I'm having a hard time with Redox and how to figure out which is redox
Select all of the reactions that are redox reactions.
I) Ca + 2H2O Ca(OH)2 + H2
II) CaO + H2O Ca(OH)2
III) Ca(OH)2 + H3PO4 Ca3(PO4)2 + H2O
IV) Cl2 + 2 KBr Br2 + 2 KCl
I and II
II and III
I and IV
III and IV
What is the oxidizing agent in the following reaction?
Zn(s) + NO31-(aq) Zn(OH)42-(aq) + NH3(aq)
Zn(s)
NO31-(aq)
Zn(OH)42-(aq)
NH3(aq)
And no this isnt homework just "practice probs" and no answer...i don't know how to do them or understand them thanx
To determine if a reaction is a redox reaction, you need to identify the changes in oxidation states of the elements involved.
In a redox reaction, there is a transfer of electrons between species, resulting in a change in their oxidation states. The species that loses electrons is oxidized and considered the reducing agent, while the species that gains electrons is reduced and considered the oxidizing agent.
Let's analyze each reaction to identify if it is a redox reaction:
I) Ca + 2H2O → Ca(OH)2 + H2
In this reaction, the oxidation state of Ca stays the same throughout the reaction. H2O is being reduced to H2 by gaining electrons. Therefore, this is a redox reaction.
II) CaO + H2O → Ca(OH)2
In this reaction, the oxidation state of Ca remains the same, while the oxidation state of O in CaO decreases from +2 to -2 when forming Ca(OH)2. However, there is no transfer of electrons between species. Thus, this is not a redox reaction.
III) Ca(OH)2 + H3PO4 → Ca3(PO4)2 + H2O
In this reaction, the oxidation states of Ca and P remain the same throughout the reaction. The oxidation states of H and O change, but there is no transfer of electrons between species. Therefore, this is not a redox reaction.
IV) Cl2 + 2 KBr → Br2 + 2 KCl
In this reaction, Cl2 is reduced to Br2 by gaining electrons. K in KBr does not change its oxidation state, and Br2 is formed. Hence, this is a redox reaction.
Based on the analysis, the redox reactions are I) and IV). Therefore, the correct answer is "I and IV."
Next, let's determine the oxidizing agent in the given reaction:
Zn(s) + NO31-(aq) → Zn(OH)42-(aq) + NH3(aq)
The oxidizing agent is the species that gets reduced and causes another species to be oxidized. In this reaction, NO31-(aq) is reduced, and Zn(s) is oxidized. Therefore, the oxidizing agent is NO31-(aq).
I hope this explanation helps you understand redox reactions better. If you have any further questions, feel free to ask!