Given the redox reaction in an electrochemical cell:

Ni(s) + Pb2+(aq) + Ni2+(aq) + Pb(s)

A salt bridge is used to connect

A) Ni(s) and Pb(s)

B) Pb2+(aq) and Ni2+(aq)

C) Ni(s) and Ni2+(aq)

D) Pb2+(aq) and Pb(s)

Please help me

Pb2+(aq) and Ni2+ B

Explanation:A salt bridge is a laboratory device used in an electrochemical cell  to connect the oxidation ( which occurs at the anode ) and reduction( which occurs at the cathode) half-cells of a galvanic cell voltaic cell, It prevents the cell from quickly  reaching equilibrium  by maintaining  electrical charge  neutrality within the internal circuit because the electrons are moving from one-half cell to the other.

In this electrochemical cell,  Ni (s) is oxidized to Ni2+(aq) and will occurs at the anode while  Pb2+(aq) is reduced to Pb (s) and will occur at the  cathode.

the grams   of   barium that   are in   2.3 x 10^23   atoms of barium   is   52.4 g (answer c)

    calculation

mass = moles   of ba   x molar   mass of ba

  molar mass of ba from periodic table=   137.3 g/mol

  use the   avogadro's law   constant   to   calculate the moles of barium

  that   is     1 mole =   6.02   x 10^23 atoms

                    ? moles = 2.3 x 10^23   atoms

by cross   multiplication

=(1 mole   x 2.3x 10^23 atoms)   / 6.02   x10^23 atoms)=   0.382   moles

mass   is therefore = 137.3   g/mol x 0.382 mol = 52.4 ( answer c)

explanation: