Question

In the reaction, 2HgO(s)⟶2Hg(s) O2(g). How many liters of oxygen, O2 measured at STP, would be produced from the decomposition of 111 g of mercury(II) oxide, HgO?

Answer 1

Answer:

5.74 L O₂

General Formulas and Concepts:

Chemistry - Gas Laws

• Reading a Periodic Table
• Using Stoichiometry
• STP (Standard Conditions for Temperature and Pressure) = 22.4 L per mole at 1 atm, 273 K

Explanation:

Step 1: Define

RxN:   2HgO (s) → 2Hg (s) + O₂ (g)

Given:   111 g HgO

Step 2: Identify Conversions

STP

Molar Mass of Hg - 200.59 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of HgO - 200.59 + 16.00 = 216.59 g/mol

Step 3: Stoichiometry

$111 \ g \ HgO(\frac{1 \ mol \ HgO}{216.59 \ g \ HgO} )(\frac{1 \ mol \ O_2}{2 \ mol \ HgO} )(\frac{22.4 \ L \ O_2}{1 \ mol \ O_2} )$ = 5.73988 L O₂

Step 4: Check

We are given 3 sig figs. Follow sig fig rules and round.

5.73988 L O₂ ≈ 5.74 L O₂