1.1(a) A sample of air occupies 1.0 L at 25 °C and 1.00 atm. What pressure is needed to compress itto 100 cm’ at this temperature?1.2(a) A perfect gas undergoes isothermal compression, which reduces itsvolume by 2.20 dm³. The final pressure and volume of the gas are 5.04 barand 4.65 dm', respectively. Calculate the original pressure of the gas in (a) bar,(b) atm.1.3(a) To what temperature must a 1.0 L sample of a perfect gas be cooled from 25 °C in order toreduce its volume to 100 cm³?1.4(a) A sample of 255 mg of neon occupies 3.00 dm at 122 K. Use the perfectgas law to calculate the pressure of the gas.1.7(a) In an attempt to determine an accurate value of the gas constant, R, astudent heated a container of volume 20.000 dm³ filled with 0.251 32 g ofhelium gas to 500°C and measured the pressure as 206.402 cm of water in amanometer at 25°C. Calculate the value of R from these data. (The density ofwater at 25°C is 0.997 07 g cm; the construction of a manometer is describedin Exercise 1.6a.)

Answered: Image /qna-images/answer/81d9c2dd-5f39-425a-ac56-af2980c44832.jpg

Answered: 1.1 (a) A sample of air occupies 1.0 L…

1.1 (a) A sample of air occupies 1.0 L at 25 °C and 1.00 atm. What pressure is needed to compress it to 100 cm at this temperature?

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

0.374 m3 of hydrogen was observed at −7.0 oC and atmospheric pressure (105 Pa). The relative molecular mass of hydrogen is 2.02 g mol-1 and the gas constant, R, is 8.314 J K−1 mol−1 a) Calculate the number of moles (round to 2 decimal places): b) Calculate the mass of the gas in g (round to 3 significant figures):
Calculate the absolute pressure at an ocean depth of 2.8 km. Assume that the density Water, Pwater is 1.025 × 10³ kg/m³ and the atmospheric pressure, Patmosphere 1.01 x 105 Pa. (Use: acceleration due to gravity, g= 9.8 m/s²) ma Counsellor
Qq.66. Subject :- Chemistry
If the atmospheric pressure is 750 mm Hg, and the air is 22% oxygen, 77% nitrogen, and the rest carbon dioxide, what is the partial pressure of oxygen? Round your answer to the nearest integer value in mm Hg.
Using (a) the ideal gas law and (b) the van der Waals equation, calculate the pressure exerted by 50.0 g carbon dioxide in a 1.00-L vessel at 25°C. Do attractive or repulsiveforces dominate?
Give two cases where the assumptions of kinetic molecular theory break down. Choose one of the two cases and describe what assumption(s) of kinetic molecular theory fail and how will the ideal gas law fail to describe the behavior of the real gas. (Explain with complete sentences).
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
A 0.350 g sample of nitrogen gas (N₂) at 90.5 K exerts a pressure of 55.0 kPa. What volume will it occupy?
Gas volume in the lungs after exhalation is 3.4 L. The pressure after exhalation matches atmospheric pressure, 1.0 atm. The temperature is at the core human temperature of 37.0 °C. (a) How many moles and molecules of gas are present in the lungs? (b) Using gas under the same conditions (but not in the lungs) , what would be the final temperature if the gas pressure was raised to 1.8 atm and the volume was reduced to 3.1 ×10^-3 m3 ?
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.
1A.10 Balloons are still used to deploy sensors that monitor meteorological phenomena and the chemistry of the atmosphere. It is possible to imvestigate some of the technicalities of ballooning by using the perfect gas law. Suppose your balloon has a radius of 3.0 m and that it is spherical. (a) What amount of H, (in males) is needed to inflate it to 1.0atm in an ambient temperature of 25 °C at sea levd? (b) What mass can the balkoon lift at sea level, where the density of air is 1.22 kg m? (c) What would be the payload if He were used instead of H? perature on asured one eam is
9) A 0.780 L flask is filled with 2.88 mol of acetylene gas (C2H2). Given that the pressureexerted by the gas is 3.60 atm, calculate its temperature.