Question

1st attempt Part 1 (1 pt) * Feedback bi See Periodic Table Complete and balance the chemical equation for this combustion reaction. Do not add states of matter. x x. "He → S. 2C4H10+1302 —— 10H20+8C02 Part 2 (1 pt) X Feedback ♡ See Hint Determine how many grams of CO2 are produced by burning 2.43 g of C4H10. g carbon dioxide

Answer 1

1)

The reaction is:

C4H10 + O2 -> H2O + CO2

Balance C:

C4H10 + O2 -> H2O + 4 CO2

Balance H:

C4H10 + O2 -> 5 H2O + 4 CO2

Balance O:

2 C4H10 + 13 O2 -> 10 H2O + 8 CO2

Answer:

2 C₄H₁₀ + 13 O₂ -> 10 H₂O + 8 CO₂

2)

Molar mass of C4H10,

MM = 4*MM(C) + 10*MM(H)

= 4*12.01 + 10*1.008

= 58.12 g/mol

mass of C4H10 = 2.43 g

mol of C4H10 = (mass)/(molar mass)

= 2.43/58.12

= 4.181*10^-2 mol

According to balanced equation

mol of CO2 formed = (8/2)* moles of C4H10

= (8/2)*4.181*10^-2

= 0.1672 mol

Molar mass of CO2,

MM = 1*MM(C) + 2*MM(O)

= 1*12.01 + 2*16.0

= 44.01 g/mol

mass of CO2 = number of mol * molar mass

= 0.1672*44.01

= 7.36 g

Answer: 7.36 g