Questions in electrochemistry

Select	Question
	During electrolysis of a solution of $AgN{{O}_{3}}$, 9650 Coulombs of charge pass through the electroplating bath, the mass of silver deposited in the cathode will be
	On passing 0.1 Faraday of electricity through aluminium chloride, the amount of aluminium metal deposited on cathode is ($Al = 27$)
	One litre of 1 M $CuSO_4$ solution is electrolysed. After passing $2F$ of electricity, molarity of $CuSO_4$ solution will be
	For ${{M}^{2+}}+2{{e}^{-}}\to M,$ 0.275 g of metal M is deposited at the cathode due to passage of 1 A of current for 965 s. Hence atomic weight of the metal $M$ is
	A certain current liberated 0.504 gm of hydrogen in 2 hours. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution
	What weight of copper will be deposited by passing 2 Faradays of electricity through a cupric salt (Atomic weight of $Cu = 63.5$)
	The quantity of electricity required to liberate $112 cm^3$ of hydrogen at STP from acidified water is
	How much charge is required to produce hydrogen gas at the rate of $1 mL s^{–1}$ by the electrolysis of molten $NaCl$
	In the electrolysis of aqueous $NaCl$ for how long would you have to pass a current of 1.0 A through the cell to convert 1.0 L of a 1 M $NaCl$ solution into 1 M of $NaOH$
	The number of electrons gained and lost during the electrolysis of $35.5 g$ of $Cl^–$ and $65.4 g$ of $Zn^{2+}$ respectively are