For a gas sample whose total pressure is 720 torr, what are the partial pressures if the gas present consists of 1.1 mol of N₂, 0.36 mol of O₂, and 0.061 mol of Ar? Partial pressure of N2 = torr Partial pressure of O2 = torr Partial pressure of Ar = torr

For a gas sample whose total pressure is 720 torr, what are the partial pressures if the gas present consists of 1.1 mol of N₂, 0.36 mol of O₂, and 0.061 mol of Ar? Partial pressure of N2 = torr Partial pressure of O2 = torr Partial pressure of Ar = torr

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: and 0.723 atm. If 0.140 mol of a third gas is added with no change in volume or temperature, what…

Q: A mixture of gasses contains 4.64 mol Ne, 0.748 mol Ar, and 2.59 mol Xe. What is the partial…

Q: Some N₂ gas is mixed with some O, gas, and the sketch below shows a representative sample of the…

Q: A mixture of gases contains 313 torr N2, 275 torr O2, and 286 torr Ar. What is the total pressure of…

Q: A sealed container contains argon, xenon, and helium gases. If the total pressure of the mixture is…

A: Dalton's law: Dalton's law of partial pressures states that in a mixture of non-reacting gases, the…

Q: A gas cylinder contains 2.2 mol of N2, 3.3 mol of O2 and 4.4 mol of Cl2. What is the partial…

A: The partial pressure (Pa) of a gas 'a' in a mixture is given by: Pa=χa×PT Here PT is the total…

Q: At 8°C a 1.0-L flask contains 1.0 x 10-2 mole of N2, 4.0 x 102 mg O2, and 4.7 x 1021 molecules of…

Q: At 2°C a 1.0-L flask contains 1.0x 10^-2 mole of N2 , 4.0x10^2 mg O2 , and 5.1x 10^21 molecules of…

A: N2 = 1.0x 10^-2 mole = 0.01 mole O2 = 4.0x10^2 mg =400 mg =0.4 g O2 = 0.4 g / 32g/mol = 0.0125…

Q: The molecular-level representation of a mixture of gases A, B and C is shown to the below. The…

A: The partial pressure of gas C is = 39.7 kPa The mole fraction of gas C =? The total pressure in kPa…

Q: A chemist has a gaseous mixture of N2, 02, and argon that has a total pressure of 716 torr. In this…

Q: An aqueous chemical reaction produces hydrogen gas with a total pressure of 295.0 torr at 17.5 °C in…

A: Given: Total pressure = 295.0 torr Vapor pressure of H2O = 15.0 Partial pressure of H2 = ?

Q: A mixture of gases contains 1.01 g of N2, 6.45 g of H2, and 2.04 g of NH3. If the total pressure of…

A: Number of moles of N2 gas = given mass/molar mass =(1.01 g ÷ 28 g/mol) = 0.036 mol Number of moles…

Q: A gas sample is collected in a 0.249 L container at 28.1 °C and 0.912 bar. If the sample has a mass…

A: Using law of Ideal gas, we can determine the moles of gas present in the sample. Ideal gas law- PV…

Q: A gas mixture contains 0.35 moles of Ne, 0.10 moles of He, and 0.39 moles of Ar. If the total…

Q: A gas mixture with a total pressure of 4.6atm is used in a hospital. If the mixture contains 5.4 mol…

Q: A mixture of neon and hydrogen gases contains neon at a partial pressure of 231 mm Hg and hydrogen…

Q: A mixture of hydrogen and carbon dioxide gases contains hydrogen at a partial pressure of 420 mm Hg…

Q: A gaseous mixture is made by mixing Gas A and Gas B together. The mixture is 58.2 mole % of Gas A.…

A: Given, Mol % of gas A = 58.2 % Total pressure of the mixture = 3.52 atm Pressure of gas B in the…

Q: Suppose that Daniel has a 2.00 L bottle that contains a mixture of O2, N2, and CO2 under a total…

A: The objective of this question is to find the partial pressure of O2 in a mixture of gases. The…

Q: You are given two closed 1.0 L flasks (A and B) connected by a stopcock, both at room temperature…

Q: A flask contains a mixture of 3.20 mol He and 3.61 mol Ne gases. Determine the partial pressure of…

A: Given :- No.of moles of He = 3.20 mol No.of moles of Ne = 3.61 mol Total pressure = 697 mm Hg To…

Q: A sample of air from a home is found to contain 8.2 × 10-6 of carbon monoxide. This means that if…

A: Given information, Mole fraction of carbon monoxide (CO) = 8.2*10-6 Total pressure = 735 torr

Q: A commercial mercury vapor analyzer can detect, in air, concentrations of gaseous Hg atoms (which…

Q: At 118oC, the pressure in a 12.0 L flask is 847 mm Hg. How many moles of gas are in the flask?

A: The ideal gas equation is shown below:P V = n R T Where; P = pressure of the gas V= volume of the…

Q: A gas storage cylinder in an ordinary chemical laboratory measures 3.0 cm wide and 12.cm high.…

A: Width of gas storage cylinder d = 3.0 cm Height of gas storage cylinder h = 12 cm Initial pressure…

Q: Find the partial pressure (in torr) of each gas in the mixture.

A: Partial pressure of any gas in a mixture of non reacting gases is defined as mole fraction of gas x…

Q: container was filled with 0.893 moles of N2, 0.687 moles of O2, 0.734 moles of H2, and 0.248 moles…

Q: Summarize each of the simple gas laws (Boyle’s law, Charles’s law, and Avogadro’s law). For each,…

Q: A commercial mercury vapor analyzer can detect, in air, concentrations of gaseous Hg atoms (which…

Q: The gaseous composition of exhaled breath of air by number an analysis of the number of moles is…

A: We have the following formula, 1. Partial pressure = mole fraction x total pressure 2. mole fraction…

Q: ntainer holds 3 gases: oxygen, CO2, and He. The partial pressure of the 3 gases are 2.00atm,…

Q: A 25.5 mL sample of CO, gas at 855 torr and a temperature of 25.00 °C is heated at constant pressure…

A: Given : volume of sample =V1= 25.5ml Pressure =855 torr Temperature (T1)= 298K T2 = 648 To…

Q: A mixture of gases at fixed volume and temperature contains 1 mole of He gas and an unknown amount…

Q: A mixture of He, Ne, and Ar has a pressure of 29.5 atm at 28.0 ∘C. If the partial pressure of He is…

A: According to the Dalton's Law of partial pressure the sum of all the partial pressure of gases is…

Q: A gaseous mixture containing 16.0 g O2, 6.00 g H2, and 4.00 g He is placed into an 8.0 L vessel at 5…

Q: At 750 K, a 296 mL container of Xe at 3.02 atm is connected by a valve to a 441 mL container of H2…

A: Ideal gas eequation can be written as: Here, P- pressure of gas V- volume of gas n- number of moles…

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

For a gas sample whose total pressure is 720 torr, what
are the partial pressures if the gas present consists of
1.1 mol of N₂, 0.36 mol of O₂, and 0.061 mol of Ar?
Partial pressure of N2
=
torr
Partial pressure of O2
=
torr
Partial pressure of Ar =
torr

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 3 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

A mixture of gases with a pressure of 800 mm Hg contains 10% oxygen and 90% nitrogen by volume. What is the partial pressure of the oxygen gas in the mixture? 10 mm Hg O 80 mm Hg O 700 mm Hg O 800 mm Hg
A gas mixture contains 0.600 mol of N2, 0.200 mol of H2, and 0.250 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 9.00 L vessel at 27.00°C. What is the total pressure of the vessel and the pressure of N2, H2, and CH4 in atm?
A gaseous mixture contains 12.4 g of N2 and 12.4 g of 02 that exerts a total pressure of 1.23 atm. What will the be the partial pressure of N2 in the mixture? 0.615 atm O 0.656 atm O 0.375 atm O 0.885 atm
The mass percent of a three component gas sample is 6.40% C2H4, 38.2% C4H8 and 55.4% N2H4. Calculate the partial pressure (torr) of C2H4 if the total pressure of the sample is 258.4 torr.
Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 800. torr. gas N₂ 0₂ carbon nitrogen oxygen 0 Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. mole fraction partial pressure torr key torr hydrogen x sulfur chlorine X S OL A
A sample contains 2.0 moles of He gas and 6.0 moles of Ar gas. What is the mole fraction of He gas (XHe)? 0.33 0.75 0.25 2.0
A gas sample containing only BF3, SO2 and S2F2 has the following mass percent composition: 44.3% BF3 and 13.3% SO2. Calculate the partial pressure (torr) of SO2 if the total pressure of the sample is 1.90 atm.
26. Consider the following balanced reaction: ( 2CH10 + 1302→ 8CO2 + 10H20 Substance Molar Mass (g/mol) 58.14 CH30 If 29.3 g Oz completely reacted, and all of the dry CO2 gas was stored in a 27.0 L container at 65 F, what would be the 32.00 CO2 44.01 pressure of the COz gas in torr? H20 18.02
se What is the partial pressure of Ar if the total pressure is 722 mmHg and it is 35% of the mixture? O 211 mmHg
A mixture of He, Ne, and Ar has a pressure of 23.3 atm at 28.0 °C. If the partial pressure of He is 4.37 atm and the partial pressure of Ar is 1.61 atm, what is the partial pressure of Ne? PNe atm