Question

What mass of carbon dioxide can be produced from 3.60 g butane and 2.30 g of oxygen in the unbalanced reaction C4H10 + O2 -> CO2 + H2O?

Answer 1

Mass = 2.64 g

Step-by-step explanation:

Given data;

Mass of butane = 3.60 g

Mass of oxygen = 2.30 g

Mass of carbon dioxide produced = ?

Solution:

Chemical equation:

O₂ + C₄H₁₀ → CO₂ + H₂O

Number of moles of BUTANE:

Number of moles = mass/ molar mass

Number of moles = 3.60 g / 58.12 g/mol

Number of moles = 0.06 mol

Number of moles of oxygen:

Number of moles = mass/ molar mass

Number of moles = 2.30 g / 32 g/mol

Number of moles = 0.07 mol

Now we compare the moles ammonia with hydrogen and nitrogen

O₂ : CO₂

1 : 1

0.07 : 0.07 mol

C₄H₁₀ : CO₂

1 : 1

0.06 : 0.06 mol

The number of moles of carbondioxide produced by butane are less so it will limiting reactant.

Theoretical yield:

Mass = number of moles × molar mass

Mass =0.06 mol × 44 g/mol

Mass = 2.64 g