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Answer :

TutorAnnego

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

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