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 calculate the total vapor pressure of the aerosol mixture, we will use Raoult's Law and Dalton's Law of Partial Pressures. This involves determining the mole fractions of each component and then summing their partial pressures. Step 1: Calculate the moles of each component. Assume a total mass of 100 g for the mixture. Mass of Propellant I (CCl_3F) = 20\% of 100 g = 20 g Mass of Propellant II (CCl_2F_2) = 80\% of 100 g = 80 g Using the given molar masses: For Propellant I (CCl_3F, M_1 = 137.4 g/mol): n_1 = 20 g137.4 g/mol = 0.14556 mol For Propellant II (CCl_2F_2, M_2 = 120.9 g/mol): n_2 = 80 g120.9 g/mol = 0.66170 mol Step 2: Calculate the total moles and mole fraction (X) of each component. n_total = n_1 + n_2 = 0.14556 mol + 0.66170 mol = 0.80726 mol Mole fraction of Propellant I: X_1 = (n_1)/(n_total) = 0.14556 mol0.80726 mol = 0.18031 Mole fraction of Propellant II: X_2 = (n_2)/(n_total) = 0.66170 mol0.80726 mol = 0.81969 Step 3: Calculate the partial vapor pressure (P) of each component using Raoult's Law (P_i = X_i · P_i^). Given pure vapor pressures: P_1^ = 13.4 Psia and P_2^ = 84.9 Psia. Partial pressure of Propellant I: P_1 = X_1 × P_1^ = 0.18031 × 13.4 Psia = 2.416 Psia Partial pressure of Propellant II: P_2 = X_2 × P_2^ = 0.81969 × 84.9 Psia = 69.582 Psia Step 4: Calculate the total vapor pressure (P_total) of the mixture using Dalton's Law of Partial Pressures. P_total = P_1 + P_2 = 2.416 Psia + 69.582 Psia = 71.998 Psia Rounding to one decimal place: P_total = 72.0 Psia The total vapor pressure of the aerosol mixture is 72.0 Psia. That's 2 down. 3 left today — send the next one.