a. Themassof 174 mL of CO₂ at STP is approximately 0.318 grams.b. The mass of 159 mL of O₂ at STP is approximately 0.356grams.c. The mass of 1.33 L of SF₆ atSTPis approximately 9.05 grams.To calculate the mass of a gas sample at STP (Standard Temperature and Pressure), we can use the relationship betweenvolume, pressure, temperature, and the molar mass of the gas.STP is defined as atemperatureof 273.15 K (0 degrees Celsius) and a pressure of 1 atmosphere (atm).To find the mass, we need to convert the given volumes to liters (L) and then use theideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.Since we are given the volume and the conditions are at STP, we can assume that thepressureis 1 atm and the temperature is 273.15 K.To calculate the number ofmoles, we can rearrange the ideal gas law equation to solve for n: n = PV/RT.Using the molar mass of each gas, we can thencalculatethe mass by multiplying the number of moles by the molar mass.For example, for part (a), CO₂ has a molar mass of approximately 44.01 grams/mol. Converting 174 mL to liters (0.174 L) and plugging in the values into theequationn = PV/RT, we can find the number of moles of CO₂. Multiplying the number of moles by the molar mass gives us the mass of CO₂, which is approximately 0.318 grams.Similarly, we can follow the same process for parts (b) and (c) using themolar massesof O₂ and SF₆, respectively, to calculate their respective masses at STP.To learn more aboutmass at STP, herebrainly.com/question/29796641#SPJ4...

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