$$2H^+ (aq)+2e^- \to H_2(g)$$. The standard electrode potential for the above reaction is (in volts):
A
$$0$$
B
$$+1$$
C
$$None\ of\ these$$
D
$$-1$$
Open in App
Solution
Verified by Toppr
Correct option is A. $$0$$ Standard electrode potential of Hydrogen is zero. Option A is correct.
Was this answer helpful?
2
Similar Questions
Q1
$$2H^+ (aq)+2e^- \to H_2(g)$$. The standard electrode potential for the above reaction is (in volts):
View Solution
Q2
The standard e.m.f. of the cell involving the reaction, 2Ag+(aq)+H2(g)→2Ag(s)+2H+(aq), is 0.80 V. The standard oxidation potential of Ag electrode is :
View Solution
Q3
The standard reduction potentials at 298K for the following half cell reaction are given below:
Based on the above reactions, select the strongest reducing agent?
View Solution
Q4
The standard reduction potential at 250C for the following half reactions are given against each -
Zn+2(aq)+2e⇌Zn(s),E0=−0.76 volt. Cr+3(aq)+3e⇌Cr(s),Eo=−0.74 volt. 2H+(aq)+2e⇌H2(g),Eo=+0.0 volt. Fe+3(aq)+e⇌Fe+2(aq),Eo=+0.77 volt.
Which is the strongest reducing agent?
View Solution
Q5
The standard reduction potential at 298 K for following half reactions are given against each Zn2+(aq)+2e−⇌Zn(s);−0.762 Cr3+(aq)+3e−⇌Cr(s);−0.740 2H⨁(aq)+2e−⇌H2(g);0.000 Fe3+(aq)+3e−⇌Fe2+(aq);0.770 Which is the strongest reducing agent ?