Question

What element is being oxidized in the following redox reaction? Sn 2+(aq) + NH4 +(aq) → Sn(s) + NO3 -(aq)

Answer 1

Answer:

Nitrogen

Explanation:

Hello,

In this case, for the given reaction we first need to assign the oxidation state for each species in the chemical reaction:

$Sn ^{2+}(aq) + (N^{-3}H^+_4)^ +(aq) \rightarrow Sn^0(s) + (N^{5+}O_3^{2-})^ -(aq)$

In such a way, since the tin is decreasing its oxidation state it is being reduced whereas the nitrogen is being oxidized as its oxidation state is being increased from -3 to +5.

Best regards.

Answer 2

The element which is oxidized in the redox reaction shown below is Nitrogen.

Sn²⁺(aq) + NH⁴⁺(aq) → Sn(s) + NO₃⁻(aq)

In this scenario, the oxidation state of Sn changed from +2 to 0 while the

oxidation state of Nitrogen changed from -3 to +5.  The Nitrogen(N) present

in the equation experienced an increase in the oxidation state which means

it was oxidized.

The Tin(Sn) on the other hand experienced a reduction in the oxidation state

which means it was reduced.

Read more on https://brainly.com/question/25544428