Identify the reduced substance, the oxidized substance, the reducing agent, and the oxidizing agent in the reaction of zinc with copper ions. Zn(s)+Cu2+(aq)⟶Zn2+(aq)+Cu(s) Which substance in the reaction gets reduced?

Zinc is the oxidized substance and therefore the reducing agent.

Copper is the reduced substance and therefore the oxidizing agent.

Explanation:

Hello.

In this case, since the following chemical reaction is a redox one because the oxidation states of the species there are changed, the first step is to assign the oxidation states for all the species there as shown below:

Since metallic zinc a copper are pure elements so they are not oxidized. Now, since zinc increases its oxidation state from 0 to +2, we infer zinc is the oxidized substance and therefore the reducing agent. Moreover, since copper decreases its oxidation state from +2 to 0, we infer copper is the reduced substance and therefore the oxidizing agent.

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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.

yes they ca   is ur ansswerrr