Which one of the following is not a redox reaction?

A. H2O(l) + NH3(g) → NH4+(aq) + OH¯(aq)
B. 2H2(g) + O2(g) → 2H2O(l)
C. Cl2(g) + 2KBr(aq) → Br2(l) + 2KCl(aq)
D. 6FeSO4(aq) + K2Cr2O7(aq)+ 7H2SO4(aq) → Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq)+ K2SO4(aq) + 7H2O(l)
E. Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)

I think it's A, but I'm not certain. Please answer ASAP, thx in advance

It was A :DDD, but I missed a question on spectator ions.

Sure thing! Well, A redox reaction involves the transfer of electrons between species. So, let's analyze the options here.

A. H2O(l) + NH3(g) → NH4+(aq) + OH¯(aq) - This reaction involves the transfer of a proton (H+) but not electrons, so it does not qualify as a redox reaction.

B. 2H2(g) + O2(g) → 2H2O(l) - This is a classic example of a redox reaction, where hydrogen is oxidized and oxygen is reduced.

C. Cl2(g) + 2KBr(aq) → Br2(l) + 2KCl(aq) - In this reaction, chlorine (Cl2) is reduced from 0 to -1, while bromine (Br2) is oxidized from -1 to 0.

D. 6FeSO4(aq) + K2Cr2O7(aq) + 7H2SO4(aq) → Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq) + K2SO4(aq) + 7H2O(l) - This equation involves the transfer of electrons, making it a redox reaction.

E. Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) - This is another redox reaction, where zinc (Zn) is oxidized, and hydrogen (H2) is reduced.

So, the answer is indeed A. It is not a redox reaction. Hope this helps, and don't hesitate to ask if you have any more questions!

To determine which one of the following is not a redox reaction, we need to identify if there is a transfer of electrons between the reactants.

A. H2O(l) + NH3(g) → NH4+(aq) + OH¯(aq)
In this reaction, the oxidation state of each element does not change. Therefore, it is not a redox reaction.

B. 2H2(g) + O2(g) → 2H2O(l)
In this reaction, hydrogen (H2) is oxidized to form water (H2O), while oxygen (O2) is reduced to form water (H2O). This is a redox reaction.

C. Cl2(g) + 2KBr(aq) → Br2(l) + 2KCl(aq)
In this reaction, chlorine (Cl2) is reduced to form bromine (Br2), while bromide ions (Br¯) are oxidized to form chloride ions (Cl¯). This is a redox reaction.

D. 6FeSO4(aq) + K2Cr2O7(aq)+ 7H2SO4(aq) → Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq)+ K2SO4(aq) + 7H2O(l)
In this reaction, iron (Fe) is oxidized, and chromium (Cr) is reduced. This is a redox reaction.

E. Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)
In this reaction, zinc (Zn) is oxidized, and hydrogen (H2) is reduced. This is a redox reaction.

Therefore, the answer is A. H2O(l) + NH3(g) → NH4+(aq) + OH¯(aq) is not a redox reaction.

To determine which one of the given reactions is not a redox reaction, we need to understand what a redox reaction is.

A redox reaction, also known as an oxidation-reduction reaction, involves the transfer of electrons between reactants. In other words, there is a change in the oxidation state of one or more elements involved in the reaction.

To identify whether a reaction is a redox reaction, we need to examine the oxidation states of the elements in the reactants and the products.

Now, let's analyze each given reaction to determine if there is a change in oxidation state:

A. H2O(l) + NH3(g) → NH4+(aq) + OH¯(aq)
In this reaction, there is no change in the oxidation state of any element. Oxygen (O) has a -2 oxidation state both in the reactants and the products, and hydrogen (H) has a +1 oxidation state in all species. Therefore, reaction A is not a redox reaction.

B. 2H2(g) + O2(g) → 2H2O(l)
In this reaction, the oxidation state of oxygen changes from 0 in O2 to -2 in H2O. Therefore, reaction B is a redox reaction.

C. Cl2(g) + 2KBr(aq) → Br2(l) + 2KCl(aq)
In this reaction, the oxidation state of chlorine (Cl) changes from 0 in Cl2 to -1 in KCl, while the oxidation state of bromine (Br) changes from -1 in KBr to 0 in Br2. Therefore, reaction C is a redox reaction.

D. 6FeSO4(aq) + K2Cr2O7(aq) + 7H2SO4(aq) → Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq) + K2SO4(aq) + 7H2O(l)
In this reaction, the oxidation state of chromium (Cr) changes from +6 in K2Cr2O7 to +3 in Cr2(SO4)3. Iron (Fe) also undergoes a change in oxidation state from +2 in FeSO4 to +3 in Fe2(SO4)3. Therefore, reaction D is a redox reaction.

E. Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)
In this reaction, the oxidation state of zinc (Zn) changes from 0 in Zn(s) to +2 in ZnSO4. Therefore, reaction E is a redox reaction.

Based on our analysis, the only reaction that is not a redox reaction is A.