[sundrops]

Select the correct net-ionic equation from the list below.

a) Fe ^2+ (aq) oxidizes Mn (s)
b) Fe (s) reduces Ni ^2+ (aq)

then there is a list of equations.

My question is: In part a does that mean that the Mn is the reducing or oxidizing agent? I think the question is worded a little funny and I'm a tad confused.

From my understanding Fe oxidizes Mn so Fe takes electons from the Mn in part a, and in part b, the Fe gives electrons to the Ni - does that make sense?


In part b) for example here are some of the given equations:
i) Fe(s) + Ni^2+ (aq) --> Fe^2+ (aq) + Ni(s)
ii) Fe(s) + Ni^2+ (aq) + H2O(l) --> Fe^2+ (aq) + Ni(s) + H2(g) + 2OH- (aq)
iii) Ni(s) + Fe^2+ (aq) --> Ni^2+ (aq) + Fe (s)

How do I know which equation to choose? How do I figure it out?

[Donaldson Tan]

list out the possible equations and calculate their individual E-cell based on the electrode potential values given for each half-equation.

[pizza1512]

Select the correct net-ionic equation from the list below.

a) Fe ^2+ (aq) oxidizes Mn (s)
b) Fe (s) reduces Ni ^2+ (aq)

then there is a list of equations.

My question is: In part a does that mean that the Mn is the reducing or oxidizing agent? I think the question is worded a little funny and I'm a tad confused.

From my understanding Fe oxidizes Mn so Fe takes electons from the Mn in part a, and in part b, the Fe gives electrons to the Ni - does that make sense?


In part b) for example here are some of the given equations:
i) Fe(s) + Ni^2+ (aq) --> Fe^2+ (aq) + Ni(s)
ii) Fe(s) + Ni^2+ (aq) + H2O(l) --> Fe^2+ (aq) + Ni(s) + H2(g) + 2OH- (aq)
iii) Ni(s) + Fe^2+ (aq) --> Ni^2+ (aq) + Fe (s)

How do I know which equation to choose? How do I figure it out?

Did you just copy your homework questions here?...

 :1eye: