困Based from the given critical temperature values in the table, rank the followingcompounds according to the strength of intermolecular attractive forces. *1- STRONGEST2345- WEAKESTNitrogenHydrogenCarbonmonoxideОхудenMethaneWhat is the relationship between critical temperature and intermolecular forces ofattraction? *InverseO Direct|4:52 pmP Type here to searcha 4) ENG23/10/2021O OO O O近 Table of Critical Temperature and Critical PressureProduct componentsCriticalCriticalTemperature, Pressure(К)(MPa)1.296HydrogenNitrogenCarbon monoxide33.145126.193.396132.863.444Охygen154.605.013Methane190.564.5994:48 pmO Type here to searcha 1) ENG23/10/2021近

The critical temperature signifies the force of attraction between the molecules. The higher the…

Answered: Based from the given critical…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter5: Gases

Section: Chapter Questions

Problem 5CO: perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.

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5-25 A gas in a bulb as in Figure 5-3 registers a pressure of 833 mm Hg in the manometer in which the reference arm of the U-shaped tube (A) is sealed and evacuated. What will the difference in the mercury levels be if the reference arm of the U-shaped tube is open to atmospheric pressure (760 mm Hg)?
One of the chemical controversies of the nineteenth century concerned the element beryllium (Be). Berzelius originally claimed that beryllium was a trivalent element (forming Be3+ ions) and that it gave an oxide with the formula Be2O3. This resulted in a calculated atomic mass of 13.5 for beryllium. In formulating his periodic table, Mendeleev proposed that beryllium was divalent (forming Be2+ ions) and that it gave an oxide with the formula Be2O3. This assumption gives an atomic mass of 9.0. In 1894, A. Combes (Comptes Rendus 1894, p. 1221) reacted beryllium with the anion C5H7O2and measured the density of the gaseous product. Combess data for two different experiments are as follows: I II Mass 0.2022 g 0.2224 g Volume 22.6 cm3 26.0 cm3 Temperature 13C 17C Pressure 765.2 mm Hg 764.6 mm If beryllium is a divalent metal, the molecular formula of the product will be Be(C5H7O2)2; if it is trivalent, the formula will be Be(C5H7O2)3. Show how Combess data help to confirm that beryllium is a divalent metal.
In dry atmospheric air, the four most abundant components are N₂, X = 0.808; O₂, X = 0.1915; Ar, X = 9.34x10-5; and CO₂, X = 4.066x104. Calculate the partial pressure of CO₂, in torr, under standard atmospheric conditions. Submit Answer Tries 0/99 This discussion is closed. M CAL 8:00- 10:50- CI 12:00 Q ! 2 @ W OCT 21 F2 # 3 E 80 F3 $ 4 R 10 Q F4 % 5 T F5 A 6 Y F6 tv A S MacBook Air & 7 8 F7 8 DII FB ( 9 F9 O ) 0 J F10 F11 + F12 Send Feedback
Determination of the Universal Gas Constant Postlab 1. An evaluation of Rwas performed using the procedures outlined in this exercise, The barometric pressure was 735 torr and the temperature was 21.5 "C. The volume of H2(9) collected was 32.7 mL. The calculated value of Rwas 0.0817 L'atm/mol-K. a. How many grams of Mg metal were used in this determination? 0.0316 70.361 b. If the correction for the vapor pressure of water had not been performed, what would be the calculated value of R? Incorrect c. If the syringe volume had been incorrectly read, resulting in a calculated H, volume of 30.6 mL, what would be the percent error in the calculated value of Rwith respect to the originally calculated value (0.0817 L-atm/mol·K)? 6.4 %
The student from question 3 then heated the beaker of water and found that at 75 °C the corrected volume of the bubble was 4.05 mL. What should she report as the vapor pressure of water PH2O) at this temperature? Answer from question 3= 0.000095 moles of trapped air This was also the question for 3 just in case you needed it for information: A student found that at 755 torr atmospheric pressure and 0.2 °C, the corrected volume of the trapped air was 2.15 mL. Under these conditions, how many moles of trapped air nair are present?
In Part B, you used a similar procedure to that of Part A to determine the mass percent of CaCO3 in an antacid tablet. The commercially accepted range of CaCO3 in an antacid tablet is 25–35% by mass. Miranda obtained the data below from her Part B trial: TRIAL PRESSURE (torr) MASS OF TABLET (g) TEMPERATURE (°C) VOLUME CO2 RECOVERED (mL) 1 750.5 0.5702 21.3 69.6 2 750.5 0.5622 21.2 68.2 Miranda determined her average % Recovery of CO2 to be 65.0% from Part A. Based on her data collected from Part A, was the average percent mass of CaCO3 in her antacid tablet within the commercially accepted range? Yes, her mass percent does fall within the commercially accepted range. No, her mass percent does not fall within the commercially accepted range.
Water Vapor pressure at 23c is 21.7 mmHG
(a) From the temperature-pressure data graphed in Part A, visually determine the gas pressure at a temperature of 350 K, including units. (b)From the temperature-pressure data graphed in Part A, determine the equation of the line of best fit. (C) What are the units for the slope of the line of best fit determined in question 2? (D) From the equation of the line of best fit determined in Question 2, algebraically determine the gas pressure at a temperature of 350 K, including units and a unit analysis.
a) From the temperature-pressure data graphed in Part A, visually determine the gas pressure at a temperature of 350 K, including units. (b)From the temperature-pressure data graphed in Part A, determine the equation of the line of best fit. (C) What are the units for the slope of the line of best fit determined in question 2? (D) From the equation of the line of best fit determined in Question 2, algebraically determine the gas pressure at a temperature of 350 K, including units and a unit analysis. Note: I only need su part D solve please
Thank you
om.google.com/u/1/w/Mzg1MzgyNTkwMDQy/t/all Partial Pressure Assessment 85. Consider the flasks in the following diagram. What are the fi- nal partial pressures of H, and N, after the stopcock between the two flasks is opened? (Assume the final volume is 3.00 L.) What is the total pressure (in torr)? 2.00 L H- 1.00 L N, 475 torr 0.200 atm. (1 atm- 760 torr) Page
Composition of Dry Air at Sea Level Gas Mole% N2 78.084 O2 20.946 Ar 0.934 CO2 0.0345 Ne 0.00182 He 0.000524 CH4 0.000168 Kr 0.000114 Using data from the above table, calculate the partial pressure of CO2 when the atmospheric pressure is 1.06 atm.At the same atmospheric pressure, if the temperature is 10°C, how many CO2 molecules would there be in 850 mL?

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