How many moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 12.0 L?

Q: A sample of gas of mass 3.66 g  occupies a volume of 515 mL  at 48 oC  and 0.24 atm  pressure. What…

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Q: What quantity in moles of chlorine gas at 120.0C and 33.3 atm would occupy a vessel of 25.0L?

A: Given,  The moles of chlorine gas at 120.°C and 33.3 atm that would occupy 25.0 L of vessel is:

Q: What volume is occupied by 0.118 mol of helium gas at a pressure of 0.97 atm and a temperature of…

A: The volume occupied by the helium gas can be calculated by the ideal gas equation as follow: In…

Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 40.0 L?

A: Temperature = T = 120°C = 393.15 K  Pressure = P = 33.3 atm  Volume = V = 40 L  No. Of moles of…

Q: What is the mass of chlorine gas present in 17.0 L at a pressure of 98.5 kPa and a temperature of 13…

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Q: How many moles of helium are contained in 890.0 mL at 21.0 °C and 99.97 kPa pressure?

A: The question is about to calculate the number of moles of Helium -

Q: How many moles of helium gas would be required to fill a 22 L container at a temperature of 35 oC…

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Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 37.0 L?

A: Ideal gas equation is given by, PV=nRT

Q: What is the volume of a mixture of 10.0 g of hydrogen gas and 10.0 g of nitrogen gas at 400 K and…

A: Given: The given mass of H2= 10 g. The given mass of N2=10 g. The temperature of the gaseous…

Q: How many moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 14.5 L?

A: To solve this problem we will use Ideal gas equation which is given below as PV = nRT  Where,  P=…

Q: What quantity in moles of chlorine gas at 120.0 degrees C and 33.3 atm would occupy a vessel of 35.0…

A: Given, Pressure (P) = 33.3 atm Volume (V) = 35.0 L Temperature (T) = 120.0 °C = (120 + 273.15) K =…

Q: Calculate the number of grams of oxygen gas represented by a sample of a pure gas at 27oC, 715 mmHg,…

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Q: When 9.81 g of neon is combined in a 100 L container at 80oC with 10.62 g of argon, what is the mole…

A: GivenMass of Ne = 9.81 gMolar mass of Ne =20.18 g/molMoles of Ne =Mass of NeMolar mass of NeMoles of…

Q: What is the pressure in atmospheres of 2.50 L of 1.5 moles of hydrogen at 230.0 K?

A: Given data,   Volume of hydrogen (V) = 2.50 L   Number of moles of hydrogen (n) = 1.5 moles…

Q: What volume is occupied by 25.8 g of argon gas at a pressure of 1.31 atm and a temperature of 467 K…

A: From ideal gas equation.         PV =nRT.         We calculate volumn of gas

Q: How many moles of chlorine gas at 120 C and 33.3 atm would occupy a vessel of 36.5L?

A: The gaseous state is the state of matter with least intermolecular force of attraction between…

Q: What volume would 1.84×1023 molecules of an ideal gas occupy at STP?

A: STP is Standard Temperature and Pressure, where temperature, T = 273.15 K and pressure, P = 100 kPa…

Q: How much pressure would 0.8 moles of a gas at 370 K exert if it occupied 17.3 L of space?

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Q: What is pressure calculated by the ideal gas equation for 1.00 mole of Cl2(g) in a volume of 1.00 L…

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Q: What volume will 9.60 moles of sulfur hexafluoride (SF6) gas occupy if the temperature and pressure…

A: If P is the pressure of the gas, V is the volume of the gas, T is the temperature of the gas in…

Q: What volume would 20.0 moles of sulfur dioxide occupy at 75.3 °C with a pressure of 2.84 atm?

A: Given: Moles of SO2 = 20.0 moles Temperature = 75.3 oC = 348.45 K Pressure = 2.84 atm

Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 13.5 L?

A: The number of moles of chlorine can be calculated by using the ideal gas equation,

Q: What quantity in moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 14.0 L?

A: The number of moles of a substance is determined as the mass of that substance upon its molar mass.…

Q: What quantity in moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 33.5 L?

A: For ideal gas PV = nRT. Or, n = PV/RT ...(1)  Here, n = moles of gas = ?,  P = pressure of gas =…

Q: What pressure, in atmospheres, will be exerted by 0.5 moles of a gas contained in a 2.4 Liter…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 24.0 L?

A: Calculate the temperature in Kelvin.

Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 12.0 L?

A: The ideal gas equation is: PV=nRT where, P is the pressure of the gas V is the volume of the gas n…

Q: What volume will 2.09 moles of nitrogen occupy at 0.947 atm and 20.0 degrees celsius?

A: Given that,  Moles of nitrogen gas n = 2.09 moles Pressure P = 0.947 atm Temperature T = 20°C  = 293…

Q: What pressure is exerted by 0.75 moles of a gas at 25°C in a container with a volume of 1.5 L?

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Q: At what temperature (in Kelvin) would 4.0 moles of hydrogen gas in a 100. liter container exert a…

A: Given :  number of moles of H2 gas (n) = 4.0 mol  volume (V) = 100. L  pressure (P) = 1.00 atm  To…

Q: What volume is occupied by 0.502 mol of CO2 at 357.9 K and 819 mmHg?

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Q: What quantity in moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 34.5 L?

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Q: How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 14.0 L?

A: Temperature of Chlorine gas (T) = 120°C = 273+120 = 393K Pressure of Chlorine gas (P) = 33.3atm…

Q: How many moles of gas are pressured in a 25L chamber containing a pressure of 750 mmHg at – 25 deg…

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Q: Calculate the pressure of one mole of an ideal gas which occupies 12.0 L at 25°C.

A: We know the relation ;  PV = nRT ( P is pressure,V is volume, n is mole number, R is gas constant,T…

Q: What is the molar mass of a gas with the density of 5.84 g/L at 1.3 ATM and 27 degrees C?

A: It is given that the density of a gas is 5.84 g/L and the pressure of the gas is 1.3 atm and at a…

Q: What quantity in moles of chlorine gas at 120.0 °C and 33.3 atm would Occupy a vessel of 18.0 L?

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Q: What volume would 1.75×1023 molecules of an ideal gas occupy at STP?

A:

Q: What mass of helium gas exerts a pressure of 965 mmHg in a volume of 5.40 L at a temperature of…

A: Assuming the gas to be an ideal gas. So according to ideal gas law, PV = nRT where, P = pressure of…

Q: How many moles of gas are present in a 2500 mL cylinder at a pressure of 2.4 atm and a temperature…

A: The moles of gas present in the cylinder is = 0.254 mol

Q: How many moles of argon gas would it take to fill a cylinder with a volume of 1.4 L to a pressure of…

A: Volume of cylinder = 1.4 L Pressure of gas = 2.5 atm Temperature of gas = 310 K No. of mol of Argon…

Q: What is the mass of xenon gas contained in a 1.4 L vessel at 3.9 bar and 319.0 K?

A: Given that, Volume of Xenon gas= 1.4 L, Temperature = 319.0 K and pressure = 3.9 bar 1 bar =0.987…

Q: What is the pressure of an 8.5 L cylinder filled with 23.5 grams of nitrogen gas at a temperature of…

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Q: How many moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 34.0 L?

A: The ideal gas equation is  PV = nRT  P = pressure of the gas V = volume of vessel n = moles of gas R…

Q: What volume would 1.20 moles of gas held under 846 torr pressure and 303 K occupy?

A: 20  Given :-  No. of moles of gas = 1.20 mol  Pressure = 846 torr  Temperature = 303 K  To calculate…

Q: How many moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 35.0 L?

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Q: Use the ideal gas equation to calculate the pressure exerted by 1.380 mol of Cl2 in a volume of…

A: A question based on ideal gas equation, which is to be accomplished.

Q: How many moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 27.0 L?

A: Record the given data, P = 33.3 atm V = 27 L R = 0.0821L.atm T = 120+273 K = 393 K

Q: How many moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 26.5 L?

A: Given, Volume of Cl2 = 26.5 L Pressure = 33.3 atm Temperature = 120°C = 120+273 = 393 K

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.