Answer:
1. HgO(s) → Hg(l) + 0.5 O₂(g)
2. 0.858 g
Explanation:
There is some info missing. I think this is the original question.
<em>The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. </em>
<em>1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. </em>
<em>2. Suppose 59.0 mL of dioxygen gas are produced by this reaction, at a temperature of 90.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.</em>
<em />
1.
The balanced chemical equation is:
HgO(s) → Hg(l) + 0.5 O₂(g)
2.
First, we will calculate the moles of O₂ using the ideal gas equation.
P × V = n × R × T
n = P × V / R × T
n = 1 atm × 0.0590 L / 0.0821 atm.L/mol.K × 363.2 K
n = 1.98 × 10⁻³ mol
The molar ratio of HgO to O₂ is 1:0.5. The moles of HgO are (1/0.5) × 1.98 × 10⁻³ mol = 3.96 × 10⁻³ mol
The molar mass of HgO is 216.59 g/mol. The mass of HgO is:
3.96 × 10⁻³ mol × 216.59 g/mol = 0.858 g
