In the video, a 5.0 L flask at 20°C was shown, containing 1.25 mol of He and 0.50 mol of H₂, at a total pressure of 8.4 atm. Which of the following outcomes would you expect of an additional 0.50 mol of H₂ were added to the flask? Select all that apply. the mole fraction of H₂ would double the partial pressure of He would remain the same the mole fraction of He would remain the same the total gas pressure would increase by 50% the total mass of gas would increase by about 1.0 g

Q: Fluorine gas exerts a pressure of 906.5 torr. When the pressure is changed to 1.50atm, its volume is…

A:

Q: 1) A gas mixture at 20.0°C and 2.0 atm contains 0.40 mol of H2, 0.15 mol of 02, and 0.50 mol of N2.…

A: 1- First calculate the mole fraction of H2 gas :  Total moles = ( moles of Hydrogen + moles of…

Q: A mixture of N2, O2, and Ar has mole fractions of 0.25, 0.65, and 0.10, respectively. What isthe…

A: Given that,Mole fraction of Mole fraction of Mole fraction of Total pressure of the mixture=The…

Q: consider an experiment where 4.55mL of an unknown H2O2(aq) solution reacted with the yeast at 19.1 C…

A: Given , Partial pressure of O2 gas collected = 1.0126 atm moles of O2 produced = 0.004142 mol

Q: A sample of gas isolated from unrefined petroleum contains 90.0% CH4, 8.9% C2H6, and 1.1% C3H8 at a…

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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: Here given,Initial pressure (P1) = 1 atmInitial volume (V1) = 10 LInitial temperature (T1) = 298.15…

Q: In a container containing CO2, F2, and O2, what is the mole fraction of CO2 if the F2 mole fraction…

A: The mole fraction of a component in the mixture is defined by the ratio of moles of that substance…

Q: Summarize each of the gas laws (Boyle's law, Charles's law, and Avogadro's law). Drag the terms on…

A: Boyle’s Law states that the volume of the gas is inversely proportional to the pressure of the gas…

Q: 3 gases are placed in a container. The partial pressures of the component gases are: N2  0.35 atm,…

A: Using Dalton's Law of according to which total pressure of gaseous mixture is sum of partial…

Q: What is the equivalent pressure of 0.900 atm in units of mm Hg?

A: Given :- pressure = 0.900 atm  To calculate :- pressure (in mm Hg)  1 atm = 760 mm Hg

Q: Consider the reaction: 2 NO(g) + Br2(g) =2 NOB1(g) A chemist placed 0.0322 mol of NO and 1.70 g of…

A: Given equilibrium reaction is: 2NO(g)+Br2(g) ⇌  2NOBr(g) Given, volume of the reaction vessel =1.0L…

Q: consider an experiment where 4.55mL of an unknown H2O2(aq) solution reacted with the yeast at 19.1 C…

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Q: Guy-Lussac's Law only applies with liquids.  True or False?

A: We have to tell given statement is true or false

Q: 1) An aerosol can with a volume of 0.55 L has a bursting point of 2.6 atm. If the can contains 1.0 g…

A: We can solve this problem by using ideal gas equation PV = nRT  Where  P = pressure V = volume T =…

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.