Can someone check my answers for me thank you. This is my 3rd time posting this one up...maybe its just not going through bc I don't see it on the current ?s.
4NH3 + 7O2 --> 4NO2 + 6H2O
1)How many grams of oxygen are necessary to produce 4.50 moles of NO2?
answer: 252 grams
2)How many molecules of water are produced when 2.25 moles of ammonia are completely reacted?
answer: 3.38 moles
I haven't seen any of this question before and I've checked from time to time today. At any rate, your answer to #1 is correct. Your answer to #2 is not. You have correctly given the answer in moles (to #2) BUT the question is how many molecules (and not moles). Remember 1 mol H2O will have 6.02 x 10^23 molecules; therefore, 3.376 mol H2O will have ?? molecules.
I made a typo. That's 3.375 mols and not 3.376. I usualy carry the extra places, then round at the end to prevent rounding errors.
So the answer to #2 would be...2.03x10^24 molecules?
yes
To calculate the answers to the given questions, we need to use the molar ratios from the balanced chemical equation provided.
1) The balanced equation is: 4NH3 + 7O2 → 4NO2 + 6H2O
To find how many grams of oxygen are necessary to produce 4.50 moles of NO2:
Step 1: Determine the molar ratio between NO2 and O2 from the balanced equation.
The coefficient of NO2 is 4, and the coefficient of O2 is 7. This means that for every 4 moles of NO2 produced, we need 7 moles of O2.
Step 2: Use the molar ratio to calculate the moles of O2 required.
Since we have 4.50 moles of NO2, we can set up a proportion:
4 moles NO2 / 7 moles O2 = 4.50 moles NO2 / X moles O2
Cross-multiplying, we get: X moles O2 = (4.50 moles NO2 * 7 moles O2) / 4 moles NO2
Simplifying, X moles O2 = 7.875 moles O2
Step 3: Convert moles of O2 to grams.
To convert moles to grams, we need to know the molar mass of O2. Oxygen has a molar mass of about 32 g/mol.
Grams O2 = 7.875 moles O2 * 32 g/mol = 252 grams O2
Therefore, the answer is 252 grams of oxygen are necessary to produce 4.50 moles of NO2.
2) The balanced equation is: 4NH3 + 7O2 → 4NO2 + 6H2O
To find how many molecules of water are produced when 2.25 moles of ammonia are completely reacted:
Step 1: Determine the molar ratio between NH3 and H2O from the balanced equation.
The coefficient of NH3 is 4, and the coefficient of H2O is 6. This means that for every 4 moles of NH3 reacted, we produce 6 moles of H2O.
Step 2: Use the molar ratio to calculate the moles of H2O produced.
Since we have 2.25 moles of NH3, we can set up a proportion:
4 moles NH3 / 6 moles H2O = 2.25 moles NH3 / X moles H2O
Cross-multiplying, we get: X moles H2O = (2.25 moles NH3 * 6 moles H2O) / 4 moles NH3
Simplifying, X moles H2O = 3.375 moles H2O
Step 3: Convert moles of H2O to molecules.
To convert moles to molecules, we need to use Avogadro's number, which is approximately 6.022 x 10^23 molecules/mol.
Molecules H2O = 3.375 moles H2O * (6.022 x 10^23 molecules/mol) = 2.03 x 10^24 molecules H2O
Therefore, the answer is approximately 2.03 x 10^24 molecules of water are produced when 2.25 moles of ammonia are completely reacted.