Use the Maxwell-Boltzmann distribution of speeds to estimate the fraction of CH4 molecules at 298.15 K that have speeds in the range 400 to 600 m.s-1? 0.002- f(v) 0.001- 0.001- 0.001 9-104 7.5-104 6-10 4.5-10 3-10 1.5-104- v (m/s) 200 400 G00 800 1-10 1.2-10 1.4-10 1.6-10* 1.8-10 2-10

Use the Maxwell-Boltzmann distribution of speeds to estimate the fraction of CH4 molecules at 298.15 K that have speeds in the range 400 to 600 m.s-1? 0.002- f(v) 0.001- 0.001- 0.001 9-104 7.5-104 6-10 4.5-10 3-10 1.5-104- v (m/s) 200 400 G00 800 1-10 1.2-10 1.4-10 1.6-10* 1.8-10 2-10

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: A gas has a known value from the van der Waals equation of a= 0.76 m6 Pa mol-2. If the volume of the…

A: Please find your solution below : The compression factor also known as compressibility factor…

Q: 15.0 moles of gas are in a 8.00 L tank at 23.5∘C . Calculate the difference in pressure between…

A: Calculating the Pideal gas:

Q: Which statement is false? O A gas is composed of molecules that are separated from each other by…

A: Postulates of kinetic theory of gases, • Gases are composed of molecules separated from each other…

Q: The partial pressure of the hydrogen gas collected is 0.931 bar. If the total volume of gas…

A: Given data is as follows: The pressure of hydrogen gas = 0.931 bar The volume of hydrogen gas = 728…

Q: Question 33 of 34 Which one of the following gases would be expected to have the highest speed? A)…

Q: For 150 mL of a gas 27°C, what is the temperature at which the volume of the gas becomes 250 mL at…

A: For an ideal gas, there is no attraction force between gaseous molecules. From the ideal gas…

Q: References Use the References to access important values if needed for this question. A 1.97 gram…

A: Given, Mass of sample = 1.97g. Pressure = 692mmHg = 0.911atm. Volume = 1.15L. Temperature = 56oC =…

Q: Constants: R = 0.0821 atmL/molK, 760 mmHg = 1atm Copper (II) sulfıde dissolves in concentrated…

A: Given: The reaction is as follows; 3CuS(s)+8HNO3(aq)---------->3CuSO4(aq)+8NO(g)+4H2O(l). The…

Q: In a sealed and rigid container, a sample of gas at 2.90 atm and 25.0 °C is heated to 50.0 °C. What…

A: From the question we have, P1 = 2.90 atm T1 = 25°C = (25+273) K = 298 K T2 = 50°C = (50+273) K = 323…

Q: Use the van der Waals equation of state to calculate the pressure of 2.60 mol of Cl2 at 469 K in a…

A: The gaseous state is the state of matter with least intermolecular force of attraction between…

Q: Your lungs are 5.23 L and 310.0 K at 1.01 atm. If 80.0% of the air is N2 and 20.0% is O2 what is the…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Consider a state for which the molar volume is 4.00 x 104 m³/mol at 288 K. If the van der Waals…

A: Given that - Molar volume = 4.00×104 m3/mol = 4.00×107 L/mol Temperature = 288 K Vander Wall…

Q: 27. Sodium metal reacts explosively with water to produce sodium hydroxide and hydrogen gas. When…

A: The balanced Chemical equation given in the question is - 2Na + 2H2O -----> 2NaOH + H2…

Q: C6H12O6 (aq) + 6 O2 (g) -------> 6 CO2 (g) + 6 H2O (l) What volume of CO2 will be…

A: To determine the volume of CO2 gas produce by the metabolism of glucose, we have to consider the…

Q: A miniature volcano is made in the laboratory with ammonium dichromate. When ignited, it decomposes…

A: Given:…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

Q: 15. s] The critical constants of ethane are Pc = 48.72 bar, Vc = 145.50 L and Tc = 305.32 K.…

Q: Three gases 8.00g of methane CH4 ,18.0g of ethane,C2H6,and an unknown amount of propane,C3H8)were…

A: First we will calculate the total number of moles of gases using ideal gas equation. Then calculate…

Q: Use the van der Waals equation of state to calculate the pressure ? of 4.00 mol of CH4 at 469 K in a…

Q: At what temperature does 0.030475 moles of Ne in a 932.2 mL container exert a pressure of 0.750 atm?

A: According to ideal gas equation ,we have P×V = n×R×T ------(1) Where P is pressure V is volume n is…

Q: Use the van der Waals equation to calculate the molar volume (L'mol-1) of ethane at 300 K and 200…

A: Van der Waals equation is given as, - (b + RT/P) + (a/P) -ab/P = 0Where,= Molar volume ,a and b are…

Q: Pressure Volume 18 kPa 60.0 ml 21 kPa 50.0 ml 27 kPa 40.0 ml 35 kPa 30.0 ml 54 kPa 20.0 ml…

A: Boyle’s law states that for constant conditions of temperature, the pressure of a gas is inversely…

Q: Which is the best estimate for the number of collisions between a N₂ molecule and other gas…

A: Diameter of N2 molecule, d= 364 pm Pressure, P=1 atm=1.01325 bar Temperature, T=25°C=298 K Molar…

Q: Consider 100.0 mL samples of O2 (g), N₂ (g), and Cl₂ (g) at the same temperature. Which of the…

A: 100.0 mL samples of O2 (g), N2 (g), and Cl2 (g) at the same temperature.

Q: Consider 1.5 mol of methane gas in a 32.414 dm³ vessel at 298 K. The van der Waals constants for…

Q: A sample of dry gas weighing 2.31 grams is found to occupy 2.850 L at 22.0°C and 98.66 kPa. What is…

A: Use ideal gas equation PV = nRT P = pressure of gas V= volume of gas n= no of moles of gas R =…

Q: A certain gas obeys the van-der-Waals equation with a = 0.50 m6 Pa mol-2. Its volume is found to be…

A: Ideal gas law is the equation which obeys gas law under all conditions of temperature and pressure.

Q: A scuba diver that ascends to the surface too quickly can experience decompression sickness, which…

A: Boyle's Law: Boyle's law is an empirical gas law. It describes how the pressure and volume of a…

Q: the pressure of 3.50 x 1022 atoms of Mandonium gas is measured to be 6.1 bar at T = 42oC Calculate…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

Q: A gas-filled weather balloon with a volume of 55.0 L is held at ground level, where the atmospheric…

Q: The experimental Boyle temperature / K 110 327 Gas The a constant of the van der Waals equation /…

Q: Use the van der Waals equation of state to calculate the pressure P of 3.00 mol of CO, at 455 K in a…

A: Van der Waals Equation for gas is [P + (a*n2/V2) ] * [V-n*b] = n*R*T where P is pressure V is…

Q: The critical constants of dichlorodifluoromethane are Tc = 111.5 °C, Pc = 39.6 atm and dc = 0.555…

A: The answer to the following question is-

Q: A certain gas obeys the van-der-Waals equation with a = 0.50 m6 Pa mol-2. Its volume is found to be…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A: Given that The van der Waals equation of state for real gas as (P+an2V2) (V-nb) =nRT where P =…

Q: At 300K, the virial coefficients (B) of N2 and CH4 are -4.2cm^3 mol^-1 and -15cm^3 mol ^-1,…

A: The virial equation for 1 mole of real gas is given below where B and C are the second and third…

Q: 10. In alcohol fermentation, yeast converts glucose to ethanol and carbon dioxide: C6H1206 (s)…

A: Given mass of glucose = 4.26 g Molar mass of glucose = 180.16 g.mol- Volume of carbon dioxide =…

Q: A mixture containing 1.58 g CO (g) and some CO2 (g) occupies a 7.24-L vessel at 42°C. The pressure…

Q: What pressure does the gas exert if the temperature changes from T1 = 600. K to T1 = 300. K, while…

A: According to Gay-Lussac's law, at constant volume pressure increases, temperature increases.

Q: References) Ethane burns in air to give H,0 and CO, 2 C,Ha(g) +7O,(8) 4 CO, (8) + 6 Hạ0(g) a What…

A: From ideal gas behavior at constant temperature and pressure – PV = nRTVn = RTPVn =constantV1n1…

Q: 6.407 g of solid CO2 (44.01 g/mol) is put in an empty sealed 3.45 x 103 mL container at a…

A: Given data in above Mass of CO2 (w) = 6.407 g Molar mass of CO2 (M)= 44.01 g/mol Volume of…

Q: Calculate pressure in atm exerted by 3 mol of CO2 behaving as a van der Waals gas in a 22.414 L…

A: 3 mol of CO2 gas in 22.414 L vessel at 273.15 K temperature behaves as a van der waal gas .a =…

Q: If you collect 45.0mL of gas at 22.0°C, through water and the total pressure of the mixture of H2…

A: Given data,Volume=45.0mLTemperature=22.0oCTotal pressure=0.9825atm

Question

v1+ v2
L:=f|
- (2–v1)
2
Use the Maxwell-Boltzmann distribution of speeds to estimate the fraction of CH4 molecules
at 298.15 K that have speeds in the range 400 to 600 m.s-1?
0.002- f (v)
0.001-
0.001-
0.001
9.104
7.5-10–4
G-104
4.5-104
3-104
1.5-104
v (m/s)
200
400
G00
800
1-10
1.2-10*
1.4-10
1.6-10
1.8-10*
2.10

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 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

Constants R = 0.0821atmolmolK . 1atm = 760mmHs , 1 gas = 22.41 (STP) Hydrogen was prepared in 1776 by a method given by the following equation. What volume (L ) of H 2 at 745 mmHg and 20°C can be prepared from 4.8 g of iron? 4H 2 O(g)+3Fe(s)--> Fe 3 O 4 (s)+4H 2 (g)
The ideal gas law is a limiting law, in that it is expected to hold as pressure approaches zero. Suppose the following measured values have been obtained for oxygen gas at 273.15K. Based on the data, calculate R for each pressure value and create a table of pressure and R values (i.e. you are treating R as a variable rather than a constant at this point). Then create a plot R vs p and find the “best value” of R by determining the y-intercept of a straight line fit. (Be sure to label your axes including units).
An important process for the production of acrylonitrile (C3H3N) is given by the following equation: 2C3H6(g) + 2NH3(g) + 302(g) - 2C3H3N(g) + 6H20(g) A 150.-L reactor is charged to the following partial pressures at 25°C: Pc3H6 = 0.500 MPa PNH3 =5 0.800 MPa Poz = 1.500 MPa What mass of acrylonitrile can be produced from this mixture (MPa = 106 Pa)? %3D 1.61 x 10 g C3H3N 1.61 x 10 g C3H3N 2.87 x 10 g C3H3N 1.00 x 10 g C3H;N
Chemistry A certain gas obeys the Van der Waals equation with a = 0.500 Pa m6 mol-2, and with molar volume equal to 5.00 x 10-4 m3 mol-1 at 273.15 K and 3.00 MPa. (a) Calculate the value of the Van der Waals constant, b. (b) Calculate the value of the compression factor Z under these conditions. (c) Do attractive or repulsive forces dominate?
A sealed container holding 0.0255 L0.0255 L of an ideal gas at 99.526 kPa99.526 kPa and 73 °C73 °C is placed into a refrigerator and cooled to 37 °C37 °C with no change in volume. Calculate the final pressure of the gas.
A chamber filled with N₂ molecules is at a low pressure of 48 Pa but high temperature of 800 K? If there is a small hole of diameter 3.0 mm on the wall of the chamber, how many N₂ molecules would effuse out per second? It is known that the molecular weight of N₂ is 28. Also recall that the area of a circle is xr², where r is the radius. Note that the answer is a big number. Submit the answer in E notation, e.g., 5.4x1012 should be entered as 5.4E12. Round the coefficient of the answer to one decimal place. Hints: 1. The number of molecules effusing out of a small hole per second is known as the effusion rate. 2. The effusion rate is the product of the molecular flux and the area of the hole. 3. Find the formulas in the notes of Unit 2.3 to solve the problem.
An average gas fireplace uses about 200 gallons (760,000 cm3) of propane gas per year. Assume that the propane, C3H8, behaves as a perfect gas for the conditions of this problem, which are 1.00 atm and 22°C. What is the mass of gas used?
At 298K, N2 molecules have a mean speed of 475 m/s. As a consequence, the probability to randomly pick 1 molecule at 475.00 m/s is extremely high. Select one: True False
Based on their respective van der Waals constants, which of these two gases: Xe (a = 4.137 L² atm mol-2, b = 0.0516 L mol-1) or CO2 (a = 3.610 L²atm mol-2, b = 0.0429 L mol-1) is expected to behave more nearly like an ideal gas at high pressures? Explain.
Gaseous neon is observed to effuse through a tiny hole at a rate of 1.90 cm3/min. An unknown gas is observed to effuse through the same tiny hole under the same conditions of temperature and pressure, at a rate of 1.05 cm°/min. What is the molar mass of the unknown gas?
Ammonia, NH3, may react with oxygen to form nitrogen gas and water. 4 NH₂(aq) + 30₂(g) →→→ 2N₂(g) + 6H₂O(1) If 3.95 g NH3 reacts with 5.93 g O₂ and produces 0.850 L. N₂ at 295 K and 1.00 bar, how many moles of N₂ can be produced by each reactant? It may be useful to consult the periodic table. NH₂: 0₂: Based on the theoretical yields, which reactant is limiting? NH,(aq) 0₂(g) What is the percent yield of the reaction? percent yield: mol N₂ mol N₂ 28
A helium-filled balloon accidentally floats to the ceiling. The balloon is initially inflated to a radius of 6 inches (assume a sphere). The balloon’s empty mass is 10 g. The density of the rubber is 0.8 g/cm3. The contents of the balloon are purely helium @ p=1 atm, T=300 K. Assume that D=3.00E-8 kg/m2s and assume the pressure inside the balloon does not change much. Calculate the time required for the balloon to start to sink on its own, because of diffusion.