Electrochemistry Test

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Electrochemistry Test - 68

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Weekly Quiz Competition

Question 1
1 / -0

For the fuel cell reaction : $$2{H_2}\left( g \right) + {O_2}\left( g \right) \to 2{H_2}O\left( l \right);\quad {\Delta _f}H_{298}^ \circ \left( {{H_2}O,l} \right) = - 285.5\ kJ/mol$$ what is $$\Delta S_{298}^0$$ for the given fuel cell reaction?

Given: $${O_2}\left( g \right) + 4{H^ + }\left( {aq} \right) + 4{e^ - } \to 2{H_2}O\left( l \right)\,; \quad {E^ \circ } = 1.23V$$

A
$$0.322 kJ/K$$

B
$$-0.635kJ/K$$

C
$$3.51kJ/K$$

D
$$-0.322kJ/K$$

Solution
Question 2
1 / -0

The electrolysis of a solution resulted in the formation of $$H_{2}(g)$$ at the cathode and $$O_{2}(g)$$ at the anode. The solution is :

A
$$AgCl(aq)$$

B
highly concentrated $$H_{2}SO_{4}(aq)$$

C
highly concentrated $$HCl$$ solution

D
$$CuCl_{2}(aq)$$

Solution
Question 3
1 / -0

An electric current is passed through a copper voltameter and a water voltameter connected in series. If the copper of the copper voltameter now weights 16 mg less, hydrogen liberated at the cathode of the water voltameter measures at STP about:

A
$$4.0ml$$

B
$$5.6ml$$

C
$$6.4ml$$

D
$$8.4ml$$

Solution
Question 4
1 / -0

The charge in coulombs of 1 mole of $$ N^{3-} $$ is (The charge on an electron is: $$ 1.602 \times 10^{-19} C ) $$

A
$$ 2.894 \times 10^5 C $$

B
$$ 3.894 \times 10^5 C $$

C
$$ 2.894 \times 10^6 C $$

D
None of these

Solution
Question 5
1 / -0

Coulomb is equal to ........

A
ampere $$\times$$ second

B
ampere $$\times$$ minute

C
watt $$\times$$ second

D
volt $$\times$$ second

Solution

The coulomb (symbolized C) is the standard unit of electric charge in the International System of Units (SI)In terms of SI base units, the coulomb is the equivalent unit of one ampere-second.

So option A is correct.
Question 6
1 / -0

The current strength of $$3.863\ amp$$ was passed through molten calcium oxide for $$41$$ minutes and $$40$$ seconds. The mass of calcium in grams deposited at the cathode is: (Atomic mass of Ca is $$40\ g/mol, 1\ f=96500\ C)$$

A
$$4$$

B
$$2$$

C
$$6$$

D
$$8$$

E
$$1$$

Solution
Question 7
1 / -0

Consider the half-cell reaction(s)
$${Cu}^{2+}+{e}^{-}\rightarrow {Cu}^{+};{E}^{o}=0.15V$$
$${Cu}^{2+}+2{e}^{-}\rightarrow {Cu};{E}^{o}=0.33V$$
$${E}^{o}$$ for the half-cell reaction: $${Cu}^{+}+{e}^{-}\rightarrow Cu$$ will be:

A
$$0.48V$$

B
$$0.18V$$

C
$$0.31V$$

D
$$0.51V$$

Solution
Question 8
1 / -0

The charge required for the reduction of 1 mol of $${\text{MnO}}_{\text{4}}^{\text{ - }}$$ to $${\text{Mn}}{{\text{O}}_2}$$ is:

A
1 F

B
3 F

C
5 F

D
7 F

Solution
Question 9
1 / -0

Consider the following $$\;{{\text{E}}^{\text{o}}}\;$$ values,
$${{\text{E}}^{\text{o}}}_{{\text{F}}{{\text{e}}^{{\text{3 + }}}}{\text{/F}}{{\text{e}}^{{\text{2 + }}}}} = {\text{ + 0}}{\text{.77V}};$$$${{\text{E}}^{\text{o}}}_{{\text{S}}{{\text{n}}^{{\text{2 + }}}}{\text{/Sn}}} = - {\text{0}}{\text{.14V}}\;\;\;\;$$

Under standard conditions the potential for the reaction is:
$${\text{Sn}}\left( {\text{s}} \right){\text{ + 2F}}{{\text{e}}^{{\text{3 + }}}}\left( {{\text{aq}}} \right) \to {\text{2F}}{{\text{e}}^{{\text{2 + }}}}{\text{(aq) + S}}{{\text{n}}^{{\text{2 + }}}}\left( {{\text{aq}}} \right)$$

A
0.91 V

B
1.40 V

C
1.68 V

D
0.63 V

Solution
Question 10
1 / -0

Three faradays of electricity is passed through molten solutions of $$Ag{NO}_{3}, Ni{SO}_{4}$$ and $$Cr{Cl}_{3}$$ kept in three vessels using inert electrodes. The ratio in mol in which the metals $$Ag, Ni$$ and $$Cr$$ will be deposited is:

A
$$1:2:3$$

B
$$3:2:1$$

C
$$6:3:2$$

D
$$2:3:6$$

Solution