NH3(g) + 202(g) = HNO3(aq) +H2O (l)

Is this reaction a combination, decomposition, single replacement, double replacment or other?

Also is it redox or non redox?

Its a redox reaction.

Is it also an "other" reaction because it is a dehydration reaction?

It may be "other" but surely not "dehydration." I don't see a loss of water anywhere. It might be "dehydrogenation" since we are dehydrogenating NH3.

Thanks. I am trying to figure out if it is an "other" reaction or double replacement. But, I just don't see the double replacement in it???

For what it's worth, I learned the types of chemical reactions as:

1. synthesis or combination reactions in which two or ore substances produce a single substance. A + B ==> AB

2. single replacement
A + BX ==> AX + B

3. double replacement.
AX + BY ==> AY + BX

4. Combustion reactions.
X + O2 ==> XO2

5. Decomposition.
AB ==> A + B

6. Redox reactions.
The reaction you posted is NOT
single replacement.
Not double replacement.
Not combustion.
Not decomposition.
is redox. I still don't know what falls under "other" in your classification but I would call redox "other."
http://chemistry.olivet.edu/classes/chem100/pdf/Labs/Kinds%20reac%20part%201%20Lab.pdf

Thank you so much. I wanted to make sure I was on the right track.

To determine the type of reaction, you can analyze the reactants and products and classify them based on their transformations.

In the given reaction: NH3(g) + 202(g) = HNO3(aq) +H2O(l)

This reaction involves the combination of two reactants, NH3(g) and O2(g), to produce two products, HNO3(aq) and H2O(l). Therefore, the reaction is a combination or synthesis reaction.

Regarding the redox or non-redox nature of the reaction, you need to determine if there is any change in the oxidation numbers of the elements involved.

First, let's identify the oxidation states of the elements in the reactants and products:
- In NH3, nitrogen (N) has an oxidation state of -3.
- In O2, oxygen (O) has an oxidation state of 0.
- In HNO3, nitrogen (N) has an oxidation state of +5, and oxygen (O) has an oxidation state of -2.
- In H2O, hydrogen (H) has an oxidation state of +1, and oxygen (O) has an oxidation state of -2.

By comparing the oxidation states of nitrogen and oxygen in the reactants and products, we can observe that the oxidation state of nitrogen has increased from -3 in NH3 to +5 in HNO3, and the oxidation state of oxygen has decreased from 0 in O2 to -2 in HNO3.

Since there is a change in the oxidation states of nitrogen and oxygen, this indicates that there has been a transfer of electrons, and the reaction is a redox (reduction-oxidation) reaction.