Describe the chemical reaction based on the chemical equation below. Also, explain whether the equation is balanced.

NH3(g) + O2(g) > NO(g) + H2O(I)

what is the explanation?

The balanced equation is: 4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(I)

4 moles of ammonia need 5 moles of oxygen to react, in order to produce 6 moles of water and 4 moles of nitrogen oxide.

Explanation:

NH₃(g) + O₂(g) → NO(g) + H₂O(I)

That is the unbalanced equation.

Ratio is 1:1, so 1 mol of ammonia and 1 mol of oxygen may react to produce 1 mol of NO and 1 mol of water

First of all we need to balance. Let's count the atoms:

In reagent side, we have 3 H and in product side there are 2H, we can add a 3, so now we have 6 H. Therefore, the reagent side must have 2 in front of the ammonia. In both sides we have 6 H

Now, that we added a 2 in the ammonia, we have 2N, so we have to add 2 to NO in the product side.

Let's count the oxygen in the product side, 5. We must add 5/2 in the reactant side. But chemical equations usually do not have rational numbers, that's why we multiply x2, all the stoichiometry.

The balanced equation is: 4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(I)

4 moles of ammonia need 5 moles of oxygen to react, in order to produce 6 moles of water and 4 moles of nitrogen oxide.

4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(I)

We need 4 moles of ammonia gas (NH3) and 5 moles of oxygen gas( O2) to produce 4 moles of nitromonoxide gas (NO) and 6 moles of water (H2O)

Explanation:

Step 1: The unabalnced equation

NH3(g) + O2(g)→ NO(g) + H2O(I)

Step 2: Balancing the equation

NH3(g) + O2(g) → NO(g) + H2O(I)

On the left side we have 3x H (in NH3), on the right side we have 2x H (in H2O)

To balance the amount of H, on both sides, we have to multiply NH3 by 4 and H2O by 6

4NH3(g) + O2(g) → NO(g) + 6H2O(I)

We have 4x N on the left side (in 4NH3) and 1x N in NO on the right side. To balance the amount of N on both sides, we have to multiply NO on the right side by 4

4NH3(g) + O2(g) → 4NO(g) + 6H2O(I)

On the left side we have 2x O (in O2, on the right side we have 10x O (4x in 4NO and 6x in 6H2O). To balance the amount of O we have to multply O2 by 5. Now the equation is balanced.

4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(I)

Step 3: Explanation

This means we need 4 moles of ammonia gas (NH3) and 5 moles of oxygen gas( O2) to produce 4 moles of nitromonoxide gas (NO) and 6 moles of water (H2O)

i think it's c. if you look search electronic symbol on google and then click on wiki it shows you a

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.