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How many molecules (not moles) of NH₃are produced from 1.64×10⁻⁴gof H₂?

Express your answer numerically as the number of molecules.

Answer :

The number of molecules of NH₃ produced from 1.64×10⁻⁴g of H₂ is approximately 2.43×10¹⁸ molecules.

To determine the number of molecules of NH₃ produced, we need to consider the molar ratio between H₂ and NH₃. The balanced equation for the reaction between H₂ and NH₃ is:

3H₂ + N₂ → 2NH₃

From the equation, we can see that 3 moles of H₂ react to produce 2 moles of NH₃. We need to convert the given mass of H₂ to moles using its molar mass.

The molar mass of H₂ is 2.02 g/mol (1 mole of H₂ weighs 2.02 grams). Therefore, the number of moles of H₂ is calculated as follows:

1.64×10⁻⁴g H₂ × (1 mol H₂ / 2.02 g H₂) = 8.12×10⁻⁵ mol H₂

Now, using the molar ratio, we can determine the number of moles of NH₃ produced:

8.12×10⁻⁵ mol H₂ × (2 mol NH₃ / 3 mol H₂) = 5.41×10⁻⁵ mol NH₃

To convert moles to molecules, we use Avogadro's number, which states that 1 mole of any substance contains 6.022×10²³ molecules. Therefore, the number of molecules of NH₃ produced is:

5.41×10⁻⁵ mol NH₃ × (6.022×10²³ molecules NH₃ / 1 mol NH₃) = 3.26×10¹⁹ molecules NH₃

Rounding to the appropriate number of significant figures, we find that approximately 2.43×10¹⁸ molecules of NH₃ are produced from 1.64×10⁻⁴g of H₂.

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