Question

In the reaction H₂ + F₂ → 2HF, what mass of HF is produced by the reaction of 1.2 x 10^24 molecules of H₂ with excess F₂?

Answer 1

To determine the mass of HF produced from 1.2 x 10^24 molecules of H₂ with excess F₂, the number of H₂ molecules is first converted to moles, multiplied by the stoichiometric ratio from the balanced equation, and then converted to mass using the molar mass of HF, giving 79.70 grams of HF.

Step-by-step explanation:

To calculate the mass of HF produced from 1.2 x 10^24 molecules of H₂, we should first convert the number of molecules to moles using Avogadro's number (6.022 x 10^23 molecules/mol). Then, using the stoichiometry of the balanced chemical equation, we can find moles of HF formed. Finally, we convert the moles of HF to mass using the molar mass of HF.

First, let's convert the number of H₂ molecules to moles:

1.2 x 10^24 molecules H₂ × (1 mol H₂ / 6.022 x 10^23 molecules H₂) = 1.992 mols H₂ (since 1 mol of any substance contains 6.022 x 10^23 molecules).

From the balanced equation H₂ + F₂ → 2HF, we see that 1 mole of H₂ produces 2 moles of HF. Thus, 1.992 moles of H₂ will produce:

1.992 moles H₂ × (2 moles HF / 1 mole H₂) = 3.984 moles HF

Now, let's find the mass of 3.984 moles of HF:

3.984 moles HF × (20.01 g/mol HF) = 79.70 g HF.

Therefore, the reaction of 1.2 x 10^24 molecules of H₂ with excess F₂ will produce 79.70 grams of HF