The reaction below is spontaneous under standard conditions - true or false? br2(l) + mn2+(aq) → mno4-(aq) + br-(g) (in acidic solution) use the fact that the reduction potential for mno4-(aq) is +1.51 v and for br2(l) it is +1.065 v.

Question

contestada

Respuesta :

okpalawalter8 okpalawalter8 · Answer 1 · 2020-04-22T04:13:53+02:00

Answer:

The answer is false

Explanation:

The given reaction is

[tex]Br_{2}_{(l)} + Mn^{2+}_{(aq)} ------->MnO_4 _{(aq)} + Br^-_{(g)}[/tex]

At the cathod the potential is

[tex]E_{cath} = + 1.065V[/tex] [This because it will attract the negative

charge]

At the Anode the potential is

[tex]E_{anode} = 1.51[/tex]

The overall potential of the cell is

[tex]E_{cell} = E_{cath} - E_{anode}[/tex]

[tex]= -0.445[/tex]

Since the potential of the cell is less than 0 then the reaction is not spontenous under standard condition

andromache andromache · Answer 2 · 2022-04-12T16:24:38+02:00

The reaction below is spontaneous under standard conditions should be considered false.

Since the given reaction is br2(l) + mn2+(aq) → mno4-(aq) + br-(g)

Also, at the anode, the potential should be

Eanode = 1.51

And, the overall potential of the cell is

= -0.445

Also, the potential of the cell should be lower than 0 so the reaction is not spontenous under standard condition

learn more about reaction here: https://brainly.com/question/1542697