Question

2C3H7OH + 9O2 --> 6CO2 + 8H2O

Determine the number of grams of CO2 produced from the reaction of 5.55 moles of C3H7OH

Answer 1

Answer:

733 g CO₂

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]   2C₃H₇OH + 9O₂ → 6CO₂ + 8H₂O

[Given]   5.55 mol C₃H₇OH

Step 2: Identify Conversions

[RxN] 2 mol C₃H₇OH → 6 CO₂

Molar Mass of C - 12.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of CO₂ - 12.01 + 2(16.00) = 44.01 g/mol

Step 3: Stoichiometry

1. Set up conversion:                    $\displaystyle 5.55 \ mol \ C_3H_7OH(\frac{6 \ mol \ CO_2}{2 \ mol \ C_3H_7OH})(\frac{44.01 \ g \ CO_2}{1 \ mol \ CO_2})$
2. Multiply/Divide:                                                                                               $\displaystyle 732.767 \ g \ CO_2$

Step 4: Check

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

732.767 g CO₂ ≈ 733 g CO₂