Lightweight camping stoves typically use a mixture of C₅ and C₆ hydrocarbons, which is called white gas.Assuming white gas is 100% C₆H₁₄ with an enthalpy of combustion of -4150 kJ/mol, how many grams of it must be used to heat 1.50 L of water from 20.0 $\degree$C to 90.0 $\degree$C? Assume all the energy is used to heat the water.

Question

Quizplus · Accepted Answer

To find the mass of C6H14 needed, calculate the energy required to heat the water using q = mcΔT, where m = 1.50 kg, c = 4.18 J/g°C, and ΔT = 70°C. Convert the energy to kJ, then use the enthalpy of combustion to find the moles of C6H14 needed, and finally convert to grams.

Lightweight Camping Stoves Typically Use a Mixture of C5 and C6

Lightweight Camping Stoves Typically Use a Mixture of C₅ and C₆