You inflate a balloon with 2.0 L air at a temperature of 10°C  and then increase the temperature to 45°C. You noticed that the volume of the balloon has changed. Assuming the pressure and moles of gas remains constant; calculate the “new” volume, in Liters, of the balloon at 45°C. Given: V1/T1 = V2/T2, K = 273 +°C A. 2.8 L B.2.3 L

Q: A tank was filled with 12 g of oxygen (O2), 73 g of nitrogen (N2) and 4 g of carbon dioxide(CO2). At…

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A: we have to calculate the final pressure of methane gas

Q: A 5.00 L tank at 4.81 °C is filled with 17.5 g of sulfur hexafluoride gas and 4.15 g of chlorine…

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Q: O GASES Calculating mole fraction in a gas mixture A 5.00 L tank at 6.1 °C is filled with 3.82 g of…

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Q: A sample of gas contains 5.25 moles at 37.8 °C in a volume of 3.61 L. If 2.67 moles of gas are…

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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: Amixture of methane and hydrogen gases contains methane at a partial pressure of 505 mm Hg and…

A: Generally the mole fraction is determined by dividing partial pressure by total pressure. First…

Q: A 6.00 L tank at 18.7 °C is filled with 5.93 g of carbon monoxide gas and 2.28 g of sulfur…

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Q: The ideal gas law, R, can be experimentally determined. Use the data provided below from the…

A: Answer:Here:

Q: The pressure of a gas is 380 mm Hg. Express this pressure in units of a. atmospheres. Pressure = b.…

A: Given:The pressure of a gas is 380 mmHg.We have to convert the pressure at different units.

Q: A 10.0L tank at 0.96°C is filled with 6.10g of dinitrogen difluoride gas and 16.0g of sulfur…

A: we have to calculate  mole fraction and partial pressure of each gas total pressure

Q: At 100 kPa and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C3H8) combusts, producing 18.0 g…

A: In this question, we have to Calculate the mole fraction of each gas in the initial mixture.

Q: Consider the following samples of gas: sample composition pressure temperature A 2.8mol Krg 2.6atm…

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Q: Consider a box divided in half. One side is filled with 1 mol Ne at 300 Kelvin, and the other is…

A: Since the gases are effusing through a small hole to reach the equilibrium  And as per the graham's…

Q: A 6.00 L tank at 8.99 °C is filled with 6.56 g of dinitrogen monoxide gas and 11.8 g of sulfur…

A: Below attached file showing the details answer  All the best.

Q: An unknown gas has a density of 1.48 g/L and a molar mass of 68.2 g/mol. You have measured the…

A: For the ideal gas, the temperature pressure and the volume are related by the ideal gas equation.…

Q: The ideal gas law, R, can be experimentally determined. Use the data provided below from the…

A: Answer:Here:

Q: 10.0L tank at 1.21°C is filled with 9.54g of dinitrogen difluoride gas and 13.5g of chlorine…

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Q: Consider a gas mixture of nitrogen (N2) and methane (CH4) of total mass 80g. 31.14% of the total…

A: Total pressure of the gas mixture :-         Total pressure exerted by a mixture of ideal gasse…

Q: If pressure is expressed in atmospheres and volume is expressed in liters, PAV has units of Latm…

A: Given,  The energy : 4  L. atm 1atm = 101325 Pa.  1 L = 1 dm3 .

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

A: According to the ideal gas law: PV = nRT where P, V, n, R and T represent pressure, volume, number…

Q: Calculate the total pressure (in atm) of a mixture of 0.0200 mol of helium, He, and 0.0100 mol of…

A: Ideal Gas Law :-  PV = nRT  P is the pressure of gas  V is the volume occupied by gas n is the…

Q: The volume of 3.3mol of ideal gas is 45.7L at 350K. Calculate its pressure (in atmospheres).

A: The pressure of the gas can be calculated by using the ideal gas equation, which is expressed as…

Q: A 10.0 L tank at 28.7 °C is filled with 4.80 g of sulfur tetrafluoride gas and 13.4 g of chlorine…

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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: To identify a diatomic gas (X2X2), 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.

Q: A tank was filled with 11 g of oxygen (O2), 87 g of nitrogen (N2) and 6 g of carbon dioxide(CO2). At…

A: we know, Molar mass of O2 = 32 g/mol Molar mass of N2 = 28.0134 g/mol Molar mass of CO2 = 44.01…

Q: A 8.00 L tank at 28.6 °C is filled with 11.1 g of sulfur hexafluoride gas and 6.50 g of carbon…

A: Volume of tank = 8 LTemperature = 28.6°CMass of SF6 = 11.1 gMass of CO = 6.50 gWe have to findMole…

Q: The van der Waals coefficents of mnatomic argon gas are a=0.003412m6 Pa/mol2 and b=23.7 x 106…

A: According to the question we have, Vander Waal coefficient of monoatomic argon  gas is given by, a=…

Q: Determine the pressure of 2.581 moles of an ideal gas to THE WHOLE NUMBER in atm that has a volume…

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Q: If pressure is expressed in atmospheres and volume is expressed in liters, PAVhas units of Latm…

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Q: A 9.00 L tank at 12.6 °C is filled with 7.50 g of carbon dioxide gas and 13.2 g of dinitrogen…

A: Given  Volume ( V ) = 9 L  Temperature ( T ) =  12.6 ℃                              =  (12.6 + 273…

Q: A 5.00 L tank at 8.18 °C is filled with 17.3 g of sulfur tetrafluoride gas and 4.95 g of chlorine…

A:

Q: A 10.0 L tank at 19.1 °C is filled with 6.04 g of dinitrogen difluoride gas and 7.73 g of chlorine…

A: Molar mass dinitrogen difluoride gas is 66.010 g/mol Molar mass chlorine pentafluoride gas is…

Q: 6. Gas containers A and B each contains an ideal gas at low pressure and 298 K. The volume of…

A: Given that, the gas containers A and B have ideal gases at low pressure and 298 K temperature. Now,…

Q: Using the ideal gas law (PV=nRT), calculate how many moles of air are in the lungs of an average…

A: Using ideal gas law we can write pV = nRT Where p = Pressure of system  V = volume of gas n = moles…

Q: For many purposes we can treat propane (C3Hg) as an ideal gas at temperatures above its boiling…

A: Answer:Here:

Q: A 10.00 L tank at 5.3 °C is filled with 5.84 g of carbon dioxide gas and 4.39 g of chlorine…

A: In the given question ->Volume of tank = 10.00 LTemperature = 5.3°CWeight of CO2 = 5.84 gmWeight…

Q: A 7.00 L tank at 6.54 °C is filled with 17.3 g of sulfur tetrafluoride gas and 17.7 g of chlorine…

A: Given : Mass of sulfur tetrafluoride i.e SF4 = 17.3 g Mass of chlorine pentafluoride i.e ClF5 = 17.7…