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 -3550 kJ/mol, how many grams of it must be used to heat 1.50 L of water from 20.0 $\degree$C to 80.0 $\degree$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 using q = mcΔT, where m = 1.50 kg, c = 4.18 J/g°C, and ΔT = 60°C. Then, convert this energy to kJ and divide by the enthalpy of combustion (3550 kJ/mol) to find moles of C5H12 needed. Finally, convert moles to grams using the molar mass of C5H12 (72.15 g/mol).

Lightweight Camping Stoves Typically Use a Mixture of C5 and C6

Lightweight Camping Stoves Typically Use a Mixture of C₅ and C₆