The density of the sun is 1.41 g/cm 3 and its volume is 1.41 x 10 27 m 3 . How many hydrogen molecules are in the sun if we assume all the mass is hydrogen gas?

Here in this practice question it says, the density of the sun is 1.41 grams per centimeters cubed, and its volume is 1.41 times ten to the 27 meters cubed. How many hydrogen molecules are in the sun if we assume all mass is hydrogen gas? Alright. So we're gonna say first that we have just this one amount here, which just has 1 unit, liters cubed. Since it has 1 unit associated with it, it must be our given amount. Remember, our given amount has only 1 unit connected to it. The density has 2 units tied together, so that is a conversion factor, which we'll deal with later. Our end amount is what we're trying to find here. So our end amount here equals some unknown amount of hydrogen molecules. Now remember, we use the term molecules when we're dealing with a compound with 2 or more nonmetals, and remember that the natural form of hydrogen is H2. Alright. So we're gonna have to try to get to our end amount for our given amount by using conversion factors. Now realize here at this point that this is in meters cubed, but our density is in centimeters cubed. So we're gonna have to use a metric prefix conversion to go from meters to centimeters. Alright. So we're going to say here that our first conversion factor will be meters on the bottom, centimeters on top. Remember that 1 centi is 10 to the negative 2. Now we're gonna have to cube this whole thing because we want meters cubes to cancel out. So here, meters cubes would cancel out, and now I have centimeters cubed. Next, I'm going to say that to cancel out centimeters cubed, I can use the density given to me in the very beginning, which is 1.41, grams of h2 for every 1 centimeters cubed, so this would be conversion factor 2. So centimeters cubes here cancel out, and now I have grams of h2. Since we have grams, remember we can go from grams to moles, and then we can go to molecules. So So this is where a mole concept steps in. We have grams of h two on the bottom, and we have 1 mole of h two on top. So remember, hydrogen itself has an atomic mass of 1.008 grams according to the periodic table, and there are 2 hydrogens involved in h 2. So that would come up to the mass a mass of 2.016 as the molar weight of h2. So this would be conversion factor 3. So grams of h2 cancel out. Now finally, we're gonna have conversion factor 4, which just requires us to go from moles to molecules. On the bottom we'll have moles of h 2 and on top we'll have 6.022 times 10 to the 23 h 2 molecules. So we're using Avogadro's number. So here, moles of h two cancel out and at the end I'll have moles, molecules of h2. So anything that's in scientific notation, remember, to avoid errors in your calculator, you want to put them in parentheses. Now, we've talked about this before, what effect would cubing everything here have in terms of my units and values? So if I cube everything in here, this would really just change this into 1 centimeters cubed on the top, and then remember if you're raising a power to a power, they're really just multiplying together. So it was negative 2, and then we cubed it, so then it's really negative 2 times 3. So that would be negative 6 meters cubed. Alright. So then multiply, multiply, multiply these on top. And make sure here that this is 10 to the negative 6, so put this in parenthesis as well, and this as well. Now, if you plug everything correctly into your calculator, you should get back as your number 5.938 65 times 10 to the 56 h two molecules. Now, this value here has 3 sig figs, this value here has 3 sig figs. So our answer at the end with 3 sig figs would be 5.94 times 10 to the 56 h 2 molecules. So this here would be our final answer. Now it's a bit tricky, but remember, look out for the given amount, which is the unit by itself, and then look to see what your end amount, what are you looking for. And then utilize some types of conversion factors to go from the given amount to the end amount.

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1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
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10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
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12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
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18. Amino Acids and Proteins1h 51m
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23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

6. Chemical Reactions & Quantities

Mole Concept

GOB Chemistry

6. Chemical Reactions & Quantities

Mole Concept

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Multiple Choice

The density of the sun is 1.41 g/cm³ and its volume is 1.41 x 10²⁷ m³. How many hydrogen molecules are in the sun if we assume all the mass is hydrogen gas?

5.94 x 10⁵⁶ H₂ molecules

8.13 x 10⁵⁷ H₂ molecules

3.04 x 10⁵⁸ H₂ molecules

7.46 x 10⁵⁹ H₂ molecules

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Verified step by step guidance

Convert the volume of the sun from cubic meters to cubic centimeters. Since 1 m³ = 1,000,000 cm³, multiply the given volume by 1,000,000.

Calculate the mass of the sun using the formula: mass = density × volume. Use the density in g/cm³ and the converted volume in cm³.

Assume the entire mass of the sun is hydrogen gas (H₂). Calculate the number of moles of hydrogen gas using the molar mass of H₂, which is approximately 2.02 g/mol.

Use Avogadro's number (6.022 × 10²³ molecules/mol) to convert the moles of hydrogen gas to the number of hydrogen molecules.

Compare the calculated number of hydrogen molecules to the given options to determine which one matches your result.