What element is being oxidized in the following redox reaction? fe 2+(aq) + nh4 +(aq) → fe(s) + no3 -(aq)

Explanation:

When there occurs a decrease in oxidation state of an element then it means the element has been reduced.

Whereas when there occurs an increase in oxidation state of an element then it means the element has been oxidized.

As the given reaction is as follows.

Oxidation state of iron is changing from +2 to 0. It means iron is getting reduced.

On the other hand, oxidation state of N in is as follows.

                                  x + 4(1) = +1

                                    x = 1 - 4

                                        = -3

Hence, oxidation state of N in is -3.

Oxidation state of N in is as follows.

                              x + 3(-2) = -1

                              x - 6 = -1

                               x = +5

Hence, oxidation state of N in is +5. It means nitrogen is being oxidized.

Thus, we can conclude that nitrogen is the element which is being oxidized in the given reaction.

? you expect us to answer this? ? this is your schoolwork, i don't think we can with this, i think it would considering being

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.