If a container of an ideal gas at standard temperature and pressure (0 °C, latm) had one mole of gas inside of it, what is the volume of this container, in Liters? (R= 0.08206 L*atm/(mol*k)

If a container of an ideal gas at standard temperature and pressure (0 °C, latm) had one mole of gas inside of it, what is the volume of this container, in Liters? (R= 0.08206 Latm/(molk)

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter13: Gases

Section: Chapter Questions

Problem 5ALQ

See similar textbooks

Related questions

Q: Using the ideal gas law, PV=nRT, calculate the number of moles of gas present in a 1.50 L container…

A: Given-> Volume = 1.50 L P = 1.25 atm T= 30°C = 30+ 273 = 303K

Q: A certain gas sample has a volume of 225 mL at a pressure of 1.25 atm at 27oC; what would be its…

A: Given: P1 = 1.25 atm V1 = 225 ml P2 = 0.75 atm V2 = ? according to boyles at constant temperature.…

Q: The particulate model shown below represents the moles of particles present in the container after…

A: Here, No. of moles of D=2 No. of moles of F2=3 No. of moles of DF4=10

Q: A container contains 0.50 g of H2(g) and 0.50 g of O2(g). The total pressure in the container is…

A: Given :- Amount of H2 = 0.50 g Amount of O2 = 0.50 g Total pressure = 1.56 atm To calculate :…

Q: (CH4) as an ideal gas at temperatures above its boiling point of -161. °C. Suppose the temperature…

A: The Ideal Gas equation is given by,PV = nRTwhere,P= Pressure in atmV = Volume in LT = Temperature in…

Q: 13 g of an unknown gas in a tank with a volume of 5.53 L has a pressure of 3.83 atm at 28°C. If the…

A: Here given, Pressure (P) = 3.83 atm Volume (V) = 5.53 L Temperature (T) = 280C = (273+28) K = 301 K…

Q: Practice 1. Determine the volume occupied by 0.582 mol of oxygen gas at 285K and 7 atm. PV = nRT P.

A: Formula used: PV=nRT Where P= pressure V= volume n = number of mole R = 0.082(gass cons)…

Q: A container contains 0.50 g of H2(g) and 0.50 g of O2(g). The total pressure in the container is…

A: Given: Mass of H2 = 0.50 g. Mass of O2 = 0.50 g. And total pressure of gases = 1.56 atm.

Q: . What volume is needed to store 5 moles of helium gas at 350 K under the pressure 190 KPA? of - A…

A: This question is related to ideal gas law. Ideal gas law is a combined gas law of Boyle's law,…

Q: A student performs an experiment like the one you saw in Experiment 8. The student determines the…

A: Given, Pressure of oxygen is 0.7811 atm Volume of oxygen is 217 ml = 0.217 L Temperature = 298.15 K…

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: A mixture of 3.0 g H2(g) and 12.0 g He(g) in a 7.0 L flask is maintained at 0 ∘C. What is the total…

A: According to ideal gas law, PV = nRT where P = total pressure of gas mixture V = volume = 7 L n =…

Q: A neon sign is made of glass tubing whose inside diameter is 2.0 cm and whose length is 4.0 m. If…

A: P = 1.5 mm Hg T = 350C = 308 K Radius = 1 cm = 0.01 m Length = 4 m

Q: For many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point…

Q: For an ideal gas, calculate the following quantities. (a) The pressure of the gas if 0.145 mol…

Q: A.) An aqueous solution of potassium acetate, KCH3COO, contains 3.47 grams of potassium acetate and…

A: The answers to the following Questions are given as:

Q: You have a cylinder of argon gas at 16.5 atm pressure at 13°C. The volume of argon in the cylinder…

A: Consider the given information is as follows; Initial pressure (P1) = 16.5 atmInitial volume V1 =…

Q: For many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point…

A: The relationship between a fixed amount of gas's pressure, volume, and absolute temperature is…

Q: A 2-liter cylinder with a piston is used in a constant-pressure thermometer. The mass of the gas is…

A: Volume of cylinder = 2 L Initial volume = 0.850 L Final volume = 0.435 L Initial Temperature =…

Q: What is the pressure of CO2 Gas that has a mass of 5.68g with a volume of 966mL. The gas has a…

Q: For many purposes we can treat propane (C3H8) as an ideal gas at temperatures above its boiling…

A: Since the given range of temperature is above the boiling point of propane so we can assume it as an…

Q: For many purposes we can treat propane (C₂Hg) as an ideal gas at temperatures above its boiling…

A: Details

Q: gas in a container occupies a volume of 695 mL at a temperature of 82 °C. What must the temperature…

A: Given- T1=82°C=(82+273)K=355K V1=695mL V2=762mL

Q: States of Matter = Using the combined gas law For many purposes we can treat butane (C4H10) as an…

A: The objective of the question is to determine if it is possible to change the temperature of butane…

Q: Chemistry a 2. Mixtures of helium and oxygen are used in scuba diving tanks to help prevent "the…

A: We are provided with a mixture of two gases, oxygen and helium. Volume of the gases are given along…

Q: This is called Boyle's law: P1V1=P2V2 A sample of ideal gas at room temperature occupies a volume of…

A: The Boyle's law describes that pressure of a gas at a given temperature will be inversely…

Q: What is the molar mass (in g/mol) of a gas that has a mass of (3.230x10^-1) g, volume of (2.51x10^2)…

A: Molar mass of gas, Mw = ? Mass of the gas, W = 0.3230 g Volume occupied by gas, V = 251 mL = 0.251…

Q: An ideal gas in a sealed container has an initial volume of 2.75 L. At constant pressure, it is…

Q: A sample of 0.225 mole of gas has a volume of 748 mL at 28°C. Calculate the pressure in atm of this…

Q: At 105.1 oC and 0.4500 atm pressure, a gas occupies a volume of 0.600 L. How many liters will it…

A: Gas laws , PV = nRT P1V1/T1 = P2V2/T2

Q: A mixture that's 35.0% N2 and 65.0% O2 by volume has a total pressure of 2500. psi. What is the…

A: To solve this problem we have to use the concept of Dalton Law of Partial Pressure.

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

Q: A student recovered0.398g of THF vapor in a 125 mL flask. Assuming the vapor is an ideal gas with a…

Q: For many purposes we can treat nitrogen (N2) as an ideal gas at temperatures above its boiling point…

A: The relationship between the temperature, pressure, and volume of the initial and final state of an…

Q: What is the temperature (K) if 5.00 g of methane (CH4) in a 100.0 mL container exerts a pressure of…

Q: What is the pressure in atm of O2 gas (density 3.00 g/L) at 11.09 °C? Gas constant = 0.08206 L…

A: Given,Density of O2 gas = 3.00 g/LTemperature = 11.09 °CGas constant = 0.08206 L atm/K molMolar…

Q: Given the ideal gas law PV=nRT calculate the pressure of a gas in atmospheres if 14 moles of the gas…

Q: A container of gas has a initial pressure of 0.8 atm The pressure is increase to 1.1atm and the…

A: The gas initial volume present in a container with given final volume, initial and final pressures…

Q: What volume of hydrogen gas, in mL, is produced from 0.128 g Mg reacting with an excess of HCI at a…

A: A question based on the mole concept. Using the information about the number of moles of reactant…

Q: If a gas remains at constant pressure while its volume increases from 0.25Liters to 500 mL when its…

A: Given data contains, Initial volume is 0.25 L. Final volume is 500 mL=0.5 L. Final temperature is…

Q: 215.0 mol of an unknown gas is stored at a temperature of 1110 K in a large, 395 L container. In…

A: Pressure is calculated by using ideal gas equation

Q: A certain gas is present in a 13.0 LL cylinder at 3.0 atmatm pressure. If the pressure is increased…

Q: A bacterial culture isolated from sewage produced 43.4 mL of methane at 34.0 °C and 772 mm Hg. What…

A: Given: Initial Volume V1 = 43.4 mL Initial Pressure P1 = 772 mmHg Initial Temperature T1 = 34 oC =…

Q: For many purposes we can treat nitrogen (N₂) as an ideal gas at temperatures above its boiling point…

A: The Ideal Gas equation is given by,PV = nRTwhere,P= Pressure in atmV = Volume in LT = Temperature in…

Q: The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The…

Question

If a container of an ideal gas at standard temperature and
pressure (0 °C, latm) had one mole of gas inside of it,
what is the volume of this container, in Liters? (R= 0.08206
L*atm/(mol*k)

AI-Generated Solution

AI-generated content may present inaccurate or offensive content that does not represent bartleby’s views.

Unlock instant AI solutions

Tap the button
to generate a solution

Click the button to generate
a solution

SEE SOLUTION

Similar questions

A typical barometric pressure in Kansas City is 740 torr. What is this pressure in atmospheres, in millimeters of mercury, and in kilopascals?
What is the value of the ideal gas constant R if the volume is specified in milliliters rather than liters?
Many nitrate salts can be decomposed by heating. For example, blue, anhydrous copper(II) nitrate produces the gases nitrogen dioxide and oxygen when heated. In the laboratory, you find that a sample of this salt produced a 0.195-g mixture of gaseous NO2 and O2 with a total pressure of 725 mm Hg at 35 C in a 125-mL flask (and black, solid CuO was left as a residue). What is the average molar mass of the gas mixture? What are the mole fractions of NO2 and O2 in the mixture? What amount of each gas b in the mixture? Do these amounts reflect the relative amounts of NO2 and O2 expected based on the balanced equation? Is it possible that the fact that some NO2 molecules combine to give N2O4 plays a role? Heating copper(II) nitrate produces nitrogen dioxide and oxygen gas and leaves a residue of copper(ll) oxide.
5-114 Carbon dioxide gas, saturated with water vapor, can be produced by the addition of aqueous acid to calcium carbonate based on the following balanced net ionic equation: (a) How many moles of wet CO (g), collected at 60.°C and 774 torr total pressure, are produced by the complete reaction of 10.0 g of CaCO3 with excess acid? (b) What volume does this wet CO2 occupy? (c) What volume would the CO2 occupy at 774 torr if a desiccant (a chemical drying agent) were added to remove the water? The vapor pressure of water at 60.°C is 149.4 mm Hg.
A 21.4-mL volume of hydrochloric acid reacts completely with a solid sample of MgCO3. The reaction is 2HCl(aq)+MgCO3(s)CO2(g)+H2O(l)+MgCl2(aq) The volume of CO2 formed is 159 mL at 23C and 731 mmHg. What is the molarity of the HCl solution?
A 0.105-g sample of a gaseous compound has a pressure of 561 mm Hg in a volume of 125 mL at 23.0 C. What is its molar mass?
5-111 Diving, particularly SCUBA (Self-Contained Underwater Breathing Apparatus) diving, subjects the body to increased pressure. Each 10. m (approximately 33 ft) of water exerts an additional pressure of 1 atm on the body. (a) What is the pressure on the body at a depth of 100. ft? (b) The partial pressure of nitrogen gas in air at 1 atm is 593 mm Hg. Assuming a SCUBA diver breathes compressed air, what is the partial pressure of nitrogen entering the lungs from a breathing tank at a depth of 100. ft? (c) The partial pressure of oxygen gas in the air at 2 atm is 158 mm Hg. What is the partial pressure of oxygen in the air in the lungs at a depth of 100. ft? (d) Why is it absolutely essential to exhale vigorously in a rapid ascent from a depth of 100. ft?
61 As one step in its purification, nickel metal reacts with carbon monoxide to form a compound called nickel tetracarbonyl, Ni(CO)4, which is a gas at temperature above about 316 K. A 2.000-L flask is filled with CO gas to a pressure of 748 torr at 350.0 K, and then 5.00 g of Ni is added. If the reaction describe occurs and goes to completion at constant temperature, what will the final pressure in the falsk be?
5-37 A sample of a gas at 77°C and 1.33 atm occupies a volume of 50.3 L. (a) How many moles of the gas are present? (b) Does your answer depend on knowing what gas it is?
5-33 A certain quantity of helium gas is at a temperature of 27 °C and a pressure of 1.00 atm. What will the new temperature be if its volume is doubled at the same time that its pressure is decreased to one-half its original value?
In an experiment in a general chemistry laboratory, a student collected a sample of a gas over water. The volume of the gas was 265 mL at a pressure of 753 torr and a temperature of 27 C. The mass of the gas was 0.472 g. What was the molar mass of the gas?
47 HCl(g) reacts with ammonia gas, NH3(g), to form solid ammonium chloride. If a sample of ammonia occupying 250 mL at 21 C and a pressure of 140 torr is allowed to react with excess HCl, what mass of NH4Cl will form?