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
Hey Emrys, good to see you again. To calculate the vapor pressure of the aerosol mixture, we will use Raoult's Law and Dalton's Law of Partial Pressures. First, we need to convert the given gauge pressures to absolute pressures, then determine the mole fractions of each component, calculate their partial pressures, and finally sum them up. Step 1: Convert the given gauge pressures (P_sig) to absolute pressures (P_abs). The atmospheric pressure is given as 14.7 Psia. P_abs = P_sig + 14.7 Psia For HFA 134a: P_134a, abs = 62.4 Psig + 14.7 Psia = 77.1 Psia For HFA 227: P_227, abs = 56.0 Psig + 14.7 Psia = 70.7 Psia Step 2: Calculate the moles of each component. Assume a total mass of 100 g for the mixture. Mass of HFA 134a = 30\% of 100 g = 30 g Mass of HFA 227 = 70\% of 100 g = 70 g n_134a = 30 g102 g/mol = 0.2941 mol n_227 = 70 g170 g/mol = 0.4118 mol Step 3: Calculate the total moles and mole fraction (X) of each component. n_total = n_134a + n_227 = 0.2941 mol + 0.4118 mol = 0.7059 mol X_134a = n_134an_total = 0.2941 mol0.7059 mol = 0.4166 X_227 = n_227n_total = 0.4118 mol0.7059 mol = 0.5834 Step 4: Calculate the partial vapor pressure (P') of each component using Raoult's Law (P' = X · P_abs). P'_134a = X_134a × P_134a, abs = 0.4166 × 77.1 Psia = 32.12 Psia P'_227 = X_227 × P_227, abs = 0.5834 × 70.7 Psia = 41.25 Psia Step 5: Calculate the total absolute vapor pressure (P_total, abs) of the mixture. P_total, abs = P'_134a + P'_227 = 32.12 Psia + 41.25 Psia = 73.37 Psia Step 6: Convert the total absolute vapor pressure back to gauge pressure (P_total, sig). P_total, sig = P_total, abs - 14.7 Psia = 73.37 Psia - 14.7 Psia = 58.67 Psig Rounding to one decimal place: P_total, sig = 58.7 Psig The total vapor pressure of the aerosol mixture is 58.7 Psig. Send me the next one 📸