Answer to Question #152896 in Chemistry for Arvin Shopon

Question

3.
Butane with an evaporation temperature of 0°C is used as liquefied gas in camping stoves. Butane is also a great power for summer hikers in Finland as a gas for a camping stove. One summer day the temperature was + 15°C and the air pressure 0.95 bar. Calculate how many liters of carbon dioxide was formed when a hiker boiled a 450-gram bottle of butane gas. Suppose the combustion was complete and that the hiker managed to cook the bottle empty (in fact, the same pressure remained inside the bottle as it was outside the bottle).

Answer 1

2C₄H₁₀ + 13O₂= 8CO₂ + 10H₂O

M (C₄H₁₀) = 58.12 g/mol

T = 15 + 273 = 288 K

n (C₄H₁₀) = 450/58.12 = 7.74 g/mol

n (CO₂) = 8/2 n (C₄H₁₀) = 8/2 x 7.74 = 30.96 mol

pV=nRT

R = 8.31 L⋅bar⋅K⁻¹⋅mol⁻¹

T = 15 + 273 = 288 K

V (CO₂) = nRT/p = (30.96 x 3.14 x 288) / 0.95 = 29 471 L