How many molecules (not moles) of NH3 are produced from 1.17×10−4g of H2?
Express your answer numerically as the number of molecules.
Well, this question seems a bit serious for me. But don't worry, I'll try my best to make it interesting for you!
First, let's start with the given information: 1.17×10−4g of H2.
Now, let's do some chemistry math in style! To figure out the number of molecules, we need to convert grams to moles, and then from moles to molecules.
The molar mass of H2 is 2 g/mol. So, if we divide 1.17×10−4g by the molar mass of H2 (2 g/mol), we can find the number of moles of H2.
1.17×10−4g ÷ 2 g/mol = 5.85×10−5 moles of H2.
Since the balanced chemical equation for the production of NH3 from H2 is 3H2 → 2NH3, we can say that for every 3 moles of H2, we get 2 moles of NH3.
So, if we have 5.85×10−5 moles of H2, we can calculate the number of moles of NH3 by using the ratio:
5.85×10−5 moles H2 × (2 moles NH3 / 3 moles H2) = 3.90×10−5 moles NH3.
Finally, to find the number of molecules, we multiply the number of moles of NH3 by Avogadro's number, which is 6.022×10^23 molecules/mol.
3.90×10−5 moles NH3 × (6.022×10^23 molecules/mol) = 2.35×10^19 molecules of NH3.
So, the answer is approximately 2.35×10^19 molecules of NH3. Ta-da! I hope I was able to make this chemical calculation a bit amusing for you.
To find the number of molecules of NH3 produced from a given mass of H2, we first need to calculate the number of moles of H2 and then use the balanced chemical equation to determine the stoichiometric ratio between H2 and NH3.
Step 1: Calculate the number of moles of H2
Given mass of H2 = 1.17×10^(-4) g
The molar mass of H2 = 2 g/mol
Number of moles of H2 = mass of H2 / molar mass of H2
= 1.17×10^(-4) g / 2 g/mol
= 5.85×10^(-5) mol
Step 2: Use the balanced equation to determine the stoichiometric ratio
The balanced equation for the reaction of H2 with NH3 is:
3H2 + N2 -> 2NH3
From the balanced equation, we see that 3 moles of H2 react to produce 2 moles of NH3.
Step 3: Calculate the number of molecules of NH3
Number of moles of NH3 = (Number of moles of H2) x (2 moles of NH3 / 3 moles of H2)
= 5.85×10^(-5) mol x (2/3)
≈ 3.90×10^(-5) mol
To convert moles to molecules, we need to multiply by Avogadro's number (6.022 × 10^23 molecules/mol).
Number of molecules of NH3 = (Number of moles of NH3) x (Avogadro's number)
= 3.90×10^(-5) mol x (6.022 × 10^23 molecules/mol)
≈ 2.35×10^19 molecules
Therefore, approximately 2.35×10^19 molecules of NH3 are produced.
To determine the number of molecules of NH3 produced from a given mass of H2, we need to follow these steps:
Step 1: Convert the given mass of H2 to the number of moles.
To do this, we need to know the molar mass of H2, which is approximately 2 grams/mol.
Given mass of H2 = 1.17×10−4 g
Number of moles of H2 = Given mass / molar mass = 1.17×10−4 g / 2 g/mol
Step 2: Use stoichiometry to relate the moles of H2 to moles of NH3.
From the balanced chemical equation for the reaction, we know that 3 moles of H2 react with 2 moles of NH3, meaning the molar ratio is 3:2.
Therefore, the moles of NH3 produced would be:
Number of moles of NH3 = (Number of moles of H2) * (2/3)
Step 3: Convert the moles of NH3 to the number of molecules.
To convert from moles to molecules, we need to use Avogadro's number, which is approximately 6.022 × 10^23 molecules/mol.
Number of molecules of NH3 = (Number of moles of NH3) * Avogadro's number
Now let's calculate it:
Number of moles of H2 = (1.17×10−4 g) / (2 g/mol)
Number of moles of NH3 = (Number of moles of H2) * (2/3)
Number of molecules of NH3 = (Number of moles of NH3) * Avogadro's number
Plug in the values and calculate the answer.