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 ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.