Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: sundrops on January 25, 2005, 12:19:24 AM
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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?
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list out the possible equations and calculate their individual E-cell based on the electrode potential values given for each half-equation.
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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: