This is called Boyle's law: P1V1=P2V2 A sample of ideal gas at room temperature occupies a volume of 22.0 LL at a pressure of 492 torrtorr . If the pressure changes to 2460 torrtorr , with no change in the temperature or moles of gas, what is the new volume, V2V2V_2?' If the volume of the original sample in Part A (P1P1P_1 = 492 torrtorr , V1V1V_1 = 22.0 LL ) changes to 80.0 LL , without a change in the temperature or moles of gas molecules, what is the new pressure, P2P2P_2? Express your answer with the appropriate units.

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: Fe(s) + H2SO(aq) → FeS0.(aq) + H2(g) The volume of the balloon was 4.8 x10° L. What mass of Fe was…

A: Equation can be written as: Fe(s)+H2SO4→FeSO4(aq)+H2(g) Molar mass of Fe = 56 g/mol H2 = Molar mass…

Q: A student wanted to check if the volume of a gas would double after doubling its temperature in °C…

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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: A sample of N2 gas occupies 1.77 L at 25.5 °C. If the gas is in a container that can contract or…

A: At contact pressure , volume is directly proportional to temperature ,so  V/T = Constant

Q: Scuba divers who suffer from decompression sickness are treated in hyperbaric chambers using a gas…

A: Answer -

Q: If 56.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

A:

Q: If 72.6 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

A: The reaction taking place is given as, => H2CO3 (aq) ----> H2O (l) + CO2 (g) Given : Volume of…

Q: The density of H2 gas in a rigid container is 0.117 g/L at 55 °C. What is the pressure of hydrogen…

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

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: If 60.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

A:

Q: Consider a rigid 21.44 L gas canister that holds a mixture of two gases, Cl₂ and Xe. The total…

A: Given the volume of the rigid container, V = 21.44 L  Total moles of gas inside the container, n =…

Q: example in Part A has an initial volume of 42.0 L , and you have determined that it contains 1.60…

A:

Q: What volume is occupied by 5.8 g of propane gas, CaHs, at 35 °C and 1.15 atm pressure?

A: Given: Mass of propane i.e. C3H8 = 5.8 g. Temperature = 35 oC And pressure = 1.15 atm.

Q: A sample of gas has a volume of 4.00 L at 0.00 °C. What is the final temperature, in Celsius, when…

A: The final temperature will be = -170.72 °C ≈ -171 °C ( rounded to 3 significant figures )

Q: A fixed amount of gas at 25.0 °C occupies a volume of 9.23 L when the pressure is 629 torr. Use…

A: Given: Temperature T1 = 25oC = 25+273 = 298 K Volume V1 = 9.23 L. Temperature T2 = 135 oC = 135 +273…

Q: If 6.90 L of gaseous ethanol reacts with 17.2 L O2, what is the maximum volume of gaseous carbon…

A:

Q: Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC₂…

A: Reaction :

Q: Oxygen gas can be prepared by heating potassium chlorate according to the following equation:…

A:

Q: According to the ideal gas law, a 9.045 mol sample of oxygen gas in a 0.8496 L container at 499.8 K…

A: The pressure of O2 gas under the given conditions has been calculated using ideal and Vanderwaal's…

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

A:

Q: According to the ideal gas law, a 10.90 mol sample of methane gas in a 0.8267 L container at 495.1 K…

A: To solve this question, we need to calculate new pressure using van der waals equation and then take…

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: A container with volume 1.48 L is initially evacuated. Then it is filled with 0.226 g of N2+. Assume…

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Q: When the ideas from Boyle’s Law, Charles’ Law and Gay-Lussac’s Law are combined, you get the…

A:

Q: If 75.2 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

A: It is a decomposition reaction in which carbonic acid is dissociated into carbon dioxide and water.…

Q: A gas with a volume of 15 L at 327°C is cooled at a constant pressure until the volume reaches 5 L.…

A: Initial volume = 15 L  Initial temperature = 327°C  Final volume = 5 L  Final temperature : A new…

Q: Na2CO3 + 2 HCl →→ 2 NaCl + H2O + CO2(g) If 3.0 L of carbon dioxide is produced at 769.8 torr and…

A: Given equation is: Na2CO3 + 2 HCl →→ 2 NaCl + H2O + CO2(g)  Volume of CO2 gas = 3.0 L Pressure of…

Q: Boyle's Law explores the effects of pressure on the volume of an ideal gas. Boyle’s Law is described…

A:

Q: Q1. A hydrocarbon (Ma=224.253 g/mol) found to contain 64.27% carbon and 7.19% hydrogen by mass, the…

A: We will first determine the molecular formula of the organic compound. Then apply stoichiometry to…

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

A:

Q: On a summer day, the temperature inside a house rises to 37 °C. In the evening, the house may cool…

A: T1=37oC=37+273=310KT2=21oC=21+273=294KV=9.50*105 LP=768 mmHgMolar mass of air = 28.8 g/mol

Q: The product gas, C,H2, is collected over water at a temperature of 20 °C and a pressure of 745 mm…

A:

Q: f 81.4 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

A: Mass of carbonic acid = 81.4 g Temperature (T) = 298.15 K Volume (V)= 2.00L Gas constant (R) = 0.082…

Q: According to the ideal gas law, a 9.556 mol sample of argon gas in a 0.8165 L container at 503.4 K…

A:

Q: Boyle's Law explores the effects of pressure on the volume of an ideal gas. Boyle’s Law is described…

A:

Q: combined gas law

A:

Q: alculate molar mass (g/mol) of an unknown gas if its root-mean-square speed is 3.61 x 102 m/s at 20…

A: Given: The root-mean-square speed, Urms =3.61 x 102 m/s Temperature,T= 20°C Temperature,T= 20+…

Q: What is the volume, in liters, of 4.00 molesmoles of methane ga

A: From ideal gas equation  P V = n R T  where P = Pressure of the gas = 2 atm  V  = Volume of gas =…

Q: If 53.6 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

A:

Q: Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC₂…

A:

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: A vessel with a volume of 2 · 10-3 m3 is filled with 19 grammes  of carbon dioxide gas (CO2) and 14…

A:

Q: Use the ideal gas equation, PV = nRT, to calculate the volume in liters of 1.808 moles of nitrogen…

A: The ideal gas law was directly used to find the volume.

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.