Question

Consider the following balanced redox reaction (do not include state of matter in your answers):2CrO2−(aq) + 2H2O(l) + 6ClO−(aq) →2CrO42−(aq) + 3Cl2(g) + 4OH−(aq)(a) Which species is being oxidized? (b) Which species is being reduced? (c) Which species is the oxidizing agent? (d) Which species is the reducing agent? (e) From which species to which does electron transfer occur?

Answer 1

Answer:

Explanation:

Hello,

At first, it is necessary to establish the oxidation states for all the species involved in the reaction:

$2(Cr^{+3}O_2^{-2})^{-}(aq) + 2H_2^{+1}O^{-2}(l) + 6(Cl^{+1}O^{-2})^{-1}(aq) -->2(Cr^{+6}O_4^{-2})^{-2}(aq) + 3Cl_2^0(g) + 4(O^{-2}H^{+1})^-(aq)$

In such a way, we answer to the questions as follows:

(a) Oxidized species is the one that has an increase in its oxidation state, this is chromium which passes from +3 to +6.

(b) Reduced species is the one that has a decrease in its oxidation state, this is chlorine which passes from +1 to 0.

(c) Oxidizing agent is the same reduced species, this is chlorine as it removes electrons.

(d) Reducing agent is the same oxidized species, this is chromium as it gains electrons.

(e) Electron transfer occur from chlorine to chromium as chlorine removes electrons and chromium gains them.

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Answer 2

From the given redox reaction, the following can be concluded:

(a) The oxidized species is chromium whose oxidation number increases from +3 to +6.

(b) The reduced species is chlorine which changes from +1 to 0.

(c) The oxidizing agent is chlorine which has been reduced.

(d) The reducing agent is chromium which has been oxidized.

(e) Electron transfer occurs from chlorine to chromium.

Redox reactions

Redox reactions are reactions in which oxidation and reduction occur simultaneously and concurrently to the same extent.

Oxidation is a reaction in which the oxidation number increases due to electron loss.

Reduction is a reaction in which the oxidation number decreases dues to electron gain.

Oxidizing agents are reduced

Reducing agents are oxidized

From the given redox reaction:

• 2CrO2−(aq) + 2H2O(l) + 6ClO−(aq) →2CrO42−(aq) + 3Cl2(g) + 4OH−(aq)

(a) The oxidized species is chromium whose oxidation number increases from +3 to +6.

(b) The reduced species is chlorine which changes from +1 to 0.

(c) The Oxidizing agent is chlorine which has been reduced.

(d) The reducing agent is chromium which has been oxidized.

(e) Electron transfer occurs from chlorine to chromium.

Learn more about redox reactions, oxidizing and reducing agents at: https://brainly.com/question/7484765