UGRENT! Please help showing all work

a. Oxygen

b. 2.62 g of NO

c. 85.2%

Explanation:

Let's see the presented reaction:

4NH₃ + 5O₂  →  4NO  +  6H₂O

4 moles of ammonia react to 5 moles of oyxgen in order to produce 4 moles of NO and 6 moles of water.

To determine limting reagent, we need moles of each reactant. Let's calculate them:

3.25 g /17 g/mol = 0.191 moles

3.50 g /32 g/mol = 0.109 moles

4 moles of amonia react to 5 moles of oxygen

Then, 0.191 moles will react to (0.191 . 5) / 4 = 0.238 moles

We only have 0.109 moles available and we need 0.238, so the oxygen is the limting reactant.

5 moles of O₂ can produce 4 moles of NO

So, our 0.109 moles will produce (0.109 . 4) /5 = 0.0872 moles

We convert the moles to mass: 0.0872mol . 30g/mol = 2.62g

(Yield produced / Theoretical yield)  . 100 = %

(2.23g / 2.62g) . 100 = 85.2%

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error