In a concentration cell the same reagents are present in both the anode and the cathode compartments , but at different concentrations. Calculate the emf of a cell of a cell containing 0.40 M. `Cr^(3+)` in one compartment and 1.0 M `Cr^(3+)` in the other if Cr electrodes are used in both.
A
0.028 V
B
0.249 V
C
0.083 V
D
0.125 V
Text Solution
Verified by Experts
The correct Answer is:
A
Topper's Solved these Questions
ELECTROCHEMISTRY
NARENDRA AWASTHI|Exercise Level 1 (Q.1 To Q.30)|1 Videos
ELECTROCHEMISTRY
NARENDRA AWASTHI|Exercise Level 1 (Q.91 To Q.120)|1 Videos
DILUTE SOLUTION
NARENDRA AWASTHI|Exercise Level 3 - Match The Column|1 Videos
In a first order reaction, the concentration of the reactant decrease from 0.6 M to 0.3 M in 15 min. The time taken for the concentration to change from 0.1 M to 0.025 M in minutes is
The rate constant of the reaction A to B is 0.6xx10^(-3) mole per second. If the concentration of A is 5 M, then concentration of B after 20 minutes is :
When 0.1M CH_(3)COOH solution is shaken with activated charcoal and the charcoal is filtered out, the concentration of acid -
For the reaction, R rarr P , the concentration of a reactant changes fro 0.03 M to 0.02 in 25 min. Calculate the average rate of reaction using units of time both in minutes an second.
The electrochemical cell shown below is a concentration cell. M|M^(2+) (saturated solution of a sparingly soluble salt, MX_2 || M^(2+) (0.001 mol dm^(-3) ) |M The emf of the cell depends on the difference in concentration of M^(2+) ions at the two electrode The emf of the cell at 298 is 0.059 V The value of DeltaG (kJ " mol"^(-1)) for the given cell is ( take 1F = 96500 C " mol"^(-1) )
The E^(@) at 25^(@)C for the following reaction at the indicated concentrations is 1.50 V . Calculate the DeltaG in kJ at 25^(@)C , Cr(s) + 3Ag^(+) (aq. 0.1 M)to Ag(s) + Cr^(3+) (aq. 0.1 M)
Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolyte cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly proportionation to the amount of charge passed through it. The mass of substance liberated at electrode is calculate using the following realation : m=(itE)/(96500) Here, E represent the equivalent mass and 96500 C is called the faraday constant. Faraday (96500 C) is the charge of 1 mole electron i.e., 6.023 xx 10^(23) electrons, it is used to liberate on gram equivalent of the substance. The passage of current liberates H_2 at cathode and Cl_2 at anode. The solution is
A tank with a square base of area 1.0 m^2 is divided by a vertical position in the middle. The bottom of the partition has a small hinged door of area 20 cm^2 The tank is filled with water in one compartment, and an acid (of relative density 1.7) in the other. both to the height of 4.0 cm compute the force necessary to keep the door close.
