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
Right ThegirlGodishelping🥰💙🫠, let's go. Step 1: Identify the given values and the formula. We are given the effusion times for gas A and CO_2 for the same volume. Graham's Law of Effusion states that the ratio of the rates of effusion of two gases is inversely proportional to the square root of the ratio of their molar masses. Since rate is inversely proportional to time for a fixed volume, we can write: t_CO_2t_A = sqrt(M_CO)_2M_A Given: t_A = 146 s t_CO_2 = 115 s Step 2: Calculate the molar mass of CO_2. The molar mass of carbon (C) is approximately 12.01 g/mol. The molar 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 values into Graham's Law equation. 115 s146 s = sqrt(44.01 g/mol)M_A Step 4: Square both sides of the equation to eliminate the square root. ((115)/(146))^2 = 44.01 g/molM_A (0.78767)^2 ≈ 0.62043 = 44.01 g/molM_A Step 5: Solve for M_A. M_A = 44.01 g/mol0.62043 M_A ≈ 70.93 g/mol The molecular mass of A is approximately 70.93 g/mol. 70.93 g/mol Send me the next one 📸