A fixed amount of gas in a capped syringe at 7 C has a volume of 12.0 mL. After heating the gas in a hot water bath, a student finds that the volume of the gas has expanded to 15.0 mL. If the pressure remains constant, what is the new temperature of the gas?

Q: A 10.0 L flask contains a mixture of neon and argon gases at a pressure of 2.38atm. Calculate the…

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Q: A sample of gas contains 0.1600 mol of HBr(g) and 0.08000 mol of Cl₂ (g) and occupies a volume of…

A: As per Dalton's law, volume and number of moles are directly proportional to each other.

Q: Calculate the final pressure of the gas. Be sure your answer has the correct number of significant…

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Q: A mixture of helium, nitrogen and oxygen has a total pressure of 755 mm Hg. The partial pressures of…

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Q: For many purposes we can treat methane (CH4) as an ideal gas at temperatures above its boiling point…

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Q: Chloroform is a common liquid used in the laboratory. It vaporizes readily. If the pressure of…

A: The given data contains, density =1.25 g/L Pressure =170 mm Hg =0.223684 atm Temperature =25°C =298…

Q: b. How many moles of hydrogen are in this sample?

A: An ideal gas equation is derived from the combination of Charle's law, Boyle's law, and Avogadro…

Q: Xenon fluoride can be prepared by heating a mixture of Xe and F2 gases to a high temperature in a…

A: Let us consider the reaction between xenon and fluorine produces the compound XeaFb, where a and b…

Q: A sample of argon gas occupies a volume of 7.82 L at 50°C and 777 mm Hg. The volume of the gas…

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Q: Use the ideal gas law to calculate an unknown property. A sample of O₂ gas has a volume of 811 mL,…

A: Given - Volume of O2 =811 mL = 0.811 L  (1L = 1000ml) Pressure of O2= 41 mmHg  Temperature =13.6 °C…

Q: A mixture of neon and argon gases exerts a total pressure of 7.9 atm. The partial pressure of the…

A: Given Data: Total Pressure (PTotal) = 7.9 atm Partial pressure of the neon (PNeon)  = 2.09 atm

Q: For many purposes we can treat methane (CH4) as an ideal gas at temperatures above its boiling point…

A: Thank you,Please rate my response.

Q: A closed one litre container at 298 K contains one mole of argon gas. a) What effect would each of…

A: Given, Temperature = 298 K Volume = 1L

Q: For many purposes we can treat methane (CH4) as an ideal gas at temperatures above its boiling point…

A:

Q: Which of the following is true for a gas under conditions of very low temperature? PV ÷ nRT = 1,…

A: To solve this problem we have to know about ideal gas equation.

Q: The temperature of a 501 mL sample of gas decreases from 251 K to 140 K. What is the final volume of…

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

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Q: 2)Boyle's Law D' states that for a certain gas in a container we have P • V = 375 where P represents…

A: Given the Boyle's law relation is: P*V = 375 where pressure, P is in pressure in mm Hg, and  volume,…

Q: A sample of helium gas at 283 K and 1.01 atm occupies a volume of 4.53 L. If the gas is compressed…

A: Answer:When number of moles of gas n are constant and since, R is always a constant, then nR will…

Q: What is the pressure in kilopascals of 1.926 x 10-6 moles of helium gas, if it occupies a volume of…

A: Ideal behaved gas and pressure calculation using ideal gas equation

Q: If 3.87 g Ar are added to 2.64 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: The number of moles of argon is calculated as follow 1 mole of argon = 39.95 g X mole of argon =…

Q: To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an…

A: Using the ideal gas equation, we can calculate the molar mass of the diatomic gas.The ideal gas…

Q: A mixture that's 35.0% N2 and 65.0% O2 by volume has a total pressure of 2500. psi. What is the…

A: To solve this problem we have to use the concept of Dalton Law of Partial Pressure.

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

A: where:when the pressure is doubled, the ammonia's temperature may be changed while maintaining a…

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

A: The given data contains, CH4 =90.0%Ethane=8.9%Propane =1.1%Total Pressure =307.2 kPa

Q: A flask contains 740 mmHg of nitrogen (N2) gas in a 4.00 L container at 25.0 °C. If 44.0 g of carbon…

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Q: A student recovered0.398g of THF vapor in a 125 mL flask. Assuming the vapor is an ideal gas with a…

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Q: A 10.0 L container at 19 °C contains 32.0 g CH4 and 15.0 g C2H6. What is the total pressure of the…

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Q: What height of water (in meters) is necessary to measure a pressure of 760 mm Hg? The density of…

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

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Q: partial pressure of each component of this gas

A: The total gas contains 90.0% of CH4, 8.9 % of C2H6 and 1.1% C3H8 So, Partial pressure of CH4 is –

Q: 7. At what temperature does 456 mL of gas exist if it expands to 3.4 L at 65.0 °C?

A: The temperature and volume are directly proportional to each other.

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

A: Answer:For a fixed mass of gas, value of  for any gas sample remains constant, therefore,

Q: For many purposes we can treat nitrogen (N₂) as an ideal gas at temperatures above its boiling point…

A: We can solve this question by using ideal gas equation i.e. PV= n RT whereP = pressure of gas, V =…

Q: A mixture of neon and argon gas exerts a total pressure of 2.39 atm. The partial pressure of the…

A:

Q: For many purposes we can treat methane (CH4) as an ideal gas at temperatures above its boiling point…

A: The Ideal Gas equation is given by,PV = nRTwhere,P= Pressure in atmV = Volume in LT = Temperature in…

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

A: Given: The initial and final temperature of ammonia gas is -12.0˚C and 21.0˚C, respectively. The…

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.