Question 6:Chlorine is widely used to purify municipal water supplies and to treat swimming poolwaters. Suppose that the volume of a particular sample of Cl₂ gas is 8.70 L at 895 torrand 24°C.(a) How many grams of Cl₂ are in the sample?⚫ Atomic mass of CI = 35.453 g/mol• Molar mass of Cl₂ = 2 x 35.453 = 70.906 g/molSolution:Use the Ideal Gas Law:Step 1: Convert Given Values• Pressure: P = 895 torr → atmPV== nRT1P = 895 ×= 1.1789 atm760•Temperature: Convert to Kelvin:T24273.15 = 297.15 K• Gas constant: R = 0.0821 L atm/mol. KVolume: V = 8.70 LStep 2: Solve for n.PVn =RTn =(1.1789)(8.70)(0.0821)(297.15)10.25n == 0.420 mol24.405Step 3: Calculate Mass of Cl₂Final Answer: 29.78 g of Cl₂.mass nx Mmass=(0.420)(70.906)mass=29.78 g (b) What volume will the Cl₂ occupy at standard temperature andpressure (STP)?STP Conditions:⚫ P = 1.00 atm•T = 273.15 KUsing Ideal Gas Law:Final Answer: 9.42 L at STP.nRTV=P(0.420) (0.0821) (273.15)V =1.009.42V == 9.42 L1.00Final Summary of Answers:1. Final volume of SO3: 25.0 mL2. Final volume of the bubble: 0.0117 L3. (a) Mass of Cl2: 29.78 g4. (b) Volume of Cl₂ at STP: 9.42 L

Question 6aGiven the following values:volume, V = 8.70 Lpressure, P = 895 torr = 1.17895…

Answered: Question 6: Chlorine is widely used to…

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter12: The Laws Of Thermodynamics

Section: Chapter Questions

Problem 72AP

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When a certain gas under a pressure of 5.00 106 Pa at 25.0C is allowed to expand to 3.00 times its original volume, its final pressure is 1.07 106 Pa. What is its final temperature? (a) 450 K (b) 233 K (c) 212 K (d) 191 k (e) 115 K
Unreasonable results. (a) Find the sped of hydrogen sulfide, H2S, molecules at a temperature of 250 K. Its molar mass is 31.4 g/mol (b) The result isn't very unreasonable, but why is it less reliable than those for, say, neon or nitrogen?
(a) Estimate the specific heat capacity of sodium from the Law of Dulong and Petit. The molar mass of sodium is 23.0 g/mol. (b) What is the percent error of your estimate from the known value, 1230 J/kg ? `
(a) Using data from the previous problem, find the mass of nitrogen, oxygen, and argon in 1 mol of dry air. The molar mass of N2 is 28.0 g/mol, that of O2 is 32.0 g/mol, and that of argon is 39.9 g/mol. (b) Dry air is mixed with pentane 5 H12, molar mass 72.2 g/mol), an important constituent of gasoline, in an air-fuel ratio of 15:1 by mass (roughly typical for car engines). Find the partial pressure of pentane in this mixture at an overall pressure of 1.00 atm.
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The active element of a certain laser is made of a glass rod 30.0 cm long and 1.50 cm in diameter. Assume the average coefficient of linear expansion of the glass is equal to 9.00 106 (C)1. If the temperature of the rod increases by 65.0C, what is the increase in (a) its length, (b) its diameter, and (c) its volume?
When a certain gas under a pressure of 5.00 106 Pa at 25.0C is allowed to expand to 3.00 times its original volume, its final pressure is 1.07 106 Pa. What is its final temperature? (a) 450 K (b) 233 K (c) 212 K (d) 191 K (e) 115 K
The air we breathe is largely composed of nitrogen (N2) and oxygen (O2) molecules. The mass of an N2 molecule is less than the mass of an O2 molecule. (a) For air at 300 K, is the average kinetic energy of an N2 molecule greater than, less than, or equal to the average kinetic energy of an O2 molecule? (b) Is the rms speed in air of an N2 molecule greater than, less than, or equal to the rms speed in air of an O2 molecule?
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The escape velocity from the Moon is much smaller than that from the Earth, only 2.38 km/s. At what temperature would hydrogen molecules (molar mass is equal to 2.016 g/mol) have a root-mean-square velocity vrms equal to the Moon's escape velocity?
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(a) Hydrogen molecules (molar mass is equal to 2.016 g/mol) have vrms equal to 193 m/s. What is the temperature? (b) Much of the gas near the Sun is atomic hydrogen (H rather than H2). Its temperature would have to be 1.5107 K for the speed vrms to equal the escape velocity from the Sun. What is that velocity?

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