Calculate how much Hg in a reaction that produces 87.4 g O2 using: 2HgO produces 2 Hg + O2
To calculate the amount of Hg (mercury) produced in the given reaction, we need to use stoichiometry. Stoichiometry is a mathematical relationship between reactants and products in a chemical reaction.
Given:
- 2HgO produces 2 Hg + O2
We are given the mass of O2 produced, which is 87.4 g. We need to find the mass of Hg produced.
To find the mass of Hg, we can follow these steps:
1. Determine the molar mass of O2. The molar mass of O2 is approximately 32 g/mol (16 g/mol for each oxygen atom). So, 87.4 g of O2 is equal to 87.4 g / 32 g/mol = 2.73 mol O2.
2. Since the stoichiometric ratio between O2 and Hg in the balanced equation is 2:2, it means that for every 2 mol of O2 produced, we have 2 mol of Hg produced.
3. Using the ratio, we can calculate the number of moles of Hg produced. Since the ratio is 2:2, the number of moles of Hg produced is also 2.73 mol.
4. Finally, we can calculate the mass of Hg produced. We know that the molar mass of Hg is approximately 200.59 g/mol. So, the mass of Hg is equal to 2.73 mol Hg * 200.59 g/mol = 547.27 g.
Therefore, the amount of Hg produced in the reaction is approximately 547.27 g.