm{\underline{S}O}_4 \text {. } \end{aligned}$ The oxidation states of the underlined elements in them are, respectively,
5 moles of liquid X and 10 moles of liquid Y make a solution having a vapour pressure of 70 torr. The vapour pressures of pure X and Y are 63 torr and 78 torr respectively. Which of the following is true regarding the described solution?
For the reaction $\mathrm{A}(\mathrm{g}) \rightleftharpoons 2 \mathrm{~B}(\mathrm{~g})$, the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500 , at 1000 K . [Given : $\mathrm{R}=0.0831 \mathrm{~L} \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ ] $\mathrm{K}_{\mathrm{p}}$ for the reaction at 1000 K is
Work through every NEET UG Physical Chemistry PYQ, year by year.