What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0209 grams of magnesium generates 21.98 mL of hydrogen at 22.7 °C with a hydrogen partial pressure of 723.9 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure.     26.6 g/mol     22.3 g/mol     24.2 g/mol     18.9 g/mol     26.5 g/mol

Q: Calculate the volume of each substance at STP.   a. 4.1 mol Ar     L   b. 1.9 g CO2     L

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Q: What is the experimental molar mass (that is, calculated from the data given and not taken from the…

A: Given Mass= 0.0316 gram Temperature =22.6 °C = 295.75K Pressure=762.6 torr Volume =31.53 mL

Q: Air contains nitrogen, oxygen, argon, and trace gases. If the partial pressure of nitrogen is 592 mm…

A: Given: Partial pressure of Nitrogen = 592 mm Hg Partial pressure of Oxygen = 160 mm Hg Partial…

Q: The radius of a xenon atom is 1.3 x 10^-8 cm. A 100-mL flask is filled with Xe at a pressure of 1.0…

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Q: If 88.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

A: Recall the reaction for decomposition of carbonic acid       H2CO3aq→H2Ol + CO2gFind moles of…

Q: A sample of argon has a volume of 155 mL at 1.00 atm. What is its volume at 1.50 atm? 118000 mL 51.5…

A: Boyle's law states that at constant temperature, pressure of gas is inversely proportional to volume…

Q: 24. A sample of oxygen that occupies 1.00 x 10° mL at 575 mm Hg is subjected to a pressure of 1.25…

A: The question is given the Boyle's law is applied Boyle's  law statements that volume of a fixed mass…

Q: How many liters of hydrogen are present in 3 moles of this gas at STP? a) 6.02 x 10^23 b) 22.4 c)…

A: Given  Number of mole of H2  = 3 mole  Volume of Hydrogen gas at STP =   ?

Q: At what temperature will 0.654 moles of neon gas occupy 12.30 liters at 1.95 atmospheres?

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Q: If 73.6 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

A: W = 73.6 g T = 298.15 k V = 2 L

Q: 24. A 2.50 L sample of nitric oxide gas at 100 °C is cooled to 20 °C. If the pressure remains…

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

Q: Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the…

A: Given : total volume of H2 collected = 93.91 mL = 0.09391 L  Barometric pressure = total pressure =…

Q: A chemist vaporized a liquid compound and determined its density. If the density of the vapor at…

A: Given density = d = 1.285 g/L  Pressure = P = 753 mmHg  Temperature = T = 90.0 0C  Gas constant = R…

Q: A 2.16 g sample of phosphorus was burned in a large excess of chlorine, and the phosphorus chloride…

A: To Calculate molar mass , we can use the relation that rate of effusion is inversely proportional to…

Q: a) Calculate the volume (in L) occupied by 16 g of Carbon dioxide gas at a pressure of 99.7 x 103 Pa…

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Q: If 75.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298 K) and…

A: Calculate the moles of carbonic acid,

Q: What is the experimental molar mass (that is, calculated from the data given and not taken from the…

A:

Q: (6.5)What is the molar volume of argon gas at STP? 15.3 L O 22.4 L O 4.00 L O 1.00 L

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Q: How many gram are present if a sample of nitrogen gas is placed in a 5.0 Liter flask at 1755 torr…

A: Nitrogen N2 is diatomic gas. Which is non-reactive and colorless in nature. It is generally used to…

Q: Calculate the volume, in liters, occupied by 1.92 mol of neon gas at STP. O 43.0 L 22.4 L 20.2 L O…

A: Introduction: We will solve this question with the help of ideal gas equation. The ideal gas law is…

Q: Suppose that 78.0 mL of H2 gas is produced at 20.0oC by the reaction of 0.0764 g magnesium and the…

A: Molar volume of gas : volume of one mole of a gas is called molar volume.

Q: The partial pressure of argon in the atmosphere is 0.0083 atm. What is the argon pressure at 55 km…

A: Given that, for argon gas, the partial pressure in the atmosphere is p0 = 0.0083 atm. We have to…

Q: 5. In the experiment aimed to calculate the molar volume of a gas, a 0.02 mole of [CuCO3.Cu(OH)2]…

A: In the experiment aimed to calculate the molar volume of a gas, a 0.02 mole of [CuCO3.Cu(OH)2]…

Q: A sample of 250.9 mL of wet nitrogen gas was collected over water at a total pressure of 753 torr…

A: As per Raoult’s Law,Total Pressure = Partial vapour pressure of water + Partial vapour pressure of…

Q: A chemist vaporized a liquid compound and determined its density. If the density of the vapor at…

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Q: What is the experimental molar mass (that is, calculated from the data given and not taken from the…

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Q: If 45.0 g of calcium carbide is allowed to react with an excess amount of water, what will be the…

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Q: One method used in the eighteenth century to generate hydrogen was to pass steam through red-hot…

A: Given that, a reaction is 3Fes+4H2Og→Fe3O4s+4H2g. The molar masses are Fe = 55.845 g/mol, H2O =…

Q: Nitrogen gas has many important applications in industry, especially in providing unreactive…

A: First, we will calculate number of moles of N2  produced , then using stoichiometric calculations,…

Q: If 3.85 L of CO was collected over water at 25°C and 689 mmHg, how many grams of HCHO2 were…

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Q: 1.3g water (18.02 gmol*) is produced by a reaction, and it is kept at 45°C in a closed flask of 4.5…

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

Q: If 69.6 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

A: Answer :- 13.7 (atm)  The final pressure of Carbon dioxide gas (CO2) = 13.7 atm…

Q: What is the experimental molar mass (that is, calculated from the data given and not taken from the…

A: Given: Mass of Mg reacting = 0.0228 g. Volume of H2 produced = 22.57 mL = 0.02257 L…

Q: A sample of oxygen gas was collected over water at a barometric pressure of 757.2 mm Hg and a…

A:

Q: Given that P = 1.03 atm R = 0.0821 L.atm/(mol. K) T = 365.62 K V = 0.19 L m = 0.16 g Calculate molar…

A: Given :-  P = 1.03 atm  R = 0.0821L.atm.mol-1.K-1  T = 365.62 K V = 0.19 L m = 0.16 g  To calculate…

Q: calculate the total amount of pressure (absolute pres.) in atmospheres that Mike is exposed to at…

A: Pressure at a certain depth = ρgh + atmospheric pressure 1 atm = 30 ft By using the unitary method…

Q: A 2.50 L sample of butane gas (C4H10), measured at 22.0 ºC and 1.20 atm pressure, is combusted…

A: Given Initial volume of butane gas = 2.50 L Temperature = 22.0°C = 295K Pressure = 1.20 atm Volume…

Q: Helium-neon lasers emit very high spectral purity red light at a wavelength of 632.8 nm, and were…

A: According to ideal gas law the volume of a gas is directly proportional to the number of moles of…

Q: Calculate the density of uranium hexafluoride (UF6) with pressure of 697 mmHg at 57oC temperature.…

A: Given: Pressure (P) = 697 mmHg P=697760 atm    ∵ 1 mmHg=1760 atm Temperature (T) = 57°C T=57+273…

Q: A sample of xenon gas occupies 38.34 L at 550.8°C. What does the volume become (in L) if the sample…

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Q: What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid…

A: The question is based on the concept of reaction Stoichiometry. We have to determine pressure in the…

Q: In a common Freshman College Laboratory experiment, KClO3 is decomposed by heating to give KCl and…

A: 2 KClO3 ---> 2 KCl + 3O2  Volume of O2 = 0.238 L  Temperature = 28°C  Pressure = 752 mm Hg 760 mm…

Q: Consider the following reaction: Zn(s)+2HCl(aq)=ZnCl2(aq)+H2(g) If 15.00 g of solid zinc reacts with…

A: The reaction  Zn(s)+2HCl(aq)------------------->ZnCl2(aq)+H2(g)

Q: If the pressure of 1.50 L of hydrogen gas at 100 °C decreases from 0.500 atm to 0.115 atm, what is…

A: Boyle's law : It sates that " at constant temperature the pressure  of certain mass of gas is…

Q: Mass of copper before electrolysis 5.621 g Mass of copper after electrolysis 5.487 g Volume of H2…

A: The given information is: Mass of copper before electrolysis = 5.621 g Mass of copper after…

Q: A student, following the procedure described to evaluate the Gas Law Constant collected the…

A: since you have posted multiple questions in a session. we are entitled to answer only first…

Q: What is the approximate percentage of the following atmospheric gases? Joxygen A. 78% v Carbon…

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Q: What is the experimental molar mass (that is, calculated from the data given and not taken from the…

A: According to an ideal gas equation PV= nRT Where P= pressure of the gas, V= volume of the gas, n= no…

Q: In a mixture of helium and chlorine, occupying a volume of 12.8 L at 605.6 mmHg and 21.6°C, it is…

A: We have given that  In a mixture of helium and chlorine, occupying a volume of 12.8 L at 605.6 mmHg…

Q: What volume of H2 will be combine with the 22 L CL2 (g) to form HCl (g)? What volume of HCl (g) will…

A: Given data contains,  Volume of chlorine is 22L.

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.