The balanced equation for the burning of N-butane is;
2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O
stoi. ratio 2 : 13 : 8 : 10
molar mass 58 32 44 18
moles X 13 X/2 8X/2 10X/2
105.86 688.10 423.45 529.31
produced mass 18632.8 g 9527.6 g
moles of n-butane = X = 6.14 x 10³ g / 58 g mol⁻¹
hence other moles of compounds can be calculated.
Mass = molar mass * moles
mass fraction = mass / total mass
hence the mass fraction of
CO₂ = 18632.8 / 6.14 x 10³ = 3.03
H₂O = 9527.6 / 6.14 x 10³ = 1.55
the required mass of air = 688.10 x 32 = 22019.2 g = 2.20 kg
Thermometer with black bulb because black reflects less heat than white
Slicing carrotsin a chemical reacționat the reactants, which are on the left side of the equation should become something else which are the products on the right side of the equation!
You get nothing but also carrot when slice it up but for example frying an egg due to the heat, chemical energy, you get scrambled egg or whatever!
