´A gas of unknown molecular mass was allowed to effuse through a small opening under constant-pressure condi- tions. It required 105 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 31 s for 1.0 L of O, gas to effuse. Calculate the molar mass of the

´A gas of unknown molecular mass was allowed to effuse through a small opening under constant-pressure condi- tions. It required 105 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 31 s for 1.0 L of O, gas to effuse. Calculate the molar mass of the

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

Related questions

Q: 9. A gas tank contains 2 gases P₂O4 and CH₂Br. If 0.029 moles of P2O4 effuses through a pinhole in…

A: The process of escaping the gas molecule through a very small hole is known as effusion. During…

Q: Find the molar mass of the Unknown gas?

A: According to Graham's law of effusion, the rate of effusion of a gas is inversely proportional to…

Q: White phosphorus melts and then vaporizes at high tempera-ture. The gas effuses at a rate that is…

A: The Scottish physical chemist Thomas Graham gives direct relation between rate of effusion of gas…

Q: To what temperature must a sample of nitrogen at 23.7oC and 0.759 atm be taken so that its pressure…

Q: In a sealed container, 230.0 L of air was collected at 50.0°C and 652 mmHg. The mole fraction of…

A: Given data,Volume(V) of air=230.0LTemperature(T)=50oC=50+273.15=323.15KPressure of…

Q: A 9.35 L container holds a mixture of two gases, gas A and gas B, at 53 ∘C The partial pressures of…

A: Dalton law of partial pressure : Ptotal = Pa + Pb + Pc + -----

Q: Three glass bulbs, joined by closed stopcocks, have the following volumes and initial pressures of…

Q: At 25.0 ° C, a 10.00 L vessel is filled with 5.25 moles of Gas A and 2.60 moles of Gas B. What is…

A: According to the ideal gas law, we know that PV = nRT Where P = pressure of the gas V = volume of…

Q: A 320.mol sample of ideal gas is heated in a 2.00L vessel. The pressure in the vessel is 2.50atm.…

A: Initial pressure (P1) = 2.50 atm Initial volume (V1) = 2 L Initial moles of gas (n1) = 320 mol New…

Q: A container has an initial pressure of 2.82 atm and an initial volume of 46.2dL. The final volume is…

Q: A sample of Helium gas is observed to effuse through a pourous barrier in 5.26 minutes. Under the…

A: Given, effusion time He gas =5.26 minuteseffusion time of unknown gas =17.1 minutesboth the gas has…

Q: White phosphorus melts and then vaporizes at high temperature. The gas effuses at a rate that is…

A: The number of atoms in molecule of white phosphorus has to be calculated.

Q: Determine the partial pressure and number of moles of each gas in a 18.50 L vessel at 33.9 °C…

Q: A helium-filled weather balloon has a volume of 882 L at 18.9°C and 757 mmHg. It is released and…

A: Given Data: The initial volume is 882 L. The initial temperature is 18.9°C = 18.9+273 = 291.9 K The…

Q: Determine the partial pressures and the total pressure in a 2.50-L vessel containing the following…

A: Given:Volume of the vessel = 2.5 LThe mixture of gases : 0.0254 mol He, 0.0591 mol H2, and 0.149 mol…

Q: A sample of an unkown gas effuses in 17.42 min. An equal volume of hydrogen gas in the sam apparatus…

A: Given that: Time of effusion of unknown gas = 17.42 min Time of effusion of Hdrogen gas = 2.15 min…

Q: The mass of an evacuated 260 mL flask is 143.217 g. The mass of the flask filled with 268 torr of an…

A: The objective of this question is to calculate the molar mass of an unknown gas given the mass of an…

Q: A vessel contains 15.0 mol of oxygen gas and 15.0 mol of carbon monoxide gas at a temperature of…

Q: A gas of unknown molecular mass was allowed to effuse through a small opening under…

A: Effusion is the process of movement of gaseous molecules through a small hole. The rate of effusion…

Q: A sample of NH3 gas is observed to effuse through a pourous barrier in 3.61 minutes. Under the same…

A: According to Graham’s diffusion law, the rate of effusion of gases is inversely proportional to the…

Q: 2. Carbon monoxide gas effuses from a container in 4.1 minutes. The same quantity of an unknown gas…

A: We will use Grahm Law of effusion for this numerical.

Q: A mixture contains O2 at 700. torr pressure, F2 at 900. torr pressure, and Cl2 at 400. torr…

A: Given that, Pressure of O2=700 torr pressure of F2=900 torr pressure of Cl2=400torr then,

Q: An effusion container is filled with 2 L of an unknown gas. It takes 400 s for the gas to effuse…

A: Volume of an unknown gas effuses in 400 s = 2 LVolume of oxygen gas effuses in 161 s = 2 LMolar mass…

Q: Under identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through…

Q: An unknown perfect gas was detected in the breath of a ferret. It appears to be made entirely of…

Q: Under identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through…

A: To Calculate molar mass of unknown gas , we would use the relation between rate of effusion and…

Q: Three glass bulbs, joined by closed stopcocks, have the following volumes and initial pressures of…

Q: the same barrier. The molar mass of the unknown gas is ____g/mol.

A: We have to find molar mass of the unknown gas

Q: The mass of an evacuated 255 mL flask is 143.187 g. The mass of the flask filled with 267 torr of an…

Q: A sample of N2O gas effuses from a container in 42 seconds.How long would it take the same amount of…

A: A gas law that relates the effusion rates of two gases is Graham's Law of Effusion. According to…

Q: Consider a reaction vessel of fixed volume containing 24.78 grams of nitrogen gas and 12.388 grams…

A: Answer: Final Pressure = 0.755 atm and Final volume = 40.3 L

Q: A mixture of xenon and argon gases, in a 5.91 L flask at 13 °C, contains 43.3 grams of xenon and…

A: Given : 43.3 grams of xenon3.83 grams of argonVolume = 5.91 LTemperature is at 13 °C = 286.15KTo…

Q: Ammonia is formed from nitrogen and hydrogen according to the following unbalanced equation N2 (g) +…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: The total pressure exerted by a mixture of He, Ne, and Ar gases is 2.00atm. What is the partial…

Q: What is the molar mass of the uranium fluoride?

Q: Imagine that you have a 6.50 LL gas tank and a 4.50 LL gas tank. You need to fill one tank with…

Q: Calculate the total pressure of a gas mixture consisting of 3 moles of gas A and 2 moles of gas B,…

A: The ideal gas law is a fundamental equation in physics and chemistry that describes the behavior of…

Q: A sample of SO2 gas is observed to effuse through a pourous barrier in 3.70 minutes. Under the same…

A: Given- Rate of effusion of SO2 gas = 3.70 min Rate of effusion of unknown gas = 1.66 min To find-…

Q: Three glass bulbs, joined by closed stopcocks, have the following volumes and initial pressures of…

Q: A sample of an unknown gas effuses in 11.1 min. An equal volume of H2 (2.016 g mol-1) in the same…

A: Given, Time: Time of unknown gas effuse (tg) = 11.1 min Time of H2 effuse (tH2) = 2.42 min Molar…

Q: A sample of Kr gas is observed to effuse through a porous barrier in 5.98 minutes. Under the same…

Q: A helium-filled weather balloon has a volume of 636 L at 23.9°C and 751 mmHg. It is released and…

A: SOLUTION: Step 1: Conversion of units: P1 =751 mm Hg 1 atm = 760 mm Hg. 751 mmHg= 0.988 atm…

Q: A sample of xenon gas occupies a volume of 6.95 L at 493K. If the pressure remains constant , at…

A: The xenon gas sample is given at - Volume, V1 = 6.95 L Temperature, T1 = 493 K Volume, V2 = 3.77 L…

Q: A mixture of xenon and argon gases, in a 9.94 L flask at 74 °C, contains 23.9 grams of xenon and…

Q: 0.200 g of aluminum reacts 854.0 ml of hydrogen sulphate gas at 30.0 o C and 123.0 kPa, calculate…

A: Mass of aluminium = 0.200 g Volume of H2SO4 = 854 ml = 0.854 L T = 30oC = 303 K P = 123 kPa = 1.214…

Question

A gas of unknown molecular mass was allowed to effuse
through a small opening under constant-pressure condi-
tions. It required 105 s for 1.0 L of the gas to effuse. Under
identical experimental conditions it required 31 s for 1.0 L
of O2 gas to effuse. Calculate the molar mass of the

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1 To Calculate

VIEW

Step 2 Concept

VIEW

Step 3 Formula used and calculations

VIEW

Step 4 Conclusion

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

To what temperature must a sample of nitrogen at 39.2oC and 0.511 atm be taken so that its pressure becomes 1.419 atm at constant volume? Enter C for unit.
A reaction occurs, producing an oxide of nitrogen as a gas. the gas has a mass of 1.211g and occupies a volume of 677mL. the tempurature is 23.0 degrees celcius and the air pressure is 0.987atm. calculate the molar mass of the gas, and the deduce the formula of the gas
A sample of He gas is observed to effuse through a pourous barrier in 5.26 minutes. Under the same conditions, the same number of moles of an unknown gas requires 17.1 minutes to effuse through the same barrier. What is the molar mass of the unknown gas
ASK YOUR TEACHER A gas of unknown molar mass was allowed to effuse through a small opening under constant pressure conditions. It required 3650 s for 1.00 L of this gas to effuse. Under identical experimental conditions it required 471 s for 1.00 L of hydrogen (H2) gas to effuse. Calculate the molar mass of the unknown gas . (Remember that the faster the rate of effusion, the shorter the time required for effusion; that is, rate and time are inversely proportional.) a) The molar mass is 0.3 g/mol.b) The molar mass is 15.6 g/mol.c) The molar mass is 0.7 g/mol.d) The molar mass is 121.1 g/mol.e) The molar mass is 5.6 g/mol.
An effusion container is filled with 2 L of an unknown gas. It takes 400 s for the gas to effuse into a vacuum. From the same container under the same conditions--same temperature and initial pressure, it takes 161 s for 2.00 L of O2 gas to effuse. Calculate the molar mass (in grams/mol) of the unknown gas.
Three glass bulbs, joined by closed stopcocks, have the following volumes and initial pressures of the specified gases.Bulb A: 100. mL of Ne(g) at 190. torrBulb B: 200. mL of He(g) at 1.00 atmBulb C: 500. mL of H2(g) at 50.663 kPaA) After both stopcocks are opened and the gases allowed to diffuse throughout, what will be the final total pressure?(The ambient temperature is constant.)Ptotal = B) What is the partial pressure of He(g)?PHe = C) What is the mole fraction of H2(g)?ΧH2 = (Answer with correct units)
References Use the References to access important values if needed for this question. A sample of NH3 gas is observed to effuse through a pourous barrier in 3.84 minutes. Under the same conditions, the same number of moles of an unknown gas requires 5.73 minutes to effuse through the same barrier. The molar mass of the unknown gas is g mol.
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.
A 30.0 L vessel contains a mixture of carbon dioxide, sulfur trioxide, oxygen, and neon gases at 25.0°C and 2.75 atm. The mole fraction of each gas is 0.25. What mass of each gas is present?
A cylinder containing 244.1 cubic centimeter of gas at a pressure of 307 kPa when its temperature is 549 K. Given that its volume is unchanged when the pressure was increased by a factor of 5, Determine the new Temperature of the gas (In Kelvin).
A cylinder containing 108.5 cubic centimeter of gas at a pressure of 226 kPa when its temperature is 415 K. Given that its volume is unchanged when the pressure was increased by a factor of 7.4, Determine the new Temperature of the gas (In Kelvin).
A sample of O2 gas is observed to effuse through a porous barrier in 7.64 minutes. Under the same conditions, the same number of moles of an unknown gas requires 12.7 minutes to effuse through the same barrier. The molar mass of the unknown gas is g/mol.