(b) Convert the O3 mixing ratio of 100 ppbv (parts-per-billion by volume) to an O3 concentration (mass/volume) value using the ideal gas equation. Assume standard temperature and pressure (STP). The molecular weight of O3 is 48 g/mol.
Parts-per-billion by volume : 1ppb = 1 microliter / cubic meter
O3 100 ppbv = 100 microliter / m3 = 10-7 m3 . = 0.0001 L
Using the ideal gas equation. PV = nRT (at STP)
From STP volume of one mole = 22.4 L
No. of moles of Ozone = 0.0001 L / 22.4 L = 4.46*10-6 moles
Molecular weight of O3 = 48 g/mol
Mass of ozone = 4.46*10-6 mole * 48 g/mol = 2.14* 10-4 gm.
So, concentration of ozone (mass/volume) = 2.14* 10-4 gm. / cubic meter
= 2.14* 10-4 gm. / 1000 L (1 c-m = 1000 L)
= 2.14* 10-7 gm. / L = 0.214 microgram / L
(b) Convert the O3 mixing ratio of 100 ppbv (parts-per-billion by volume) to an O3 concentration...
Unit conversion. (10 pts) Convert a concentration of 5.62 ´1013 molecules/cm 3 to the ppb scale. Assume 25° C and 1.0 atm total air pressure. Convert a concentration of 6.0 ´1014 molecules/cm 3 to the moles per liter (molarity) scale. Assume 27.5° C and 0.99 atm total air pressure. Convert a concentration of 36.5 ppb of ozone, O3, into the number of molecules/cm3. Assume the air mass temperature is 25.3° C and its total pressure is 1.05 atm. Convert a...
Standard Temperature and Pressure Standard Temperature Standard Pressure Is there such a thing as standard volume? Example #1 A gas at 772 mmHg and 35.0°C occupies a volume of 6.85 L. Calculate its volume at STP. Remember Mass to moles → Formula Weight Volume of solution to moles → Molarity Volume of a gas to moles → Ideal Gas Law
1a) It is desired to inflate a baggie with a volume of 936 milliliters by filling it with methane gas at a pressure of 1.18 atm and a temperature of 296 K. How many grams of CH4 gas are needed? _____ g 1b) A 0.705 gram sample of an unknown gas is found to occupy a volume of 0.620 L at a pressure of 472 mm Hg and a temperature of 59°C. The molecular weight of the unknown gas is...
A 2.54 gram sample of an unknown gas is found to occupy a volume of 1.43 L at a pressure of 989 mm Hg and a temperature of 40°C. The molecular weight of the unknown gas is g/mol. Assume ideal behavior.
please do all. thanks. 1. a. A weather balloon is filled to the volume of 105 L on a day when the temperature is 25°C. If no gases escaped, what would be the volume of the weather balloon after it rises to an altitude where the temperature is -9°C? Volume = L? b A 203-mL sample of a gas exerts a pressure of 2.55 atm at 19.5°C. What volume would it occupy at 1.85 atm and 190.°C? Volume = ?mL...
Use the ideal gas law to calculate the volume occupied by 1.00 mol of ideal gas at 1.00 atm pressure and 10.0°C. Given that the average molecular weight of air is 28.9 g/mol, calculate the mass density of air, in kg/m3at the above conditions.
6. "In evaluating indoor air concentrations of carcinogenic or toxic compounds, some confusion exists over the various units in use. Common units of indoor air measurements include ug/m3 or mg/m3, ug/L or mg/L, ppbV and ppmV. The confusion arises in converting from mass-per-volume to parts-per- number-volume units. It is important to remember that ug/L in gas systems IS NOT equal to ppbV, nor is mg/L in gas systems equal to ppmV. Each of these conversions is dependent upon the molecular...
Given: At normal temperature and pressure, the following conversion formulas may be used to convert back and forth between ppm and mg/m3 . mg/m3= [(MW x ppm) / 24.45] or ppm = [(24.45 x mg/m3 ) / MW] MW: molecular weight in g/mole In these equations 24.45 is the volume (in liters) of a mole (gram molecular weight) of a gas or vapor when the pressure is at 1 atmosphere (760 mmHg) and the temperature is at 25°C. When temperature...
6) In the absence of turbulent mixing, the partial pressure of each constituent of air would fall off with PiPleMi8:/RT height above sea level in Earth's atmosphere as where Pi is the partial pressure of component i at height z, Po is the partial pressure of component i at sea level, g is the acceleration due to gravity, R is the gas constant, T'is the absolute temperature, and Mi is the molecular mass of component i. As a result of...
Need help solving these last 7 questions. Please use the data above to calculate the answers. Molar Volume of a Gas Room temperature (T2): Barometric pressure: C be & torr Tria .0544 Data Trial 2 Trial 1 Mass of Mg strip Temperature of water in the 600-mL beaker 8.1 torr 142 Vapor pressure of water at the temperature in the 600-mL beaker torr torr S6.4 A.1 Volume of gas collected at room temperature mL mL ,67as 0541 S04L Volume of...