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.

Best reards.

the answer to your question is c.

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given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g