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Elan Coil [88]
3 years ago
11

Which one has the greatest mass?

Chemistry
2 answers:
Shtirlitz [24]3 years ago
8 0
To determine the one with the greatest mass, we convert all options into the same units of mass as follows:

<span>1. 3.55 mol O atoms ( 16 g / mol ) = 56.8 g O
2. 4.52 g O atoms 
3. 0.0032 kg O2 molec ( 1000 g / 1kg ) ( 1 mol / 32 g ) ( 2 mol / 1 mol ) ( 16 g / mol) = 3.2 g O
4. 7.39 × 10^23 O2 molec ( 1 mol / 6.022x10^23 molecules) (2 mol / 1 mol)(16 g/mol) = 39.27 g O</span>
dexar [7]3 years ago
7 0

<u>Answer:</u> The correct answer is Option 1.

<u>Explanation:</u>

For the given options:

  • <u>Option 1:</u>  3.55 mole of O atoms

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of Oxygen = 3.55 mol

Molar mass of Oxygen = 16 g/mol

Putting values in above equation, we get:

3.55=\frac{\text{Mass of oxygen}}{16g/mol}\\\\\text{Mass of oxygen}=56.8g

Mass of oxygen atoms = 56.8 g

  • <u>Option 2:</u> 4.52 g of O atoms

Mass of oxygen atoms = 4.52 g

  • <u>Option 3:</u> 0.0032 kg of O_2 molecule

Converting this into grams, we use the conversion factor:

1 kg = 1000 g

So, 0.0032 kg = 3.2 g

Mass of O_2 molecule = 3.2 g

  • <u>Option 4:</u> 7.39\times 10^{23} of O_2 molecule

According to mole concept:

1 mole of an atom contains 6.022\times 10^{23} number of atoms.

If, 6.022\times 10^{23} number of atoms occupies 32 grams of oxygen molecule.

So, 7.39\times 10^{23} number of atoms will occupy = \frac{32g}{6.022\times 10^{23}}\times 7.39\times 10^{23}=39.2g

Mass of O_2 molecule = 39.2 g

Hence, the greatest mass is coming out from option 1.

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Answer:

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Explanation:

The number of balloons can be calculated as follows:

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Where:

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Therefore, the number of balloons is 948.8.

I hope it helps you!        

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