Among the following, which is an oxidation-reduction reaction?
A. Na2S + CaCO3 → CaS + Na2CO3
B. 2HNO3 + Mg(OH)2 → Mg(NO3)2 + 2H2O
C. H2 + F2 → 2HF****
D. 3Ba(OH)2 + 2H3PO4 → Ba3(PO4)2 + 6H2O
right. You may want to look at the iron question below. I don't think B is right.
DrBob222 I did see it, I answered to your comment, please see what I wrote :) and thank you for your help :)
3. Na2S in Oxidation-reduction reactions can be …:
A) reducing agents only
B) oxidizing agents only
C) both reducing and oxidizing agents
D) metals don’t have Oxidation-reduction properties
To determine which of the given reactions is an oxidation-reduction reaction, we need to identify if there is a transfer of electrons between the reactants.
In an oxidation-reduction reaction, also known as a redox reaction, one species (atom, ion, or molecule) loses electrons (undergoes oxidation), while another species gains electrons (undergoes reduction).
Let's analyze the given reactions:
A. Na2S + CaCO3 → CaS + Na2CO3
B. 2HNO3 + Mg(OH)2 → Mg(NO3)2 + 2H2O
C. H2 + F2 → 2HF
D. 3Ba(OH)2 + 2H3PO4 → Ba3(PO4)2 + 6H2O
In reaction A, there is no change in oxidation states for the elements involved. Therefore, it is not an oxidation-reduction reaction.
In reaction B, nitrogen in HNO3 increases its oxidation state from +5 to +6, while magnesium in Mg(OH)2 decreases its oxidation state from +2 to 0. This indicates a transfer of electrons, making it an oxidation-reduction reaction.
In reaction C, hydrogen in H2 goes from an oxidation state of 0 to +1 in HF, while fluorine in F2 goes from 0 to -1. This also indicates a transfer of electrons, making it an oxidation-reduction reaction.
In reaction D, there is no change in oxidation states for the elements involved. Therefore, it is not an oxidation-reduction reaction.
Based on this analysis, the oxidation-reduction reactions are option B (2HNO3 + Mg(OH)2 → Mg(NO3)2 + 2H2O) and option C (H2 + F2 → 2HF).