The standard volume was derived from the ideal gas law.

Q: At a pressure of 1 atm and a temperature of 20oC, dry air has a density of 1.2256 g/L. What is the…

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Q: Which of the following statements about the Kinetic Theory of gases is false? o Kinetic energy of a…

A: Kinetic molecular theory of gases: Postulates are  1.kinetic energy of a molecule is directly…

Q: 5. The volume for one mole of ideal gas at 47 ° C and one pressure:

A: Given :-  Number of moles of ideal gas = 1 mol  Pressure of gas = 1 atm  Temperature = 47°C  To…

Q: If the density of an ideal gas at STP is found to be 1.96 g/L, what is its molar mass? molar mass:…

A: Given, the density of an ideal gas at STP =1.96 gLWe are asked to calculate the molar mass of ideal…

Q: 2. A sample of He gas effused 5.3 times faster than an unknown gas, under the same conditions.…

A: Given: The Helium gas with atomic  mass of = 4 u.

Q: Can (L), be a unit of pressure?

A: Detail description is given below

Q: 1. A 0.678 gram sample of gas occupies 0.214 L at standard conditions; what is the molar mass of the…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: What gas law is applied in breathing?

A: To find: The law which is applied in breathing

Q: At 741 Torr and 44°C, 7.10 g of a gas occupies a volume of 5.40 L. What is the molar mass of the gas…

A: Given: Pressure is 741 torr Volume is 5.40 L Temperature is 44oC Mass is 7.10 g To find: Molar mass

Q: What is the ideal gas law?

A: The Ideal Gas Law is simply the combination of all Simple Gas Laws (Boyle's Law, Charles' Law, and…

Q: . In a hospital an oxygen cylinder contains 423 L of pure oxygen at a pressure of 136 atm. What is…

A: In this question, we will determine the volume of oxygen gas at 1.00atm when temperature and number…

Q: What was Boyles most famous discovery about gases?

A: Introduction In 1662, a scientist Robert Boyle studies the changes in volume of a particular gas by…

Q: how the Ideal Gas Law can be used to find the molar mass of a metal like magnesium?

A: The concept of ideal gas law is assumed to be followed by all the gases. There are certain reactions…

Q: The rms speed of the molecules of a gas at 137 C is 191 m/s. Calculate the mass ? of a single…

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Q: a rate of effusion th

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Q: At 4.00 L, an expandable vessel contains 0.864 mol of oxygen gas. How many liters of oxygen gas must…

A:

Q: Cyanogen, a highly toxic gas, is composed of 46.2% C and 53.8% N by mass. At 25 degrees C and 751…

A: Given:Mass percent composition of carbon is 46.2%.Mass percent composition of nitrogen is 53.8%. The…

Q: The density of 1.00 mol of an unknown gas at a temperature of -71oC and a pressure of 2,359 torr is…

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Q: For an ideal gas, classify the pairs of properties as directly or inversely proportional.

A: To classify the given pairs of properties as directly or inversely proportional. P and V P and T P…

Q: 1. What are the three assumptions of the kinetic theory as it applies to gases?

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Q: The excluded volume in a real gas is?

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Q: Which of the following instruments would be used to measure the pressure of a gas sample relative to…

A: We know that, Pressure represent the force applied perpendicular to the surface of any object per…

Q: How does the density of a gas depend on temperature? Pressure? How does it depend on the molar mass…

A: The molar mass of a substance (M) is characterized as the number of grams (m) per mole (n) of that…

Q: What is the density of xenon gas at standard conditions

A: Molar mass of xenon = 131.293 g The volume occupied by 1 mol of any gas on STP is 22.4 L. Hence, the…

Q: If 760 Torr is equivalent to 1 atm and to 1.01325 bar, then a pressure of 1 bar is equivalent to

A: given760 torr = 1 arm760 torr = 1.01325 barthen 1 bar = To be determined

Q: the time required for given volume of Nitogen molecule to duffuse through an orifice is 35 seconds.…

A: Use concept of grams law of diffusion t2/t1=M.w2/M.w1 And get the answer.

Q: If a sample contaimns 0.312 moles of Xe and 0.8 moles of He, determine the total pressure of the gas…

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Q: It states that for a fixed amount of gas at a constant temperature, the gas volume is inversely…

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Q: STANDARD PRESSURE Convert 29.17 inches of Hg to atm

A: 1 inch of Hg is equal to 0.0334211 atm

Q: What is the average speed for carbon monoxide molecules at the same temperature and pressure ?

A: Average speed of a gas can be calculated by using the following formula.    Since the value of…

Q: Calculate the % error in the universal gas constant you found:

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Q: The ability to replace moles with volume in stoichiometric expressions when temperature and pressure…

A: The ideal gas equation is as follows,                         P V = n R T Where, P is the pressure…

Q: Which of the following statements regarding the kinetic molecular theory of gases is NOT correct?

A:

Q: There are three postulates/assumptions of the kinetic model of gases, which of the following is not…

A: The incorrect option is C  The volume of the gas is due to the large number of molecules in a gas.

Q: At SATP, a gas has a density of 1.78 g/L. What is the molar mass of the gas?

A: We have the ideal gas law as: PV= nRT We know no of moles = given mass÷ molar mass ⇒PV = (w÷M)RT…

Q: The volumes of gases A, B, C and D are in the ratio 1: 2:2:4 under the same conditions of temperatue…

A: The gasses are the state of matter having that has negligible forces of attraction between then and…

Q: [References] Use the References to access important values if needed for this question. The rate of…

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Q: 6. What is the densest known gas at standard temperature and pressure (STP)? What is its density?

A: Density of as gas can be calculated as: Density = MassVolume At standard temperature and pressure,…

Q: Calculate the density of NO2 gas at 0.970 atm and 35C.

A: Using the ideal gas equation, the density of given NO2 is determined.

Q: If the density of an ideal gas at STP is found to be 1.25 g/L, what is its molar mass? molar mass:…

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Q: Briefly describe the concepts of ideal gas law

A: Ideal gas law

Q: What volume will a 0.981 mole gas sample occupy at standard temperature and pressure?

A: We can calculate the volume occupied by 0.981 moles by using the ideal gas equation:…

Q: When calculating a ratio for the mean speeds, does the ratio change with temperature?

A: Welcome to bartleby. The answer to the question is given below.

Q: What is the rms speed of carbon tetrachloride molecules at 25.00C?

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Q: 0.101 L of gas at 760. torr is compressed to 800. torr.  Calculate the resulting gas volume in mL at…

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

Q: How does the density of the gas depend on the molar mass of the gas?

A: The density of the gas depends on the molar mass of the gas has to be defined.

Q: If the pressure of a gas sample is octupled and the absolute temperature is quadrupled, the volume…

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Q: Explain the relationship between partial pressure and total pressure, and between the volume and…

A: To identify: The relationship between the partial pressure and total pressure. And between the…

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.