Electrochemistry

Step 1: Understanding the equation for electrolysis.
The mass of the copper deposited is given by the formula: where: - is the molar mass of copper (63.5 g/mol), - is the current (2.5 A), - is the time (193 s), - is the number of electrons involved in the reaction (2 for copper), - is the Faraday constant (96500 C/mol). Step 2: Substituting values.
Substituting the values: Step 3: Conclusion.
The amount of copper deposited is g. The correct answer is (1) 1.5875 g.

Step 1: Understanding molar conductivity.
The molar conductivity at infinite dilution is the sum of the individual conductivities of the ions formed in the solution. For weak electrolytes like acetic acid, we can use the relationship between the conductivities of HCl, NaCl, and acetic acid.
Step 2: Applying the relationship.
Using the known conductivities for HCl, NaCl, and acetic acid, and knowing the ionization of acetic acid, we can estimate its molar conductivity. We use the weighted sum based on known molar conductivities and ionization constants. Step 3: Conclusion.
The for acetic acid is calculated to be approximately S cm . The correct answer is (3) 461 S cm .

Step 1: Understanding the formula for emf.
The emf of the galvanic cell is given by: Here, the cathode is copper ( ) and the anode is zinc ( ). Step 2: Substituting the given values.
Step 3: Conclusion.
The emf of the galvanic cell is . The correct answer is (1) 1.13 V.