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
Here's how to calculate the molecular mass of gas A: Step 1: State Graham's Law of Effusion. Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. For two gases, A and B, effusing under identical conditions: Rate_ARate_B = sqrt((M_B)/(M_A)) Since the volume effused is the same for both gases, the rate is inversely proportional to the time taken for effusion ( Rate = VolumeTime ). Therefore, we can write: (t_B)/(t_A) = sqrt((M_B)/(M_A)) Where t_A and t_B are the times for effusion, and M_A and M_B are the molar masses. Step 2: Calculate the molar mass of CO_2. The atomic mass of Carbon (C) is approximately 12.01 g/mol. The atomic mass of Oxygen (O) is approximately 16.00 g/mol. M_CO_2 = 12.01 + (2 × 16.00) = 12.01 + 32.00 = 44.01 g/mol Step 3: Substitute the known values into Graham's Law and solve for M_A. Given: t_A = 146 s t_CO_2 = 115 s M_CO_2 = 44.01 g/mol 115 s146 s = sqrt(44.01 g/mol)M_A Square both sides of the equation: ((115)/(146))^2 = 44.01 g/molM_A (0.78767)^2 = 44.01 g/molM_A 0.62043 = 44.01 g/molM_A Now, solve for M_A: M_A = 44.01 g/mol0.62043 M_A ≈ 70.93 g/mol The molecular mass of gas A is 70.9 g/mol. That's 2 down. 3 left today — send the next one.