7.37g of CO₂ is formed by burning 2. 43 g of c4h10.
Calculating mass of CO2 produced.
The balanced reaction is given as
2C₄H₁₀ + 13O₂ ---> 8CO₂ + 10H₂O
The stoichiometry of C₄H₁₀ to CO₂tells us that
- for every 2 mole of butane used up,8 moles of CO₂ are formed
or simply
- for every 1 mole of butane used up,4 moles of CO₂ are formed
Calculating the number of moles used, we first find molar mass of butane
molar mass of butane = (12 g/mol x 4) + (1 g/mol *x10) = 58 g/mol
Number of moles = Mass / Molar mass
= 2. 43 g/ 58 g/mol= 0.041 8mol
Rem,
1 mol of butane forms 4 mol of CO₂
Therefore 0.041 8mo lof butane forms = 4 x0.041 8mol = 0.1675mol of CO₂
molar mass of CO₂ = 44 g/mol
Mass of CO₂ formed =0.1675mol X 44 g/mol = 7.37g of CO₂ is formed
Learn more on finding mass using stoichiometry : https://brainly.com/question/9081030
