Question

CH4 + 202 → CO2 + 2H2O
How many grams of O2 produced from 2 moles of H20?

Answer 1

Mass of O₂= 64 g

Further explanation

Given

Reaction

CH₄ + 20₂ → CO₂ + 2H₂O

2 moles of H₂O

Required

Mass of O₂

Solution

In a chemical equation, the reaction coefficient shows the mole ratio of the compounds involved in the reaction, reactants or products

From the equation, mol ratio of H₂O : O₂ = 1 : 1, so moles O₂ :

= 1/1 x moles H₂O

= 1/1 x 2

= 2 moles

Mass of O₂ :

= mol x MW

= 2 x 32 g/mol

= 64 g

Answer 2

60 g O₂

General Formulas and Concepts:

Math

Pre-Algebra

Order of Operations: BPEMDAS

1. Brackets
2. Parenthesis
3. Exponents
4. Multiplication
5. Division
6. Addition
7. Subtraction

• Left to Right

Chemistry

Atomic Structure

• Reading a Periodic Table

Stoichiometry

• Using Dimensional Analysis

Explanation:

Step 1: Define

[RxN - Balanced] CH₄ + 2O₂ → CO₂ + 2H₂O

[Given] 2 mol H₂O

[Solve] x g O₂

Step 2: Identify Conversions

[RxN] 2 mol H₂O → 2 mol O₂

[PT] Molar Mass of O - 16.00 g/mol

Molar Mass of O₂ - 2(16.00) = 32.00 g/mol

Step 3: Stoichiometry

1. Set up conversion:
   `\displaystyle 2 \ mol \ H_2O((2 \ mol \ O_2)/(2 \ mol \ H_2O))((32.00 \ g \ O_2)/(1 \ mol \ O_2))`
2. Divide/Multiply:
   `\displaystyle 64.00 \ g \ O_2`

Step 4: Check

Follow sig fig rules and round. We are given 1 sig fig.

64.00 g O₂ ≈ 60 g O₂