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.
ScanSolve AI Answer
To determine which gas has the lowest rate of diffusion, we use Graham's Law of Diffusion, which states that the rate of diffusion of a gas is inversely proportional to the square root of its molar mass. This means that the gas with the highest molar mass will have the lowest rate of diffusion. We need to calculate the molar mass for each gas given the atomic masses: H=1.0, C=12.0, N=14.0, O=16.0. Step 1: Calculate the molar mass for each gas. A. Nitrogen (N_2) Molar mass of N_2 = 2 × Atomic mass of N Molar mass of N_2 = 2 × 14.0 = 28.0 g/mol B. Ammonia (NH_3) Molar mass of NH_3 = Atomic mass of N + (3 × Atomic mass of H) Molar mass of NH_3 = 14.0 + (3 × 1.0) = 14.0 + 3.0 = 17.0 g/mol C. Oxygen (O_2) Molar mass of O_2 = 2 × Atomic mass of O Molar mass of O_2 = 2 × 16.0 = 32.0 g/mol D. Methane (CH_4) Molar mass of CH_4 = Atomic mass of C + (4 × Atomic mass of H) Molar mass of CH_4 = 12.0 + (4 × 1.0) = 12.0 + 4.0 = 16.0 g/mol Step 2: Compare the molar masses. Nitrogen (N_2): 28.0 g/mol Ammonia (NH_3): 17.0 g/mol Oxygen (O_2): 32.0 g/mol Methane (CH_4): 16.0 g/mol Oxygen (O_2) has the highest molar mass (32.0 g/mol) among the given options. Step 3: Determine the gas with the lowest rate of diffusion. According to Graham's Law, the gas with the highest molar mass will have the lowest rate of diffusion. Therefore, Oxygen (O_2) has the lowest rate of diffusion. The correct option is C. The final answer is C