Give an example of a "real life application" of Boyle's Law. What is the gas law that applies to your example and describe the relation of the 2 variables involved in the gas law.

Q: What is Boyle’s law? Explain Boyle’s law from the perspective of kinetic molecular theory

A: Boyle’s law has to be defined. Boyle’s law from the perspective of kinetic molecular theory has to…

Q: 1. A gaseous compound that actually exists in the environment. 2. It is made up of small particles…

A: 1. REAL 2. REAL 3. BOTH 4. IDEAL 5. IDEAL 6. IDEAL 7. BOTH

Q: The partial pressures of H2 gas and O2 gas in a mixture are 2.35 atm and 1.09 atm, respectively.…

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Q: General: 2.0 L of O2(g) and 8.0 L of N2(g) , each at STP, are mixed together. The non-reactive…

A: Given that : The volume of oxygen gas = 2.0 L The volume of nitrogen gas = 8.0 L At STP, the…

Q: The deviation from ideal behavior of a gas is most evident at high temperature. Explain

A: Given statement: The deviation from ideal behavior of a gas is most evident at high temperature.

Q: In a mixture of hydrogen and nitrogen gases, the mole fraction of nitrogen is 0.333. If the partial…

A: Given,The mole fraction of nitrogen is 0.333,The partial pressure of hydrogen in the mixture is 75.0…

Q: determine the temperature

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Q: Using the Ptotal from question #1 and the partial pressure of Gas B, determine the mole fraction,…

A: Hi. Since your question has multiple parts, we will solve the second question for you. If you want…

Q: What is Boyle law?

A: Gas laws gives the relationship between temperature, pressure and volume of a gas.

Q: Consider a mixture of 2 lit of CH4 and 7 Lit of C3H7. Calculate mole fraction of both gases.

A: Volume of CH4 is 2 L Volume of C3H7 is 7 L Mole fraction of both = ?

Q: A gaseous mixture contains 435.0 Torr H2(g), 387.5 Torr N2(g), and 85.3 Torr Ar(g). Calculate the…

A:

Q: How does the partial pressure of gas A in a mixture compare to its mole fraction in the mixture?…

A: How does the partial pressure of gas A in a mixture compare to its mole fraction in the mixture has…

Q: A chamber contains equal molar amounts of He, Ne, Ar, and Kr. If the total chamber pressure is 1…

A: Given: Total pressure of the chamber is 1 atm And moles of all gases are equal.

Q: The gas from an active volcano had the following composition in mole percent; 65 % CO,, 25% H, 5.4 %…

A: The partial pressure of a substance is equal to the product of its mole fraction and pure vapor…

Q: A mixture of 5.00 moles of neon gas and 3.00 moles of nitrogen gas, N2, occupy a vessel where the…

A: Given :  Number of moles of Ne = 5.00 mol  Number of moles of N2 = 3.00 mol  Total pressure = 6.00…

Q: Answer the following and note that this is seriously not out of scope for Solutions. 3.) Which…

A: The kinetic theory of gases is summarized as below: 1) The gas particles are smaller compared to the…

Q: The atmospheric concentration of CO2 gas is presently 407 ppm (parts per million, by volume; that…

A: Given,The atmospheric concentration of CO2 gas is 407 ppm (or) 407 L of every 106 L of atmosphere…

Q: What gas law is applied in the operation of hot air balloon? Gay-Lussac's law Charles's law…

A: Which gas law is applied in the operation of hot air balloon :

Q: A gaseous mixture contains 421.0 Torr H₂(g), 339.1 Torr N₂(g), and 89.5 Torr Ar(g). Calculate the…

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Q: In the Dumas Method for the determination of the molar mass of a vapor, it was assumed that the…

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Q: A gaseous mixture contains 421.0 Torr H, (g), 370.1 Torr N, (g), and 75.9 Torr Ar(g). Calculate the…

A:

Q: If He(g) has an average kinetic energy of 6750 J/mol under certain conditions, what is the root mean…

A: The root mean square velocity of gas is inversely proportional to the square root of its molecular…

Q: What is the effect on the volume of 1 mole of an ideal gas if both the pressure and the temperature…

A: For an ideal gas: PV = nRT Where, P = pressure (atm); V = volume (L); n = number of moles; R = gas…

Q: If an ideal gas initially at 0.8 bar and 1.7 L is compressed at constant temperature to a volume of…

A: An ideal gas initially at 0.8 bar and 1.7 L is compressed at constant temperature to a volume of 0.9…

Q: Calculate the root mean square velocities of CH4(g) and N2(g) molecules at 273 K and 564 K.

A: To find: The root mean square velocities of CH4(g) and N2(g) molecules at 273K and 564K

Q: Define the term Mole Fraction?

A: The term mole fraction has to be defined.

Q: A gaseous mixture contains 420.0 Torr H, (g), 361.7 Torr N, (g), and 82.1 Torr Ar(g). Calculate the…

A: In the given question we have to calculate the mole fraction ' X ' of each gases. Given data :…

Q: Which of the following gas laws allows the approximation of the absolute zero by extrapolation?…

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Q: For a gas sample whose total pressure is 740 torr, what are the partial pressures if the moles of…

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Q: At what temperature (in °C) would one liter of ethene gas, C2H4, have a mass of 1.166 g, if the gas…

A: A mole of a substance refers to the mass of that substance which will contain same number of   atoms…

Q: The volume of a sample of pure HCl gas was 189 ml at 25°C and 108 torr. It was completely dissolved…

A: Given that,  Volume of HCl gas = 189ml = 0.189L Pressure = 108torr = 0.142atm Temperature = 25°C =…

Q: At constant temperature, how can you express the rate of change of the pressure in an ideal gas law,…

A: From the ideal gas equation:

Q: What is Boyle’s law, and what variables must be kept constant for the law to hold?

A: Boyle's law is a gas law which states that the pressure exerted by a gas (of a given mass, kept at a…

Q: 2. A cylindrical tank with piston on top confines a 543.78 K of hydrogen gas in a 1.34 m' space…

A: Pressure , temperature and volume are interrelated for a gas by various laws.

Q: 1. Which one of the three varlables: Pressure, Volume or Temperature cannot be changed in Boyle's…

A: To answer questions regarding Boyle's Law.

Q: How does the root mean square velocity of an ideal gas vary as the molar mass of the gas increases?…

A: The relation between root mean square velocity of an ideal gas and its molar mass is to be…

Q: How does the partial pressure of gas A in a mixture compareto its mole fraction in the mixture?…

A: Partial pressure: It is the pressure that is exerted by individual gaseous atoms or molecules in a…

Q: A diver breathes a helium and oxygen mixture with an oxygen mole fraction of 0.050. What must the…

A: Mole fraction of the oxygen gas = 0.050 Partial pressure of the oxygen gas = 0.20 atm

Q: gaseous mixture contains 4.56 g propane, C3H8, and 1.22 g chloroform, CHCL3. Assuming that both…

A: Mass of propane  = 4.56 g Mass of chloroform = 1.22 g V = 100 ml = 0.1 L  T = 28oC  = 301 K Molar…

Q: How are Van der waal’s constants ‘a’ and ‘b’ related to the tendency to liquefy?

A: The Vanderwall’s equation of gas is: where P represents the pressure, V represents the volume, n…

Q: In what situation would we rather use a Erlenmeyer flask over a beaker if both cannot be used to…

A: Erlenmeyer flask has a narrow neck and the beaker has a wide-open mouth.

Q: Mass of flask +cap= 96.421g temp. of boiling water= 100 C Mass of flask+ cap+ condensed vapor=…

A: 1) Calculation of the average mass of the flask + cap + vapor: Average mass=97.005 g+96.957 g+96.984…

Q: How can the ideal gas law be used to find the molar mass of an unknonwn liquid?

A: Molar mass of unknown liquid can be calculated by Dumas method. In this method we vaporize the…

Q: P

A:

Q: What is the significance of the critical constants of a gas?

A: Critical constant can be described as the constant which indicates the point above which it is…

Q: Which assumptions of the kinetic–molecular theory explain the behavior of gases described by Boyle’s…

A: The kinetic molecular theory has the following postulates:

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.