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कर्नाटक बोर्ड पी.यू.सी.पीयूसी विज्ञान 2nd PUC Class 12

Match the terms given in Column I with the units given in Column II. Column I Column II (i) Λm (a) S cm-¹ (ii) ECell (b) m-¹ (iii) K (c) S cm2 mol-¹ (iv) G* (d) V - Chemistry

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प्रश्न

Match the terms given in Column I with the units given in Column II.

Column I Column II
(i) Λm (a) S cm-¹
(ii) ECell (b) m-¹
(iii) K (c) S cm2 mol-¹
(iv) G* (d) V
जोड्या लावा/जोड्या जुळवा
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उत्तर

Column I Column II
(i) Λm (c) S cm2 mol-¹
(ii) ECell (d) V
(iii) K (a) S cm-¹
(iv) G* (b) m-¹
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पाठ 3: Electrochemistry - Exercises [पृष्ठ ४०]

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एनसीईआरटी एक्झांप्लर Chemistry [English] Class 12
पाठ 3 Electrochemistry
Exercises | Q IV. 50. | पृष्ठ ४०

संबंधित प्रश्‍न

Among Zn and Cu, which would occur more readily in nature as metal and which as an ion?


How many faradays of electricity are required to produce 6 g of Mg from MgCl2?


How many moles of electrons are required for reduction of 2 moles of Zn2+ to Zn?


How many faradays of electricity are required for the following reaction to occur

\[\ce{MnO^-_4 -> Mn^2+}\]


Consider the change in the oxidation state of Bromine corresponding to different emf values as shown in the expression below:

\[\ce{BrO^-_4 ->[1.82 V] BrO^-_3 ->[1.5 V] HBrO ->[1.595 V] Br2 ->[1.0652 V] Br^-}\]

Then the species undergoing disproportionation is:


Define cathode


Two metals M1 and M2 have reduction potential values of −xV and +yV respectively. Which will liberate H2 and H2SO4.


Write a note on sacrificial protection.


Use the data given in below find out the most stable oxidised species.

`E^0 (Cr_2O_1^(2-))/(Cr_(3+))` = 1.33 V   `E^0 (Cl_2)/(Cl^-)` = 1.36 V

`E^0 (MnO_4^-)/(MN^(2+))` = 1.51 V   `E^0 (Cr^(3+))/(Cr)` = – 0.74 V


A galvanic cell has electrical potential of 1.1V. If an opposing potential of 1.1V is applied to this cell, what will happen to the cell reaction and current flowing through the cell?


Match the items of Column I and Column II.

Column I Column II
(i) K (a) I × t
(ii) Λm (b) `Λ_m/Λ_m^0`
(iii) α (c) `K/c`
(iv) Q (d) `G^∗/R`

Calculate the standard EMF ofa cell which involves the following cell reactions

\[\ce{Zn + 2 Ag+ -> Zn^{2+} + 2 Ag}\]

Given that \[\ce{E^{o}_{Zn/Zn^{2+}}}\] = 0.76 volt and \[\ce{E^{o}_{Ag/Ag^{+}}}\] = – 0.80 volt.


If the half-cell reaction A + e → A has a large negative reduction potential, it follow that:-


In a Daniel cell, ______.


In a solution of CuSO4, how much time will be required to precipitate 2 g copper by 0.5 ampere current?


The two half cell reaction of an electrochemical cell is given as 

\[\ce{Ag+ + e- -> Ag}\], `"E"_("Ag"^+//"Ag")^circ` = - 0.3995 V

\[\ce{Fe^{2+} -> Fe^{3+} + e-}\], `"E"_("Fe"^{3+}//"Fe")^{2+}` = - 0.7120 V

The value of EMF will be ______.


What should be the signs (positive/negative) for \[\ce{E^0_{cell}}\] and ΔG0 for a spontaneous redox reaction occurring under standard conditions?


Can we construct an electrochemical cell with two half-cells composed of ZnSO4 solution and zinc electrodes? Explain your answer.


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