ok.. im confused:
Ammonia and oxygen react in the equation: 4NH³+5O²--> 4NO+6H²O. When 2.4 mol of NH³ are present, the reaction yields ____ mol of O².
i have no clue how ot do this!
Look at your problem to make sure it is posted correctly. NH3 REACTS with O2; it doesn't yield O2.
thats exactly what it says on my homework
That may be why you are confused. I'm sure the problem was meant to ask for number of mols O2 USED when 2.4 mols NH3 are consumed.
Of course, if the problem is stated correctly, then the answer is that the reaction produces zero mols O2.
ok- Thanks!
You're welcome! I apologize for the confusion. In the given chemical equation, 4NH3 + 5O2 → 4NO + 6H2O, ammonia (NH3) and oxygen (O2) react to produce nitric oxide (NO) and water (H2O). To determine the number of moles of O2 produced or consumed in the reaction, we need to use stoichiometry.
Stoichiometry is a calculation process that allows us to determine the relationship between the amounts of reactants and products in a chemical reaction. In this case, we want to find the number of moles of O2 when a certain amount of NH3 is present.
Step 1: Convert the given amount of NH3 to moles.
Given: 2.4 mol NH3
Step 2: Use the mole ratio from the balanced equation to find the moles of O2.
From the balanced equation, we can see that the ratio between NH3 and O2 is 4:5. This means that for every 4 moles of NH3 consumed, 5 moles of O2 are consumed/produced. Therefore, we can set up the following proportion:
4 moles NH3 / 5 moles O2 = 2.4 moles NH3 / x moles O2
Cross-multiplying, we get:
4 moles NH3 * x moles O2 = 2.4 moles NH3 * 5 moles O2
Simplifying, we have:
4x = 12
Dividing both sides by 4, we find:
x = 3
Therefore, when 2.4 moles of NH3 are present, the reaction yields 3 moles of O2.
However, it seems that there might be an error in the given problem. NH3 and O2 react to produce NO and H2O, not O2. Therefore, if the problem is stated correctly, the answer would be 0 moles of O2 produced. It may be worth double-checking with your teacher or textbook to confirm the accuracy of the problem.