How many molecules (not moles) of NH3 are produced from 3.55×10−4g of H2?
See your post below under the screen name of Branson. That should tell you how to work the problem. By the way, you make it difficult to help if you change screen names.
To determine the number of molecules of NH3 produced from a given mass of H2, you need to follow a set of steps. Here's how you can do it:
Step 1: Convert the given mass of H2 to moles.
To convert grams to moles, you need to use the molar mass of hydrogen gas (H2), which is 2 g/mol. Divide the given mass of 3.55×10−4 g by the molar mass:
3.55×10−4 g / 2 g/mol = 1.775×10−4 mol
Step 2: Use the balanced chemical equation to relate the moles of H2 to NH3.
The balanced equation for the reaction of H2 to NH3 is:
3H2 + N2 -> 2NH3
From the balanced equation, you can see that for every 3 moles of H2, 2 moles of NH3 are produced.
Step 3: Calculate the moles of NH3 produced.
Using the stoichiometry from the balanced equation, you can calculate the moles of NH3 produced. Since the molar ratio of H2 to NH3 is 3:2, you can calculate it as follows:
1.775×10^-4 mol H2 * (2 mol NH3 / 3 mol H2) = 1.183×10^-4 mol NH3
Step 4: Convert moles of NH3 to molecules.
To convert moles to molecules, you can use Avogadro's number, which states that 1 mole of any substance contains 6.022×10^23 molecules. Multiply the moles of NH3 by Avogadro's number to get the number of molecules:
1.183×10^-4 mol NH3 * 6.022×10^23 molecules/mol = 7.121×10^19 molecules
Therefore, from 3.55×10^-4 g of H2, approximately 7.121×10^19 molecules of NH3 are produced.