Predict whether a spontaneous redox reaction will occur if a nickel (2) nitrate solution is with a tin(2) sulfate solution. Support your answer with a half reaction equations and balanced redox equation.
To determine whether a spontaneous redox reaction will occur when a nickel (2) nitrate solution is mixed with a tin (2) sulfate solution, we need to compare the reduction potentials of the two reactants.
First, let's write the half-reaction equations for the reduction of Nickel (Ni) and Tin (Sn):
Ni2+(aq) + 2e- -> Ni(s)
Sn2+(aq) + 2e- -> Sn(s)
The reduction potential for Nickel can be found in a standard reduction potential table and is +0.25 V. The reduction potential for Tin is also positive, but its exact value is not necessary for this analysis.
Now, let's compare the reduction potentials. If the reduction potential for the species being reduced (the one gaining electrons) is more positive than the reduction potential for the species being oxidized (the one losing electrons), then the reaction is spontaneous.
In this case, the reduction potential of nickel (+0.25 V) is more positive than the reduction potential of tin, so we can predict that a spontaneous redox reaction will occur.
To write the balanced redox equation, we need to multiply the half-reactions by appropriate coefficients so that the number of electrons gained and lost is the same:
2Ni2+(aq) + 2e- -> 2Ni(s) (multiply the reduction half-reaction by 2 to balance the electrons)
Sn2+(aq) + 2e- -> Sn(s) (no need to balance this half-reaction)
Now, combining these two half-reactions gives us the balanced redox equation:
2Ni2+(aq) + Sn(s) -> 2Ni(s) + Sn2+(aq)
Thus, when a nickel (2) nitrate solution is mixed with a tin (2) sulfate solution, a spontaneous redox reaction will occur.