In the cell reaction Cu + 2Ag+→ 2Ag + Cu2+, Anode is the oxidation half-cell Reaction - Cu → Cu2+ + 2e- Cathode is the reduction half-cell Reaction - 2Ag+ + 2e- →2Ag
with platinum electrodes.
with platinum electrodes.Solution: (iii) At the cathode, the following reduction reaction occurs to produce $H_{2}$ gas. $$ H{(a q)}^{+}+e^{-} \rightarrow \frac{1}{2} H_{2(g)}$$At the anode, the following processes are...
with silver electrodes. (ii) An aqueous solution of with platinum electrodes.Solution: (i) At the cathode: The following reduction reactions are in competition with one another for space at the cathode.$$A g_{(a q)}^{+}+e^{-} \rightarrow A g_{(s)} ; E ^{0}=0.80 V$$$$H_{(a...
and 
Solution: When it comes to electrochemistry, the term "standard electrode potential" refers to the value obtained by measuring the standard emf of a cell in which molecular hydrogen under standard...
and 
and Solution: When it comes to electrochemistry, the term "standard electrode potential" refers to the value obtained by measuring the standard emf of a cell in which molecular hydrogen under standard...
and 
and 
Solution: When it comes to electrochemistry, the term "standard electrode potential" refers to the value obtained by measuring the standard emf of a cell in which molecular hydrogen under standard...
and 
, respectively are connected in series. A steady current of 
amperes was passed through them until 
of silver was deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?According to the information given in the question the reaction will be,$$A g_{(a q)}^{+}+e^{-} \rightarrow A g_{(s)}$$i.e., $108 g$ of $Ag$ is deposited by $96487 C$.Therefore, $1.45 g$ of $Ag$ is...
is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?Solution: As a result of the reaction, it is $$N i^{2+}+2 e^{-} \rightarrow N i_{(s)}+e^{-}$$ Nickel deposited by $2 \times 96487 C =58.71 g$ Therefore, nickel deposited by $6000 C =\frac{58.71...
to 
?
?Solution: (i) From given data, we write the equations that can be derived$$H_{2} O \rightarrow H_{2}+\frac{1}{2} O_{2} $$ We can say that : $$ O^{2-} \rightarrow \frac{1}{2} O_{2}+2...
of 
from molten 
? 
of 
from molten 
?Solution: (i) From given data, we write the equation of cell, $$Ca ^{2+}+2 e^{-} \rightarrow Ca$$ Evaluating the value of electricity in terms of Faraday we have, Electricity required to produce $40...
of 
to ? of 
to 
? of 
to 
?Solution: As we know that, 1 mole of electron has a charge of 1 faraday (i) $A l^{3+}+3 e^{-} \rightarrow A l$Required charge $=3 F$$=3 \times 96487 C$$=289461 C$(ii) $C u^{2+}+2 e^{-} \rightarrow C...
acetic acid is 
. Calculate its molar conductivity. If 
for acetic acid is 
, what is its dissociation constant?Solution: Given, $K =7.896 \times 10^{-5} S m ^{-1} c$ $$=0.00241 mol L ^{-1}$$As we know, molar conductivity, $\Lambda_{m}=\frac{k}{c}$ Substituting the value of known parameters we...
Solution: Evaluating the value of Λm for each case, Given,$$K =1.237 \times 10^{-2} S m -1, c =0.001 M$$Then, $K =1.237 \times 10^{-4} S cm ^{-1}, c ^{1 / 2}=0.0316 M ^{1 /...
Solution: Given,Conductivity, $k =0.146 \times 10^{-3} S cm -1$Resistance, $R =1500 \Omega$Concept : We know the formula is, $$ \text { Cell constant }= k \times R$$ Calculation: Substuting the...
. Calculate its molar conductivity.Solution: Given, $K =0.0248 S cm ^{-1} C$$$c =0.20 M$$ Concept: We know that Molar conductivity, $\Lambda_{m}=\frac{k \times 1000}{c}$ Calculation: Substituting the value of known parameter,...
Solution: Conductivity: The conductivity of a solution is defined as the conductance of a solution with a length of 1 cm and an area of cross-section of 1 sq. cm and a cross-sectional area of 1 sq....
Solution: Given, $E_0 = 1.104 V$ We know that, $$\Delta_{r} G^{\Theta}=-n F E^{\Theta}$$ Thus substituting the value of parmeters. = −2 × 96487 × 1.04 = −213043.296 J = −213.04...
Solution: Nernst equation in electrochemistry is a relationship between the reduction potential of a reaction (either a half-cell or full-cell reaction) and various parameters such as the standard...
Solution: Nernst equation in electrochemistry is a relationship between the reduction potential of a reaction (either a half-cell or full-cell reaction) and various parameters such as the standard...
Solution: (i) Given: $E_{C r^{3+} / C r}^{\Theta}=0.74 V$ $$E_{C d^{2+} / C d}^{\Theta}=-0.40 V$$The galvanic cell of the given reaction is represented as :$$C r_{(s)}\left|C r_{(a q)}^{3+} | C d_{a...
takes place. Further show: (i) Which of the electrode is negatively charged? (ii) The carriers of the current in the cell. (iii) Individual reaction at each electrode.Solution: It is an electrochemical cell named after the inventors Luigi Galvani and Alessandro Volta, respectively, in which an electric current is generated through spontaneous reactions. The...
Solution: As the reduction potential is reduced, the reducing power increases proportionally. The following are the standard electrode potentials in ascending order (increasing order): K+/K <...
Solution: According to their reactivity, the following metals replaces in the following order: magnesium, aluminum, zinc, iron, and copper. Magnesium > Aluminum > Zinc > Copper