Download App

2. Electrochemistry — Chemistry STD 12 Science — Question

Gujarat BoardEnglish MediumSTD 12 ScienceChemistry2. Electrochemistry1 Mark
MCQ
In a typical fuel cell, the reactant ($R$) and product ($P$) are
  • A
    $R=H_{2(g)} \cdot N_{2(g)}: P=N H_{3(a q)}$
  • B
    $R=H_{2(g)} \cdot O_{2(g)}: P=H_{2} O_{2(n)}$
  • ✓
    $R=H_{2(g)} \cdot O_{2(g)}: P=H_{2} O_{(n}$
  • D
    $R=H_{2(g)} \cdot O_{2(g)} \cdot C I_{2(g)}: P=H C I O_{4( aq )}$
✓

Answer

Correct option: C.
$R=H_{2(g)} \cdot O_{2(g)}: P=H_{2} O_{(n}$
c
Cell reaction involved in hydrogen-oxygen fuel cell is

$2 H _{2}( g )+ O _{2}( g ) \longrightarrow 2 H _{2} O (\ell)$

Need a full question paper?

Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.

Start Generating Free

Explore more

More "M.C.Q (1 Marks)" from 2. Electrochemistry→2. Electrochemistry — all question types→Chemistry STD 12 Science question papers→Gujarat Board STD 12 Science question papers→Gujarat Board question paper generator→

Similar questions

The oxidation state of $Cr$ in ${[Cr{(N{H_3})_4}C{l_2}]^ + }$ is
→
A hydrogen gas electrode is made by dipping platinum wire in a solution of $HCl$ of $pH = 10$ and by passing hydrogen gas around the platinum wire at one atm pressure. The oxidation potential of electrode would be .......... $V.$
→
The incorrect statement $(s)$ about $O_3$ is (are)
→
The spin only magnetic moment value of the ion among $\mathrm{Ti}^{2+}, \mathrm{V}^{2+}, \mathrm{Co}^{3+}$ and $\mathrm{Cr}^{2+}$, that acts as strong oxidising agent in aqueous solution is .......... BM (Near integer).

(Given atomic numbers: $\mathrm{Ti}: 22, \mathrm{~V}: 23, \mathrm{Cr}: 24$, Co: $27$)

→
The standard reduction potentials at $298 \mathrm{~K}$ for the following half cells are given below :

$\mathrm{Cr}_2 \mathrm{O}_7{ }^{2-}+14 \mathrm{H}^{+}+6 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cr}^{3+}+7 \mathrm{H}_2 \mathrm{O}, \mathrm{E}^{\circ}=1.33 \mathrm{~V}$

$\mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}  \mathrm{E}^{\circ}=-0.04 \mathrm{~V}$

$\mathrm{Ni}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Ni}  \mathrm{E}^{\circ}=-0.25 \mathrm{~V}$

$\mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Ag} \mathrm{E}^{\circ}=0.80 \mathrm{~V}$

$\mathrm{Au}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Au} \mathrm{E}^{\circ}=1.40 \mathrm{~V}$

Consider the given electrochemical reactions, The number of metal$(s)$ which will be oxidized be $\mathrm{Cr}_2 \mathrm{O}_7{ }^{2-}$, in aqueous solution is. . . . . . 

→
The formation of $PH_4^+$ is difficult compared to $NH_4^+$ because
→
A solution of a salt of a metal was electrolysed for $150$ minutes with a current of $0.15$ amperes. The weight of metal deposited was $0.783\,gm$. The equivalent weight of the metal is ................... $\mathrm{gm}$
→
The reduction of benzoyl chloride with $Pd$ and $BaSO_4/CaCO_3$ produces :
→
For the reaction $4NH_3 + 5O_2 \to 4NO + 6H_2O$ , if the rate of disappearance of $NH_3$ is $3.6 \times 10^{-3}\, mol\, L^{-1}\,s^{-1}$ , what is the rate of formation of $H_2O$ ?
→
Efficiency of a cell with cell reaction under standard conditions is $70\%$ cell reaction

${A_{\left( s \right)}} + {B^ \oplus } \longrightarrow {A^ \oplus } + {B_{\left( s \right)}}\,;\,\Delta {H^o} =  - 551.5\,KJ$ Calculate standard electrode potential of cell (in $volt$). .......... $\mathrm{volt}$

→