Question

What is the mass in grams of 4.57 × 10¹⁵ molecules of CO₂?

Answer 1

Answer:

In carbon dioxide's case, its molar mass is equal to 44.01 g/mol , which means that every mole of CO2 will have a mass of 44.01 g

Answer 2

The mass of 4.57 × 10¹⁵ molecules of CO₂ is approximately 3.35 × 10⁻⁷ g.

To calculate the mass of 4.57 × 10¹⁵ molecules of CO₂, we need to use the molecular weight of CO₂ and Avogadro's number.

The molecular weight of CO₂ is 44.01 g/mol (12.01 g/mol for each carbon atom and 16.00 g/mol for each oxygen atom).

Avogadro's number is 6.022 × 10²³ molecules/mol, which means there are 6.022 × 10²³ CO₂ molecules in one mole of CO₂.

We can use these values to convert the number of molecules to grams:

Calculate the number of moles of CO₂ in 4.57 × 10¹⁵ molecules:

Number of moles = Number of molecules / Avogadro's number

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= 4.57 × 10¹⁵ / 6.022 × 10²³

= 7.60 × 10⁻⁹ mol

Calculate the mass of 7.60 × 10⁻⁹ mol of CO₂:

Mass = Number of moles × Molecular weight

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= 7.60 × 10⁻⁹ mol × 44.01 g/mol

= 3.35 × 10⁻⁷ g

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