Use tabulated standard electrode potentials to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 ∘c: 3pb2+(aq)+2cr(s)→3pb(s)+2cr3+(aq)(n ote that the equation is balanced.)

Answer : The standard cell potential of the reaction is, -1.46 V

Explanation :

The given balanced cell reaction is,  

Here, chromium (Cr) undergoes oxidation by loss of electrons and act as an anode. Lead (Pb) undergoes reduction by gain of electrons and thus act as cathode.

The standard values of cell potentials are:

Standard reduction potential of lead

Standard reduction potential of chromium

Now we have to calculate the standard cell potential for the following reaction.

Therefore, the standard cell potential of the reaction is, -1.46 V

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.