A sample of 3 mol of CO2(g) is confined to a 3.000-L container at 23 C. Calculate the pressure of the gas using (a) the ideal-gas equation and (b)the van der Waals equation.

Q: n addition to filling in the blanks below, show all of your work for this problem on paper upload. A…

A: Ideal gas equation is the relationship  among the volume  temperature  , pressure  and amount of gas…

Q: A 10.0 L flask contains a mixture of neon and argon gases at a pressure of 2.38atm. Calculate the…

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Q: b. How many moles of hydrogen are in this sample?

A: An ideal gas equation is derived from the combination of Charle's law, Boyle's law, and Avogadro…

Q: Explain why the molar volume of helium (or any other ideal gas) is 22.4 L.

A: The volume occupied by one mole of gas at temperature 0°C (273K) and 1.00 atm pressure can be easily…

Q: There are 101.0 g of chlorine gas (Cl2) and 26.0 g of helium (He) mixed in a container with a total…

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Q: The volume of a sample of hydrogen gas was decreased from 11.97 L to 5.26 L at constant temperature.…

A: According to ideal gas law  PV = nRT  where P = pressure  V = volume n = moles  R = gas constant  T…

Q: According to the ideal gas law, a 0.9513 mol sample of argon gas in a 1.456 L container at 272.8 K…

A: Answer:Here:

Q: If 48.070 L of gas is collected at a temperature of 20.531°C and a total pressure of 798.00 torr,…

A: The given data contains, Volume = 48.070 L. Total pressure = 798 torr. Temperature = 293.531 K

Q: Calculate the mass and number of moles of dinitrogen difluoride gas that were collected. R

A: Given: Volume= 30.0 L Pressure= 0.320 atm Temperature= 8.0oC= 281.15 K   To calculate:

Q: Calculate the pressure (atm) exerted by 1.00 mol of gascontained in a 7.55-L cylinder at 458C.

A: The effect of pressure and temperature is measured by Boyle’s law and Charles's law respectively.…

Q: At 304.8 K, a 9.58 L tank contains 1.90 moles of H2 gas under a certain pressure in atm. Calculate…

A: Given, Volume = 9.58 L Number of moles = 1.90 mol Temperature = 304.8 K

Q: 891 mm Hg and a temperature of 65°C, occupies a volume of 17.9 liters. If the gas is heated at…

A: We have to find  effect of temperature change on volume

Q: 132.0 g of chlorine gas (Cl2) and 24.0 g of helium (He) are mixed in a container with a total…

A: Given,  Mass of. Cl2 = 132 g Molar mass of Cl2 = 71 g/mol Moles = mass/MM     = 132/71   = 1.86 mol…

Q: In a flask, there are two gases (gas 1 and gas 2). There is 2.34 L of gas 1, with 3.2 bars of…

A: Given a flask contains gas 1 and gas 2 2.34 L of gas 1.  Partial pressure of gas 1 = 3.2 bars 6.19 L…

Q: A sample of 257.0 mL of wet nitrogen gas was collected over water at a total pressure of 759 torr…

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Q: A 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at…

A: Stoichiometry relates the amount of reacting with the formed species. As per this concept, the…

Q: Calculate the pressure exerted by 106.359 grams of chlorine gas, confined to a volume of 510 mL at…

A: The ideal gas equation is  PV = nRT  P = pressure of gas  V = volume  n = moles of gas = mass/molar…

Q: 1.50 grams of nitrogen (N₂) gas is sealed in a 750.00 ml container at 35.0°C. Calculate the pressure…

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Q: Suppose 10.05 mol of Ar gas are pumped into a 1.41  L container at 293.15  K. Calculate the expected…

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Q: The volume of a sample of hydrogen gas was decreased from 12.62 L to 5.91 L at constant temperature.…

A: According to Boyle’s law,

Q: 103.0 g of chlorine gas (Cl2) and 23.0 g of helium (He) are mixed in a container with a total…

A:

Q: What is the origin of the discrepancy between the theoretical and experimental values of the molar…

A: The ideal gas law is a fundamental concept in the field of chemistry that describes the behavior of…

Q: Calculate the temperature in oC when 2.50 moles of argon occupy 25.0 L at 1.20 atm. Write the ideal…

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Q: Suppose 10.00  mol of Ar gas are pumped into a 1.06  L container at 293.15  K. Calculate the…

A: Solution : Ideal gas law is used to describe the behavior of a gaseous substance which shows…

Q: A reaction between liquid reactants takes place at 18.0 °C in a sealed, evacuated vessel with a…

A: Given: Mass of dinitrogen monoxide gas = 10 g Volume of vessel = 45 L Temperature = 18 °C = 18 +273…

Q: A 40.0 g sample of potassium metal is allowed to react with excess hydrochloric acid to produce H2…

A: First we would Calculate moles of Hydrogen gas produced and using ideal gas law we would Calculate…

Q: Consider a gas mixture that contains only helium (He) and neon (Ne). If the partial pressure of He…

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Q: Hydrogen gas, oxygen gas, and water vapor are collected in eudiometer. The eudiometer contains…

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Q: At 304.8 K, a 9.58 L tank contains 1.90 moles of H2 gas under a certain pressure in atm. Calculate…

A: Ideal gas equation is, PV= nRT Where, P=pressure, V=Volume, n =number of moles R=gas constant…

Q: According to the ideal gas law, a 9.919 mol sample of argon gas in a 0.8468L container at 497.2 K…

A: Given Pideal = 477.9 atm  Volume = 0.8468L  Temperature 497.2 K  Moles = 9.919  We have to find the…

Q: Calculate the density of He gas at 1atm of pressure and 20.00C. Explain (using your calculated…

A: To calculate the density of the He gas at 1 atm pressure and 20.0oC temperature.

Q: 2.58 gram sample of an unknown gas is found to occupy a volume of 1.53 L at a pressure of 687 mmHg…

A: Given that:  Mass of gas = 2.58g Volume(V) = 1.53L P = 687 mmHg = 687mmHg×1atm/760mmHg = 0.9039atm T…

Q: What mass of helium gas is needed to pressurize a 92.0 L tank to 209 atm at 18 °C? What mass of…

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Q: use the ideal gas law to identify this gas.

A: Ideal Gas Law :-  PV = nRT  P is the pressure of gas  V is the volume occupied by gas n is the…

Q: Calculate the mass of 6.2 L of CO2 at 300° K and a pressure of 758.0 mm Hg.

A: CO2 gas Volume = V = 6.2 L Temperature = T = 300 K Pressure = P = 758.0 mm Hg ( 1 atm = 760 mm Hg )…

Q: You have 448. mL of chlorine trifluoride gas at 681. mmHg and 30. °C. What is the mass (in g) of the…

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Q: A sample of an ideal gas at 1.00 atm and a volume of 1.90 L was placed in a weighted balloon and…

A: Interpretation -  To detrmine the volume of the sample when pressure is increased to 80 atm of a…

Q: A 32.80 g sample of argon gas is added to a 15.50 g sample of radon gas in a 10.0-L container at…

A: Given that,  Amount of argon gas = 32.80 g Moles of argon gas = 32.80 g/39.948 g/mol = 0.82 mol…

Q: Suppose 10.05 mol of Ar gas are pumped into a 1.56  L container at 293.15  K. Calculate the…

A: The van der-Waal's equation is given by (P+an2V2)(V−nb)=nRT R = gas constant n = number of moles of…

Q: A certain amount of chlorine gas was placed inside a cylinder with a movable piston at one end. The…

A: Given that: Initial volume of gas = 3.00 LFinal volume of gas = 1.00 LInitial pressure of gas = 1.25…

Q: 51. A sample of 5.22 grams of xenon gas occupies a 500. mL container with a pressure of 565 kPa.…

A: The given information is: Mass of xenon = 5.22 g Volume = 500 ml = 0.5 L Pressure = 565 kPa = 5.576…

Q: At 304.8 K, a 9.58 L tank contains 1.90 moles of H2 gas under a certain pressure in atm. Calculate…

A: Given, Volume = 9.58 L Number of moles = 1.90 mol Temperature = 304.8 K

Q: To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an…

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Q: According to the ideal gas law, a 10.24 mol sample of xenon gas in a 0.8381 L container at 499.4 K…

A: The objective of the question is to calculate the percent difference between the pressure calculated…

Q: A gas made up of homonuclear diatomic molecules escapes through a pinhole 1.19 times as fast as Ar…

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Q: Use the van der Waal's Equation to calculate the pressure exerted by 80.0 grams of hydrogen sulfide…

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Q: Use the van der Waals equation and the ideal gas equation to calculate the pressure exerted by 1.000…

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Q: The atmospheric pressure on a particular day is 726 mmHg. Given that the mole fraction of N2 in air…

A: Answer: 567.006 mmHg

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.