Calculate the total pressure (in atm) of a mixture of 0.0200 mol of helium, He, and 0.0100 mol of hydrogen, H2, in a 1.50 L flask at 10°C. ASsume ideal gas behavior. Given that R = 0.0821 L-atm/(mol·K). a. 0.349 atm. O b. 0.697 atm. c. 0.465 atm. d. 0.279 atm. e. 1.39 atm.

Calculate the total pressure (in atm) of a mixture of 0.0200 mol of helium, He, and 0.0100 mol of hydrogen, H2, in a 1.50 L flask at 10°C. ASsume ideal gas behavior. Given that R = 0.0821 L-atm/(mol·K). a. 0.349 atm. O b. 0.697 atm. c. 0.465 atm. d. 0.279 atm. e. 1.39 atm.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter9: The Gaseous State

Section: Chapter Questions

Problem 40P

See similar textbooks

Related questions

Q: Find the temperature (in °C) at which 2.10 moles of chlorine gas filled in a 25.0L cylinder will…

A: Ideal gas equation: PV = nRT 1.25 x 25.0 = 2.10 x 0.0821 x T T = 181.25 K T = 181.25 - 273.15 oC…

Q: The temp of an ideal gas in a 5 . 00 L container originally at 1 . 0 atm pressure and 2 5 C is…

Q: What quantity in moles of chlorine gas at 120.0C and 33.3 atm would occupy a vessel of 25.0L?

A: Given, The moles of chlorine gas at 120.°C and 33.3 atm that would occupy 25.0 L of vessel is:

Q: An ideal gas originally at 0.85 atm and 62°C was allowed to expand until its final volume, pressure,…

A: Given,Initial pressure, P1 = 0.85 atmInitial pressure, T1 = 62 oC = (62 + 273.15) K = 335.15…

Q: A mixture containing 0.250 mol N2 (g), 0.150 mol CH4 (g), and 0.100 mol O2 (g) is confined in a 1.00…

A: Given: moles of N2 = 0.250 mol moles of CH4 = 0.150 mol moles of O2 = 0.100 mol Temperature = 35 oC…

Q: When a supply of hygrogen gas is held in a 4L container at 320K it exerts a pressure of 800 torr.…

Q: An equimolar (i.e. containing same molar amount) mixture of O2, N2, Kr, and CO2 gases is placed in a…

A: The Scottish physical chemist Thomas Graham gives direct relation between rate of effusion of gas…

Q: Many water treatment plants use chlorine gas to kill mi-cro organisms before the water is released…

A: From ideal gas law, PV = nRT , P = (80 / 100 ) × 85 = 68 atm, T = 298 K , R = 0.082 L , V = 850 L…

Q: An ideal gas originally at 0.85 atm and 65°C was allowed to expand. until its final volume,…

A: Ideal gas law , Ideal gas law state the relation between the pressure, temperature, volume and…

Q: A mixture of hydrogen gas and oxygen gas exerts a total pressure of 3.0 atm on the walls of its…

A: Given total pressure = 3.0 atm Partial pressure of hydrogen = 1.65 atm Mole fraction of oxygen can…

Q: A gaseous compound has a density of 1.12 g/L at 23.3 °C and 1.11 atm. What is the molar mass of the…

Q: The flame produced by the burner of a gas (propane) grill is a pale blue color when enough air mixes…

Q: A 0.11 g of H2O2(l) decomposes to O2 (g) and H2O(g) in a 2.5L flask at 25C? What is the pressure for…

A: Given:Mass of H2O2 = 0.11 g.Volume of flask = 2.5 L.Temperature = 25 oC = 298 K.Chemical reaction of…

Q: A mixture of 3.00 moles of neon gas and 4.00 moles of nitrogen gas, N2, occupy a vessel where the…

A: daltons law of partial pressures P total=P neon + P N2 Partial pressure = P total ×mole fraction…

Q: 1. Given the reaction: 2 Al (s) + 6 HCl (aq) --> 2 AlCl3 (aq) + 3 H2 (g) A strip…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: The following chemical reaction represents the combustion of sugar. C6H12O6(s) + 6 O2(g) → 6 CO2(g)…

Q: 1. Mass of flask, foil, rubber band 66.3842_ g 2. Temperature of boiling water 95.60 wou 3.…

A: Acc. to Ideal gas Equation P*V = n * R *…

Q: The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of…

Q: Suppose you are given two 1-L flasks and told that one contains a gas of molar mass 30, the other a…

A: From ideal gas equation,

Q: What is the volume(in L) of carbon dioxide at 1.00atm and 298.15 k are released from a car's engine…

A: Here pressure of the car engine is fix at 1 atm. So Charle's law is applicable here. According to…

Q: For the given reaction, what volume of Br2 would be required to react with 6.4Lof NO, measured at…

A: The given reaction is

Q: A gas mixture consists of 0.421 mol hydrogen (H2), 0.664 mol carbon dioxide (CO2), and 1.965 mol…

A: Given :- Number of moles of H2 = 0.421 mol Number of moles of CO2 = 0.664 mol Number of moles of…

Q: A gas originally at 25oC and 1.50 atm pressure in a 2.3 liter container is allowed to expand until…

Q: The density of an ideal gas at STP is found to be 1.94 g/L . What is its molar mass? molar mass:…

A: The ideal gas equation is given by: PV=nRT where P is the pressure of the gas V is the volume of the…

Q: (SF) A certain reaction occurs, producing an oxide of nitrogen as a gas. The gas has a mass of 1.211…

A: The molar mass of gas can be calculated by using ideal gas equation PV = nRT Where P=…

Q: A gas mixture at 20.0°C and 2.0 atm contains 0.40 mol of H2, 0.15 mol of 02, and 0.50 mol of N2.…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: In any equation forms of the Ideal Gas Law, IGL, molar mass must be in what unit? a mol b kg/mol…

A: Given Ideal Gas Law Equation Unit if molar mass = ?

Q: You start with an equimolar mixture of the gases SO, and O, in a container. The SO, and O, react to…

Q: 3.If you are asked to calculate the volume of Carbon dioxide gas at 25oC and 802 torr that could be…

A: In this question, we will Identify which unit is best for pressure to converting Torr pressure unit…

Q: For many purposes we can treat propane (C,H) as an ideal gas at temperatures above its boiling point…

A: Here we use ideal gas equation because the gas is above -42 degree celcius.

Q: 1. Which one of the three varlables: Pressure, Volume or Temperature cannot be changed in Boyle's…

A: To answer questions regarding Boyle's Law.

Q: Which one of the following expressions should be used to determine the number of moles of gas, n,…

A: Ideal gas law: It can be define as the equation which relates volume pressure and temperature for…

Q: Use the standard molar volume of a gas at STP (1mol/22.4L) to find how many moles of methane (CH4)…

Q: A sample of 4.5 moles of an unknown gas occupies a volume of 1.6L at 23.2atm, what is the ideal…

A: The equation of the state of a fictitious ideal gas is known as the ideal gas law. Although it has…

Q: An ideal gas originally at 0.85 atm and 62°C was allowed to expand until its final volume, pressure,…

A: P1V1/T1 = P2V2/T2 V1 = P2V2T1/P1T2

Q: V55)4 Y6C102?. O GASES Calculating partial pressure in a gas mixture Jacqueline v A 7.00 L tank at…

Q: What does R the gas constant represent? What are standard conditions for any sample of an ideal gas?…

Q: Find the temperature (in °C) at which 2.10 moles of chlorine gas filled in a 25.0L cylinder will…

Q: Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime…

Q: The following data presented in Table 1 below were obtained for a virial gas at 25 degrees Celsius.…

A: The virial-equation of state (ignoring the third virial coefficient) is given as: PVRT=1+BV…

Q: When 0.1 mol of HCl gas is placed in a 10 liter box at 25 degree C, the pressure is about the same…

A: Explanation: when NH3 and HCl are mixed we get the product ammonium chloride (NH4Cl) NH3 + HCl…

Q: Question attached

A: Ideal gas Law: It is also known as a gas equation. It states that pressure, volume, and temperature…

Q: A storage tank of volume V contains the mass M of oxygen (O2) at pressure P. What is the temperature…

A: Given, Volume = V Mass of oxygen = M Pressure = P Required, Temperature…

Q: A moture of gaseous reactants is put nto a cyinder, where a chemical reaction turns them nto gaseous…

Q: Which of the following gas samples would be most likely to behave ideally under the stated…

A: From given Ideal gas is explained based on temperature and pressure and for the given gas samples…

Q: An average gas fireplace uses about 200 gallons (760,000 cm3) of propane gas per year. Assume that…

A: We would use ideal gas equation to calculate the mass of propane used .

Q: Acetylene gas can be produced by slowly reacting calcium carbide with water. CaC2(s) + 2H2O(l) ➡…

A: The number of moles of calcium carbide that involve in the reaction is determined on substitution…

Q: iron(s) + hydrochloric acid(aq) ---> ferric chloride(aq) + hydrogen(g) How many grams of iron are…

A: The reaction taking place is given as, => Iron (s) + Hydrochloric acid (aq) ------> Ferric…

Question

I need the answer as soon as possible

Calculate the total pressure (in atm)
of a mixture of 0.0200 mol of helium,
He, and 0.0100 mol of hydrogen, H2,
in a 1.50 L flask at 10°C. Assume
ideal gas behavior. Given that R =
0.0821 L'atm/(mol·K).
a. 0.349 atm.
b. 0.697 atm.
c. 0.465 atm.
d. 0.279 atm.
e. 1.39 atm.

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

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

93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
A collapsed balloon is filled with He to a volume of 12.5 L at a pressure of 1.00 atm. Oxygen, O2, is then added so that the final volume of the balloon is 26 L with a total pressure of 1.00 atm. The temperature, which remains constant throughout, is 21.5 C. (a) What mass of He does the balloon contain? (b) What is the final partial pressure of He in the balloon? (c) What is the partial pressure of O2 in the balloon? (d) What is the mole fraction of each gas?
Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
A 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000 1.5928 0.7500 1.0601 1.0000 0.7930 Use these data to calculate the value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). Plot the apparent molar masses against pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?