Which equations represents a redox reaction

In this case, you can apply that rule to the equation of the choice number 3. In that, you can see that Cu is pure which as per the mentioned rule means that its oxidation state is 0. As Cu is combined with O, CuO, in the reactant side of the chemical equation, then its oxidation number is not 0. Of course other atoms had to be oxidized. Answer : The correct option is, D. This reaction is a double displacement reaction in which the cation and anion of two reactants are exchange their places to give two different products.

This reaction is a decomposition reaction in which the larger molecule decomposes to give two or more products. This reaction is a neutralization reaction in which an acid and a base react to give a salt and water as a product.

This reaction is a redox reaction in which the oxidation and reduction reaction occur simultaneously. Oxidation reaction is the reaction in which a substance looses its electrons. In this oxidation state increases. Reduction reaction is the reaction in which a substance gains electrons. In this oxidation state decreases. Your email address will not be published. Save my name, email, and website in this browser for the next time I comment.

For that to occur, carbon needs to be plus four and then for water. We've got minus two and plus one. If we look closely, there is no change in oxidation state of any element because there's no change in oxidation state of any element. This is not a redox reaction. The next one we have potassium nitrate going to potassium nitrite and oxygen will assign oxidation. States, oxygen is minus two. Potassium is plus one Nitrogen is going to be the minus two, multiplied by three is minus six plus one.

So what's left would be plus five in order to get this to be somewhat to zero. Then when we go over to potassium nitrite, got minus two on oxygen plus one on potassium, so that gives us minus four and a plus one. So this needs to be plus three and oxygen elements by themselves in their elemental form, have an oxidation state of zero. So we now see that nitrogen went from plus five two plus three, so it was reduced and oxygen went from minus 2 to 0, so it was increased.

It was oxidized. The potassium nitrate is serving as both the oxidizing and the reducing agent. Normally, when we defined the agent, it's the entire compound. However, some teachers might suggest that the agent is going to be the element within the compound.

But it's more correctly to describe the agent as an actual chemical. That is, that is part of the chemical reaction. So we would say that potassium nitrate is serving both as theocracy izing and the reducing agent. This is often this often occurs with many redox reactions.

The next reaction is hydrogen gas, with copper to oxide going to copper metal on water. Hydrogen gas is an element by itself, so it has an oxidation state of zero. Oxygen has a minus two charge, so it has a minus two oxidation state and copper as a plus to charge, so it has a plus to oxidation state copper by itself.

Here is zero, and then the water oxygen's minus two and hydrogen is plus one, so we see that hydrogen has a change in oxidation state of zero to plus one. So it increased. So it was oxidized and copper goes from plus 2 to 0. So it decreased, so it was reduced. So we would say that hydrogen gas is the reducing agent, and copper to oxide is the oxidizing agent. For the next one, we have sodium hydroxide reacting with hydrochloric acid producing sodium chloride and water sodium has a plus one charge.

So it has a plus one oxidation state hydroxide. Oxygen hydroxide is minus two. The hydrogen is plus one. They all some up to zero. Hydrogen is gonna be plus one. So to sum, up to zero chloride needs to be minus one.

So dems plus one because that's his charge. Chlorides minus one because that's its charge. And then hydrogen and hydrogen typically being plus one and oxygen typically being minus two. We look closely. We see that there is no change in oxidation state of any element present. So this is not a redox reaction. The next one is hydrogen gas with chloride gas going to hydrogen chloride. Hydrogen by itself as an element in its pure form, has an oxidation state of zero chlorine gas, an element by itself has an oxidation state of zero.

But when we form hydrogen chloride, hydrogen with plus one and chloride will be minus one similar to what we had up here. We do see a change in oxidation state are hydrogen goes from zero to plus one. So it was oxidized and chlorine goes from zero to minus one. Which element is oxidized? Not a redox reaction.

Which equations shows an oxidation reaction? What are the oxidation numbers for NH 4 Cl. What element is being reduced? Which element is being oxidized in the following chemical reaction? Which element is reduced in the following reaction? What are the oxidation numbers of elements in sulfuric acid, H 2 SO 4?

What are the oxidation numbers of elements in phosphoric acid, H 3 PO 4? What is oxidation number of O in O 2?