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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Ch 7 EOC #8
At atmospheric pressure, a sample of O2 gas has a volume of 47 mL at 27°C. What volume, in milliliters, will the O2 gas occupy if the temperature is decreased to 4°C and the pressure is held constant?
Volume = ______mL
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- E For many purposes we can creat dimethyl ether eat dimethyl ether (C₂H5O) Suppose the pressure on a 130. mL sample of dimethyl ether gas at 4.00°C is doubled. tab aps lock N O STATES OF MATTER Using the combined gas law 60 fn Is it possible to change the temperature of the dimethyl ether at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. Explanation esc K →1 Type here to search ? A Z hp 12 Check 2 W S *si # 3 X alt E f4 $ 4 C R O 15 F do % 40 5 as an ideal gas at temperatures above its boiling point of -24. °C. 100 V f6 - G 17 Y B ♫+ & 7 H no fg N © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Cer a @ IAA * 8 Oyes O no fg °C DII ( M K f10 DDI 12. 1/5 X { insert alt 76°F [ ? 66 prarrow_forwardOxygen gas can be prepared by heating potassium chlorate according to the following equation:2KClO3(s) -> 2KCl(s) + 3O2(g)The product gas, O2, is collected over water at a temperature of 20 °C and a pressure of 748 mm Hg. If the wet O2 gas formed occupies a volume of 5.90 L, the number of grams of O2 formed is __________ g. The vapor pressure of water is 17.5 mm Hg at 20 °C.arrow_forward16.3 L of gas at 33.6 °C and 711 mm Hg are heated to 193 °C, and the pressure is changed to 364 mm Hg. What is the new volume? Volume= _________Larrow_forward
- A mixture of oxygen and helium gases, at a total pressure of 851 mm Hg, contains 6.62 g of oxygen and 0.609 g of helium. What is the partial pressure of each gas in the mixture ? P O2= _____ mm Hg P He= _____ mm Hgarrow_forwardeq req < 1req For each of the following sets of volume/temperature data, calculate the missing quantity after the change is made. Assume that the pressure and the amount of gas remain constant. V=2.30 L at 22.0 °C V = 4.98 L at ? °C PC V = 120. mL at 281 K V = ? mL at 386 K mL V=49.7 mL at 37.0 °C V = ? mL at 357 K a. APR 30 b. C. Submit Answer 2 mL Retry Entire Group Show Hint tv [Review Topics] Ⓒ 9 more group attempts remaining [References] SENSA SPREC ********* Previous Next Save and Exit 3arrow_forwardA cylinder with a movable piston records a volume of 12.8 L when 3.5 mol of oxygen is added. The gas in the cylinder has a pressure of 5.83 atm. The cylinder develops a leak, and the volume of the gas is now recorded to be 12.0 L at the same pressure. How many moles of oxygen are lost? ____ molarrow_forward
- Calculate the volume of a gas in a system when 22.0 g of O2 (Molar mass = 32 g/mol) at a pressure of 12.0 atm is placed in a container at a temperature of 450K. R = 0.0821 L*atm/mol*K Egn PV= nRT O 2.12 L O 8.88 L O 4.24 L O 22.5 L Question 22 4 pts Calculate the density of a gas in a system when O2 (Molar mass = 32g/mol) is placed in a 1.0 Liter container at a pressure of 6.2 atm and at a temperature of 250K. R = 0.0821 L"atm/mol*K O 0.085 g/Larrow_forwardPam The pressure of a sample of gas is measured with an open- ended manometer, shown to the right. The atmospheric pressure is 758 mm Hg. The liquid in the manometer is mercury. What is the pressure of the gas in mm Hg? (1 cm 10 mm) 1. Gas Open end 5.13 cm The total pressure in a tire is 1.20 atm at 23.0 °C. If the temperature is increased to 47.0 °C, what is the new pressure in the 2. tire? Assume the volume of the tire does not change.arrow_forwardPlease don't provide handwriting solutionarrow_forward
- A sample of hydrogen gas occupies a volume of 9.26 L at 55.0°C and 0.950 atm. If it is desired to increase the volume of the gas sample to 11.9 L, while increasing its pressure to 1.32 atm, the temperature of the gas sample at the new volume and pressure must be ______ °C.arrow_forwardWhich of the gases shown here will exert the highest pressure, assuming that each container has the same volume and temperature? (Each symbol represents one mole of the gas.) Select one: Ar a. Ar Rn Rn Rn b. Rn Rn Rn Rn Rn Ne Ne С. Ne Ne Ne Не d. Не Не Не e. All of the samples will exert the same pressure.arrow_forwardAccording to Dalton, the pressure exerted by a gas inside a container is proportional to the number of molecules of that gas. If 4.00 x 1023 molecules of N2 and 2.00 x 1023 molecules of O2 are mixed in a container they exert a total pressure of 1686 torr. What portion of that pressure (in torr units) is exerted by the N2? Report answer to four significant figures in decimal notation. _____________________ torr, What portion of that pressure (in torr units) is exerted by the O2? Report answer to four significant figures in decimal notation. ____________________ torrarrow_forward
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