nce you’ve identified the initial and final conditions, you’re ready to solve for the unknown quantity in your problem.  Boyle’s Law expresses the pressure-volume relationship as P1V1=P2V2, so you will need to solve this equation for the unknown quantity and then plug in your known values to calculate the unknown. What pressure would it take to compress 300. L of helium gas initially at 1.00 atm into a 2.00 L tank at constant temperature?

Q: Suppose the pressure at a point within a column of mercury in a tube is 74 mm Hg. What is the…

A: Pressure of the mercury column is 74 mm Hg.

Q: a) If 56.0 g of N2 gas occupies 44.8L under Standard Conditions, then what is the mass of 134.4 L of…

A:

Q: H2(g) O2(g) 4.0 g 64 g V = 10.0 L T = 300. K V = 10.0 L T = 300. K Representations of two gas…

A:

Q: Exhaled air contains 16% oxygen by volume. Assuming you exhale like the average person does during…

A: When we workout our muscles work harder our body uses more oxygen and produces more carbon dioxide.

Q: A flexible container at an initial volume of 6.13 L6.13 L contains 6.51 mol6.51 mol of gas. More gas…

A: Given that :  Initial volume (V1) = 6.13 L Initial moles(n1) = 6.51 mol Final volume (V2) = 18.5L…

Q: . Nitrogen gas occupies a volume of 1.87 x 102 mL, at 27 °C, and 0.89 atm of pressure. How much…

A: We have to calculate the pressure exerted.

Q: Liquid mercury has a density of 13.534 g/mL. If a barometer (used to measure pressure) requires…

A: Given : Density of mercury = 13.534 g/mL And volume of mercury required = 12.00 mL

Q: P4(g) + 6Cl2(g) → 4PCl3(g) 4.53 L of P4(g) is mixed with 6.80 L of Cl2(g) and reacts with 100%…

A:

Q: A gas sample in a Boyle’s law apparatus is compressed to a volume of 22.0 mL. If its original volume…

A:

Q: If 0.00890 mol neon gas at a particular temperature and pressure occupies a volume of 179 mL, what…

A: Given, n1= 0.00890 mol , n2= 0.00652 mol V1 = 179 mL , V2 = ? Ideal gas law : PV = nRT , where P =…

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: A gas is heated from 213.0 K to 298.0 K and the volume is increased from 14.0 liters to 35.0 liters…

A:

Q: A sample of neon gas has a volume of 752 mL at 25.0 °C. What will the volume at 50.0°C be if…

A: The problem is asking us to find the volume of a gas at a different temperature, given the initial…

Q: A gas sample with a volume of 5.3 L has a pressure of 745 mmHg at 29 ∘C.

A: Form combined gas law   P1 V1T1  =  P2 V2T2       where  P1 = 745 mmHg x 1atm/760 mmHg  = 0.98 atm…

Q: A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas…

A: We will solve this question using gas laws

Q: Helium is a gas at the boiling point of liquid nitrogen, 77.0 K. If 2.00g of He is placed inside a…

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

Q: A) A sample of ideal gas at room temperature occupies a volume of 40.0 L at a pressure of 542 torr .…

A: Boyle’ law states that at a particular temperature and number of moles, the pressure of a gas is…

Q: Sample of oxygen, at 25°C, occupies a volume of 5.40 X 10" milliliters (mL) at 1.42 atm pressure.…

A:

Q: Consider a gas cylinder with a volume of 1.6 L that contains 28.07 g of CH4gas. What is the total…

A: Please see the attached image for the solution.   If there are queries or if the image is not…

Q: A balloon of carbon dioxide gas has a volume of 56.7 Liters at a pressure of 56.7 atmospheres and a…

A:

Q: A sample of an ideal gas at 1.00 atm1.00 atm and a volume of 1.28 L1.28 L was placed in a weighted…

A: according to boyl's law at constant temperature pressure is inversely proportional to volume

Q: The initial volume of a gas cylinder is 750.0 mL. If the pressure of a gas inside the cylinder…

A: Given  Initial volume of a gas cylinder is 750.0 mL  Pressure of a gas inside the cylinder changes…

Q: A low pressure of 1.00 x 10^-3 Torr is readily obtained in the laboratory by means of a mechanical…

A: Pressure = 1.00×10-3 TorrVolume = 1mLTemperature = 20°C = 293.15 KGas constant, R = 62.363…

Q: A certain gas is present in a 13.0 L cylinder at 1.0 atm pressure.  If the pressure is increased to…

A: Initially : Volume, V1 = 13 L               Pressure, P1 = 1 atm Finally : Volume, V2 = 6.5 L…

Q: final pressure

A:

Q: What volume of propane (C3H8) is required to produce 64.8 liters of water according to the followin…

A:

Q: A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas…

A: Given,  P1= initial pressure of the gas = 158 kPa  P2 = final pressure of the gas = ?  V1= initial…

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: A 280-mL flask contains pure helium at a pressure of 748 torr. A second flask with a volume of 460…

A:

Q: 10.0 g of gaseous ammonia and 6.50 g of oxygen gas are introduced into a previously evacuated 5.50 L…

A:

Q: A sample of gas has a volume of 2.03 L at a temperature of 58.10 °C. The gas sample is heated to a…

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

Q: A reaction between liquid reactants takes place at 17.0 °C in a sealed, evacuated vessel with a…

A: Welcome to bartleby !

Q: The volume of a sample of hydrogen gas was decreased from 12.01 L to 5.30 L at constant temperature.…

A:

Q: Gases exert a measurable pressure (P) on the walls of their container. The SI unit for pressure is…

A: The relationship between pressure is the pascal  and millimeters of mercury is 101325 Pa = 760 mmHg…

Q: An aerosol can contains 400.0 mL of compressed gas at 5.2 atm pressure.  When the gas is sprayed…

A: Given that: Volume of compressed gas = 400 mL = 0.400 L              Pressure of the gas = 5.2 atm…

Q: A cylinder of gas was set at a pressure of 1.45 atm and 2.53 Liters. The cylinder was compressed to…

A:

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: volume:

A:

Q: A boy with pneumonia has lungs with a volume of 2.0 L that fill with 0.085 mol of air when he…

A:

Q: Enter your answer in the provided box. A sample of sulfur hexafluoride gas occupies 7.37 L at 202°C.…

A: Initially, Volume (V1) = 7.37 L Temperature (T1) = 202°C = (202 + 273.15) K = 475.15 K Later (after…

Q: What pressure would it take to compress 350. L of helium gas initially at 1.00 atm into a 2.00 L…

A: Boyle's Law : It states that pressure of a gas varies inversely with the volume at constant…

Q: A sample of gas is collected in a balloon that can easily expand and contract. It should be noted…

A: An ideal gas is one that obeys ideal gas equation at all temperatures and pressures. A perfect ideal…

Q: In the olden days people estimated the temperature using volume of gas. if a gas bubble of volume…

A: At constant pressure, the volume of the gas is directly proportional to the temperature in kelvin…

Q: Avogadro's Law explores the relationship between volume and number of moles of an ideal gas.…

A: Answer:Avogadro's law  states that at constant temperature and pressure, volume of gas is directly…

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.