Solution: Calculate the mass of octane, C8H18(g), that must be burned in air to evolve the same quantity of energy as produced by the fusion of 3.2 g of hydrogen in the following fusion reaction: 411 H  →  24

Calculate the mass of octane, C₈H₁₈(g), that must be burned in air to evolve the same quantity of energy as produced by the fusion of 3.2 g of hydrogen in the following fusion reaction: 4₁¹ H  →  ₂⁴ He + 2₁⁰ e Assume that all the products of the combustion of C₈H₁₈ are in their gas phases. Use data from Exercise 21.50, Appendix C, and the inside covers of the text. The standard enthalpy of formation of octane is -250.1 kJ/mol.