**Average Composition of the Atmosphere up to an Altitude of 25 km**| Gas Name | Chemical Formula | Percent Volume ||-----------------|------------------|----------------|| Nitrogen | N₂ | 78.08% || Oxygen | O₂ | 20.95% || Water | H₂O | 4% || Argon | Ar | 0.93% || Carbon Dioxide | CO₂ | 0.036% || Neon | Ne | 0.0018% || Helium | He | 0.0005% || Methane | CH₄ | 0.00017% || Hydrogen | H₂ | 0.00005% || Nitrous Oxide | N₂O | 0.00003% || Ozone | O₃ | 0.000004% |**Questions:**4. Under STP conditions, compare the relative rates at which Earth’s atmospheric gases diffuse through a common orifice. List them in order of fastest to slowest to diffuse (WITH numeric proof!).5. What is the partial pressure of carbon dioxide in Earth’s atmosphere?6. What does the table of atmospheric gases tell you about the mole fraction of sulfur hexafluoride in the atmosphere?7. What is the mole fraction of greenhouse gases in the atmosphere? (Please use the given table.)8. We already broke down the sources of anthropogenic CO₂ in class. All SF₆ is anthropogenic. Not all CO₂ and CH₄ are anthropogenic. Do you believe human activity can change the partial pressure of CO₂ enough to make a difference? Why or why not?9. What are you personally doing for the big beautiful world lately?

Under standard temperature and pressure (STP) conditions, the rates of diffusion of gases are determined by their molar masses. Graham's law of diffusion describes that the rate of diffusion of a gas is inversely proportional to the square root of its molar mass.We need to list the Earth's atmospheric gases from fastest to slowest to diffuse.The molar mass of N2 = 28 g/molThe molar mass of O2 = 32 g/molThe molar mass of H2O = 18 g/molThe molar mass of Ar = 40 g/molThe molar mass of CO2 = 44.01 g/molThe molar mass of Ne = 20 g/molThe molar mass of He = 4 g/molThe molar mass of CH4 = 16 g/molThe molar mass of H2 = 2 g/molThe molar mass of N2O = 44 g/molThe molar mass of O3 = 48 g/molAccording to the relationship between the rate and molar mass of two gases:Now, compare the relative rates of diffusion:The higher the rate of diffusion, the greater the speed of the gas.Therefore, the fastest to slowest gases are:H2HeCH4H2ONeN2O2ArN2OCO2O3Therefore, the fastest to slowest gases are:H2HeCH4H2ONeN2O2ArN2OCO2O3

Answered: 4. Under STP conditions, compare the…

Science

Chemistry

4. Under STP conditions, compare the relative rates at which Earth's atmospheric gases diffuse through a common orifice. List them in order of fastest to slowest to diffuse (WITH numeric proof!)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Application of gas laws to atmospheric science
A weather balloon is inflated to a volume of 28.5 L at a pressure of 748 mm Hg and a temperature of 28.0 oC. The balloon rises where the pressure is 385 mm Hg and the temperature is 15.0 oC. Assuming the balloon can freely expand, calculate the volume of the balloon in liters.
Given the following: Difference in height 55.0 mm Volume of enclosed gas (V) 0.0638 L Temperature of enclosed gas (T) 22.0°C Barometric pressure (Pbar) 755 Torr Pressure of water vapor (Pwater vapor) 19.3 Torr Pre-weighed mass of Mg 0.0590 g Calculate: Pressure of trapped air (Ptrapped air), Torr Pressure of dry air (Pdry air), Torr Moles of gas produced, mol Calculated mass of Mg, g Percent error, %
A sample of nitrogen gas occupies a volume of 6.54 L at 65.0°C and 403 torr. If the volume of the gas sample is increased to 9.12 L, while its temperature is increased to 124.0°C, the resulting gas pressure will be torr.
In an expandable balloon we find a mixture of two gases only. The mass percent of the gases are: 65% 02 and 35 % H2. The mass of the gases combined is 4.6 grams. Calculate the total volume these two gases occupy at 298 K and 1.10 atm.
b 11. example outcome paper DP X II. Outcome paper INSTRUCTIO X1. Assignment Submission Fold X ← → CO app.101edu.co 1971. Brightspace Walmart - Hiring Ce... Esc Lock # A sample of argon has a volume of 1.20 L at STP. If the temperature is increased to 28.0 °C and the pressure is lowered to 0.800 atm, what will the new volume be, in L? + F1 ! 1 4x t Q A 7 F2 2 O W S F3 W ➡ # 3 X F4 144 D $ 4 F5 ► 11 E R F % 5 F6 64 TCV T G F7 A 6 Y B F8 & 7 H Question 5 of 9 DELL U N F9 Aktiv Chemistry (fka: Chem10 X * : 00 J S F10 M ( 9 K F11 O 1 4 7 +/- PrtScr yº + 2 + 11 LO 5 8 Insert . X } il : BO . ; ? Q C 0 Del Bac 1
A balloon of volume 100.2 L contains a gas at a temperature of 22.0°C and pressure of 0.981 atm. This balloon is released, travels upward in the atmosphere, and passes over the top of Pikes Peak. At the top of Pikes Peak the temperature is 1.24°C and the balloon has expanded to 144.5 L. What is the pressure of the gas inside the balloon as as it clears the top of America’s Mountain?
3. A certain mass of magnesium is reacted with 6M HCl. The hydrogen gas liberated is collected by displacing 200 mL of water. The pressure of the gas and the atmospheric pressure are equalized. The atmospheric pressure is 762 mmHg. The temperature of the experiment is 27°C. How many moles of hydrogen have been liberated, and what is the mass of the magnesium that reacted?
A 19.50 g sample of a gas occupies a volume of 24.8 L at 22.7ºC and 748.3 mmHg. What is its molecular mass? Give units in your answer here.