Question

Determine how many grams of CO2 are produced by burning 8.21 g of C4H10

Answer 1

25.872 g of carbon dioxide will produced.

Step-by-step explanation:

Given data:

mass of butane (C4H10) = 8.21 g

mass of carbon dioxide = ?

Solution:

Chemical equation

C4H10 + O2 → CO + H2O

Balanced chemical equation

2C4H10 + 13O2 → 8CO + 10H2O

First of all we will calculate the moles of butane.

number of moles = mass/ molar mass

number of moles = 8.21 g/ 58 g/mol

number of moles = 0.147 mol

from balanced chemical equation we will compare the moles of C4H10 with CO2,

C4H10 : CO2

2 : 8

0.147 : 8/2×0.147 = 0.588 moles

now we will calculate the mass of carbon dioxide from moles,

mass of CO2 = number of moles × molar mass of CO2

mass of CO2 = 0.588 mol × 44 g/mol

mass of CO2 = 25.872 g