6. The combustion of a sample of butane, C. H. (lighter fluid), produced 2.46 grams of water. Using the balanced equation below, calculate the mass (grams) of carbon
dioxide produced.
2 C. H. + 13 0, > 8 CO, +10 H2O.

please help me find the carbon dioxide :)

Hey,

QUESTION)

1) We balance the equation of the reaction, that to say :

2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O

2) Calculating the molar mass of simple butane :

M(C₄H₁₀) = 4M(C) + 10M(H)

M(C₄H₁₀) = 4 x 12,0 + 10,0 M(C₄H₁₀) = 58,0 g/mol

3) Let us calculate the quantity of material corresponding to the mass of simple butane :

n(C₄H₁₀) = m/M

n(C₄H₁₀) = 2.46/58,0 n(C₄H₁₀) = 4,24 x 10⁻² mol

4) Determining the progress maximal x of the reaction,

xmax = n(C₄H₁₀)/2

xmax = 4,24 x 10⁻²/2 xmax = 2,12 x 10⁻² mol

5) If the reagents are supplied in a stoichiometric quantity, and the combustion is complete, then :

n(CO₂) = xmax x 8

n(CO₂) = 2,12 x 10⁻² x 8 n(CO₂) = 17,0 x 10⁻² mol

m(CO₂) = M(CO₂) x n(CO₂)

m(CO₂) = (12 + 2 x 16) x 17,0 x 10⁻² m(CO₂) = 7,48 g The mass of carbon dioxide is therefore 7.48 g.

1.from liquid state to gaseous state is evaporation 3.solid to liquid is melting 5. solid to gaseous state is sublimation 6. gas to solid state is decomposition 7. a change of state is known as the states of matters

Sorry i dont understand the question can you rephase it?