How many grams of CO2could be produced from the combustion of 23g of C4H10in the presence of an adequate amount of O2?

Mass = 70.4 g

Explanation:

Given data:

Mass of CO₂ produced = ?

Mass of C₄H₁₀ = 23 g

Solution:

Chemical equation:

2C₄H₁₀ + 13O₂  →   8CO₂ + 10H₂O

Number of moles of C₄H₁₀:

Number of moles = mass/ molar mass

Number of moles = 23 g/ 58.12 g/mol

Number of moles = 0.4 mol

Now we will compare the moles of C₄H₁₀ and  CO₂  from balance chemical equation.

                   C₄H₁₀          :           CO₂

                        2             :             8

                      0.4           :          8/2×0.4 = 1.6 mol

Mass of CO₂:

Mass = number of moles × molar mass

Mass = 1.6 mol × 44 g/mol

Mass = 70.4 g

6.4 cm (max) - 25 cm (min)

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.