A mixture of neon and argon gases is maintained in a 9.32 L flask at a pressure of 3.44 atm and a temperature of 55 °C. If the gas mixture contains 15.0 grams of neon, the number of grams of argon in the mixture is g.

Q: At a pressure of 1 atm and a temperature of 20oC, dry air has a density of 1.2256 g/L. What is the…

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Q: What is the density of a sample of argon gas at 55°C and 765mmHg?a) 2.99 g/L b) 1.13 * 103g/Lc) 1.49…

A: The given problem can be solved by using the formula as:  dRT=PM…

Q: A mixture of argon and helium gases is maintained in a 9.63 L flask at a pressure of 2.57 atm and a…

A: Ideal gas equation: where, P= pressure of the gas V= volume of the gas n=number of moles of the gas…

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A: The question is based on the concept of Boyle's law. it states that for a given amount of gas , at…

Q: If 1.04 g Ar are added to 4.83 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: We have to calculate the total gas pressure of mixture.

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Q: If 1.36 g of a gas occupies a volume of 1.00 L at 0.984 atm and 30 C, what is the molar mass in…

A: From ideal gas law, we know that  PV = nRT Where  P = pressure of the gas V = volume of gas n =…

Q: A mixture of neon and xenon gases is maintained in a 7.59 L flask at a pressure of 1.80 atm and a…

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Q: A mixture of oxygen and neon gases is maintained in a 5.98 L flask at a pressure of 2.08 atm and a…

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Q: A 3.95 g sample of an unknown gas at 69 °C and 1.00 atm is stored in a 1.75 L flask. What is the…

A: The ideal gas equation relates the pressure, volume, temperature, and number of moles of gases of a…

Q: A mixture of xenon and hydrogen gases at a total pressure of 965 mm Hg contains xenon at a partial…

A: Given-> Total pressure (P) = 965 mmHg Partial pressure of xenon (Xxe) = 313 mmHg Weight of Xe =…

Q: A 0.790 g sample of an unknown substance was vaporized in a 250. mL flask at 77.1 °C and 1.03 atm.…

A: Since the sample is finally in gaseous form. Hence the ideal gas law is applicable. According to…

Q: A gaseous compound has a density of 1.69 g/L at 25.2 °C and 1.45 atm. What is the molar mass of the…

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Q: If 4.28 g Ar4.28 g Ar are added to 2.52 atm He2.52 atm He in a 2.00 L cylinder at 27.0 °C, what is…

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Q: What mass of potassium nitrate is needed to generate 243.0 L of gas, composed of 97.00 L of N₂ and…

A: As per the guidelines, I am allowed to answer one question at a time. Please re upload the rest.…

Q: If the temperature of a gas confined to such a cylinder is raised from 221°C to 635°C, what is the…

A: Since the cylinder is confined means no change in moles of gas And pressure is also given constant…

Q: What volume of hydrogen gas is produced when 45.3 g of iron reacts completely according to the…

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Q: A 25.0 L container at 23.0 °C contains 60.54 g Ne and 167.6 g Kr. What is the total pressure of the…

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Q: What volume is occupied by a 1.83 mol sample of nitrogen gas at a temperature of 0 °C and a pressure…

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Q: A gaseous compound has a density of 1.36 g/L at 23.5 °C and 1.50 atm. What is the molar mass of the…

A: Given Density = 1.36 g/L Temperature = 23.5 oC = ( 273 + 23.5 ) = 296.5 K Pressure = 1.50 atm

Q: If the temperature of a gas confined to such a cylinder is raised from 245°C to 554°C, what is the…

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Q: At SATP, a gas has a density of 1.78 g/L. What is the molar mass of the gas?

A: We have the ideal gas law as: PV= nRT We know no of moles = given mass÷ molar mass ⇒PV = (w÷M)RT…

Q: A steel tank has a volume of 438 L and is filled with 0.885 kg of O₂. Calculatethe pressure of O₂ at…

A: Given : Volume of vessel = 438 L Mass of O2 = 0.885 Kg = 885 g…

Q: 1.55 g of an unknown gas at 65 °C and 1.10 atm is stored in a 1.65 L flask. What is the density of…

A: Mass of the unknown gas, m = 1.55 g  Temperature, T =  65 °C = 65 + 273.15 K = 336.15 K Presssure, P…

Q: A sample of gas contains 0.1300 mol of H2(g) and 6.500×102 mol of 02(g) and occupies a volume of…

A: Volume of the gas is directly proportional to the number of moles of the gas at constant pressure…

Q: 7.If container "A" is occupied by 1.0 mole of oxygen gas (molar mass 32.0 g/mol) while container "B"…

A: Using ideal gas equation,  PV=nRT  If T and P are constant then volume is directly proportional to…

Q: A 334-mL cylinder for use in chemistry lectures contains 5.225 g of helium at 23 °C. How many grams…

A: Given,Mass = 5.225 gMolar mass of helium is = 4.0 g/molVolume = 0.334 LTemperature = 23 oC = 273.15…

Q: A mixture of oxygen and chlorine gases contains twice as much oxygen (by mass) as chlorine. Ifthe…

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Q: Calculate the density of hydrogen gas (in g/L) at 899 mmHg and 42.4 °C. ______ g/L

A: According to ideal gas law PV = nRT Where , P = pressure V = volume n = moles of gas R = gas…

Q: A student collects 122. mL of hydrogen gas at 23.8 °C. The pressure of the hydrogen gas was…

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Q: A gaseous compound has a density of 1.67 g/L at 22.1 °C and 1.42 atm. What is the molar mass of the…

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Q: If the temperature of a gas confined to such a cylinder is raised from 272°C to 692°C, what is the…

A: At constant pressure, volume of the gas is directly proportional to its temperature. V1/T1 = V2/T2 =…

Q: A gaseous compound has a density of 1.64 g/L at 21.6 °C and 1.27 atm. What is the molar mass of the…

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Q: If 22.5 L of nitrogen gas at 3.5 atm are compressed to 0.8 atm at constant temperature, what is the…

A: Given: Initial volume of nitrogen gas = 22.5 L Initial pressure of nitrogen gas = 3.5 atm Final…

Q: If 4.68 g Ar are added to 4.09 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: no of moles Ar=4.6840                      =0.117no of moles of He , under given conditionAssuming…

Q: The mass of 1.12 L gas at STP is found to be 6.23 g. What is the molar mass of gas Y ?

A: Given data is: Volume of gas = 1.12 L  Given mass = 6.23 g The procedure to finding the molar mass…

Q: If 2.35 g Ar are added to 4.43 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

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Q: An ideal gas originally at 0.85 atm and 62°C was allowed to expand until its final volume, pressure,…

A: P1V1/T1 = P2V2/T2 V1 = P2V2T1/P1T2

Q: A gas initially at 4.83 L, 1.36 atm, and 81°C undergoes a change so that its final volume and…

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Q: An experiment shows that a 111 mL gas sample has a mass of 0.171 g at a pressure of 741 mmHg and a…

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

Q: If 1.79 g Ar are added to 1.18 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

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Q: An experiment shows that a 111 mL gas sample has a mass of 0.171 g at a pressure of 742 mmHg and a…

A: As from the question,Volume of gas (V) = 111 mLPressure (P) =742 mmHg.Temperature (T) = 32˚C.Mass of…

Q: A mixture of helium and nitrogen gases is maintained in a 5.66 L flask at a pressure of 1.31 atm and…

A: Given, Volume of flask = 5.66L. Pressure = 1.31atm. Temperature = 20oC = 293K. Mass of helium =…

Q: A 1.20-g sample of an unknown gas is placed in a 275.0 mL flask at 35 0C and 1.00 atm. What is the…

A: Mass of a sample = 1.20 g  Volume = 275.0 ml  ....Or  because 1L = 1000 ml    so,  = 275.0 ml × (1L…

Q: A mixture of neon and argon gases, at a total pressure of 882 mm Hg, contains 3.46 grams of neon and…

A: Given that, total pressure  (Ptotal) = 882 mmHg Mass of neon = 3.46 g Mass of argon = 2.27 g Partial…

Q: A 1.06 mol sample of hydrogen gas is collected at a pressure of 228 torr and a temperature of 15 °C.…

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Q: At 24 °C and 745 mmHg, the density of an unknown gas is determined to be 7.76 g/L. What is the molar…

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Q: A mixture of hydrogen and nitrogen gases at a total pressure of 775 mm Hg contains hydrogen at a…

A: The number of moles of hydrogen gas is calculated as,

Q: Calculate the change in volume of a 3.26 L sample of Argon, at 0.999 atm, that is heated from 22 °C…

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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.