This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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You're on a roll — To find the volume occupied by the gas mixture, we will use the Ideal Gas Law, PV = nRT. First, we need to calculate the total number of moles of gas. Step 1: Calculate the mass of each gas. The total mass of the gases is 8.4 g. Mass of O₂ = 60\% of 8.4 g = 0.60 × 8.4 g = 5.04 g. Mass of H₂ = 40\% of 8.4 g = 0.40 × 8.4 g = 3.36 g. Step 2: Calculate the moles of each gas. The problem states the molar mass of O₂ is 16 g/mol and H₂ is 2 g/mol. For molecular oxygen (O₂), the molar mass is typically 2 × 16 g/mol = 32 g/mol. We will proceed with the chemically correct molar mass for O₂ as 32 g/mol, assuming the given 16 g/mol refers to atomic oxygen. Moles of O₂ (n_O_2): n_O_2 = Mass of O_2Molar mass of O_2 = 5.04 g32 g/mol = 0.1575 mol Moles of H₂ (n_H_2): n_H_2 = Mass of H_2Molar mass of H_2 = 3.36 g2 g/mol = 1.68 mol Step 3: Calculate the total moles of gas. n_total =