Lightweight camping stoves typically use a mixture of C₅ and C₆ hydrocarbons, which is called white gas. Assuming white gas is 100% C₅H₁₂ with an enthalpy of combustion of -3,550 kJ/mol, how many grams of it must be used to heat 1.50 L of water from 20°C to 80°C? Assume all the energy is used to heat the water.

Question

Quizplus · Accepted Answer

To find the mass of C5H12 needed, first calculate the energy required to heat the water: q = m * c * ΔT. For 1.50 L of water (1,500 g), with c = 4.18 J/g°C, and ΔT = 60°C, q = 1,500 * 4.18 * 60 = 376,200 J = 376.2 kJ. The moles of C5H12 needed = 376.2 kJ / 3550 kJ/mol = 0.106 mol. The molar mass of C5H12 is 72.15 g/mol, so mass = 0.106 mol * 72.15 g/mol = 7.64 g.

Lightweight Camping Stoves Typically Use a Mixture of C5 and C6

Lightweight Camping Stoves Typically Use a Mixture of C₅ and C₆