A mouse is placed in a sealed chamber with air at 750.0 torr. This chamber is equipped with enough solid KOH to absorb any CO2 and H2O produced by the mouse. The gas volume in this chamber is measured to be exactly 2.50 L, the temperature is held constant at 302 K. After two hours the pressure inside the bottle falls to 718.7 torr. What mass of oxygen has the mouse consumed?

Q: A sample of argon gas at a pressure of 0.752 atm and a temperature of 25.8 °C, occupies a volume of…

A: Given data, Initial pressure (P1) = 0.752 atm Initial volume (V1) = 441 mL Final Pressure (P2) =…

Q: The composition of the atmosphere is relatively constant, with the exception of humidity; the amount…

A: (a) Dalton's law states that the total pressure of a mixture of gaseous mixture is the sum of…

Q: The pressure of a sample of argon gas was increased from 2.91 atm to 7.75 atm at constant…

A: The initial volume is identified by using the new pressure, new volume and initial pressure since…

Q: A sample of an ideal gas at 1.00 atm and a volume of 1.09 I was placed in a weighted balloon and…

A: To find out the new volume of an ideal gas, use the formula of Boyle's law and find out the volume…

Q: 0.0380 g of Mg strip reacted completely with 6 M HCl in the gas buret and 35.8 mL of hydrogen gas is…

A: Given: The vapor pressure of water is 17.54 torr. The pressure of wet hydrogen is 747.50 torr.

Q: A sample of krypton gas at 316 K and 0.675 atm occupies a volume of 2.15 L. If the gas is allowed to…

A: where:may be written as follows when the amount this:PV=nRTwhere: P represents the gas pressure. V…

Q: partial pressure in torr due to nitrogen?

A:

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: Two samples of gas are separated in two rectangular 1.00 -L chambers by a thin metal wall. One…

A: Given: Volume = 1.00 L = 0.001 m3 Temperature =27oC = 27+273K = 300 K Pressure= 2.00 x 10-6 atm…

Q: A sample of an ideal gas at 1.00 atm and a volume of 1.91 L was placed in a weighted balloon and…

A: We have given that initial Pressure (P1) = 1 atm Volume (V1) = 1.91 L And after dropping into the…

Q: A 2.00 L reaction container at 25.0 °C contains CO2 (g) and O2 (g). The total pressure of the gases…

A: In this question, total volume of the container is to be determined on addition of 15.0 g of…

Q: “A mouse is placed in a sealed chamber with air at 762.0 torr. The chamber is equipped with enough…

A: We know that the ideal gas equation is PV = nRT , where P = Pressure V = Volume  n = number of moles…

Q: A sample of nitrogen gas was collected via water displacement. Since the nitrogen was collected via…

A:

Q: The pressure of a sample of argon gas was increased from 1.73 atm to 6.57 atm at constant…

A: Given data is as follows: The initial pressure of the gas P1= 1.73 atm The final pressure of the gas…

Q: 4. A light bulb contains 0.0560 g of Argon gas with a pressure of 1.34 atm at 26.0 °C. The light…

A: Ideal gas equation can be used to calculate P, V, T and number of moles of ideal gas:    P×V=n×R×T…

Q: A sample of solid potassium chlorate was heated in a test tube and decomposed into potassium…

A:

Q: At 535 mm Hg and 58.4 °C, a sample of carbon monoxide gas occupies a volume of 0.415 L. The gas is…

A:

Q: 4. A light bulb contains 0.0560 g of helium gas with a pressure of 163 torr at 24.0 C. The light…

A:

Q: A sample of hydrogen gas occupies a volume of 8.58 L at 48.0°C and 0.540 atm. If it is desired to…

A: Initial volume (V1) = 8.58 L Initial temperature (T1) = 48.0°C Initial Pressure (P1) = 0.549 atm…

Q: Three gases are present inside an 20.0L chamber. Argon is present at a partial pressure of 154 torr,…

A: Given that a 20.0L chamber contains,  Partial pressure of Argon gas pAr   = 154 torr Partial…

Q: A sample of nitrogen gas kept in a container of volume 2.40 L and at a temperature of 27. °C exerts…

A: Ideal gas equation is  PV = nRT  Where,  P is pressure of the gas  V is volume of the gas n is no.…

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

A: To calculate the molar mass of Mg , we would first calculate moles of hydrogen produced using ideal…

Q: sample of xenon gas at a pressure of 0.577 atm and a temperature of 23.9 °C, occupies a volume of…

A: At constant Temperature,  Using Boyle's law,  P1V1 = P2V2  0.577 × 12.6 = P2 × 19.4 P2 = 0.375 atm

Q: The total pressure within a closed vessel containing equal masses of hydrogen, helium, and argon gas…

A: Recall the expression of partial pressure partial pressure=mole fraction×total pressuregiven that…

Q: 5. A student conducts a laboratory investigation of anaerobic respiration. The student places 10.0 g…

A: We are authorized to answer three subparts at a time since you have not mentioned which part you are…

Q: A sample of an ideal gas at 1.00 atm and a volume of 1.59 L was placed in a weighted balloon and…

A: Given, P1= 1.00 atm V1 = 1.59 L P2 = 80.0 atm V2 = ?

Q: Consider a gas mixture composed of 0.200 mol N2, 0.0800 mol O2, and 0.0200 mol Ar.  The total…

A: Mole N2= 0.200  Mole O2= 0.0800  Mole Ar= 0.0200    Total mole= 0.200+0.0800+0.0200  Total mole=…

Q: A 44.0 L metal cylinder stores a sample of gas at 6 °C under 1.02 atm. The temperature of the…

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

Q: partial pressure

A:

Q: Another balloon is inflated to a volume of 1.250 L with dry hydrogen gas, at 28.0 °C. The balloon is…

A: Here, pressure is constant during the process.  Hence, Chales law is applicable

Q: A sample contianing 6.88g of solid CO2 is put in an empty sealed 5.4L container at a temperature of…

A: Using ideal gas equation  PV = nRT Where P is the pressure  V is the volume  R is the gas constant =…

Q: The volume of a sample of hydrogen gas was decreased from 11.09 L to 4.38 L at constant temperature.…

A: Boyle's law This law states that the absolute pressure exerted by a given mass of an ideal gas is…

Q: What is the new volume

A: for a ideal gas in closed flexible container, the number of the moles are constant, which gives…

Q: 1.329 x 10–2 L of H2 (g) is collected over water at a total gas pressure of 744 torr and a…

A:

Q: series of iron standard solutions need to be made from a 40 ppm iron stock solution provided. For…

A: As we know , Moles the solute remains same on dilution but volume of the solution increases.…

Q: The ideal gas law allows us to predict that: As the temperature of a gas increases, the volume of…

A: The ideal gas law allows us to predict that: As the temperature of a gas increases, the volume of…

Q: 1. A 5.85 g sample containing only MgO and CuO is placed in a 5.00 L container. The container is…

A:

Q: A sample of argon gas occupies a volume of 9.60 L at 53.0°C and 0.850 atm. If it is desired to…

A:

Q: A sample of Ne gas (5.2 L) at 5.4 atm and 25 °C was combined with 2.2 L of Ar gas at 3.6 atm and 25…

A:

Q: A mixture of gases consists of helium at a partial pressure of 400. torr, neon at a partial pressure…

A: Applying concept Doltons rule P= PHe+ PN2+ PAr

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.