Identify the oxidizing agent in the reaction: sn(s) + 2h+(aq) → sn2+(aq) + h2(g) sn2+ h2 h+ sn

H⁺(aq)

Explanation:

Let's consider the following redox reaction.

Sn(s) + 2 H⁺(aq) → Sn²⁺(aq) + H₂(g)

We can identify both half-reactions.

Oxidation: Sn(s) → Sn²⁺(aq) + 2 e⁻

Reduction: 2 H⁺(aq) + 2 e⁻ → H₂(g)

Sn(s) undergoes oxidation so it is the reducing agent, while H⁺(aq) undergoes reduction so it is the oxidizing agent.

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.

they it depends on if one believes about radioactivity, they make a geiger counter beep but maybe it was going to beep anyway electronics do wierd things all the time or it was programmed to beep near certain metals.