1. What is the volume in liters (L) of 2 moles of an ideal gas at 25°C and 790 mmHg? (remember that temperature must be expressed first in Kelvin)

Q: Using the ideal gas law, PV=nRT, calculate the number of moles of gas present in a 1.50 L container…

A: Given-> Volume = 1.50 L P = 1.25 atm T= 30°C = 30+ 273 = 303K

Q: The temp of an ideal gas in a 5 . 00 L container originally at 1 . 0 atm pressure and 2 5 C is…

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Q: 3. At a pressure of 780.0 mm Hg and 24.2 °C, a certain gas has a volume of 350.0 mL. What will be…

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Q: is the molar mass of a gas that has a sample mass of 3.17 g and occupies a volume of 548 mL at 2.00…

A: Answer  Calculate molar mass of gas   Gas equation   PV   =    nRT…

Q: A flask weighs 50.1305g when clean, dry, evacuated, 150.2410g when filled with water (density =…

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Q: A 2.55 g sample of an unknown gas at 31 ∘C and 1.05 atm is stored in a 2.85 L flask. What is the…

A: First the density is determined by using density formula as shown below,

Q: A sample of gas at 840.9 mmHg and occupying a volume of 13.84 L is transferred to a smaller…

A: Boyle's law It states that at a given temperature and composition pressure of any gas is inversely…

Q: An ideal gas originally at 0.85 atm and 65°C was allowed to expand. until its final volume,…

A: Ideal gas law ,   Ideal gas law state the relation between the pressure, temperature, volume and…

Q: A 1.00 L sample of dry gas at 16 °C and 744 mmHg contains 0.520 g N₂. What is the partial pressure…

A: Given that, Volume of the dry gas is 1.00 L. Temperature = 160C Total pressure = 744 mm Hg Mass of…

Q: 0. At what temperature in Kelvin will 0.730 moles of oxygen gas occupy 6.50 L and exert 2.90 atm of…

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Q: 7. A mixture of three gases is contained in a steel tank with a volume of 2.50-L and has a total…

A: Given: Volume of the tank, V= 2.50 L Total pressure  of the gas, P = 1560 mm-Hg amount of Ne = 25%…

Q: if 19.28 L of CO2 are collected at 52 celceus, at what temperature would the volume of this gas be…

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Q: What is the molar volume of an ideal gas at 546 R and 1.00 atm? 16.9 L 89.6 L 22.4 L 11.2 L 44.8 L

A: To calculate the molar volume of an ideal gas at 546 K and 1.00 atm.

Q: A mixture of gases containing 0.362 moles of oxygen, 1.23 moles of nitrogen, and 0.0234 moles of…

A: Given: moles of O2 = 0.362 mol moles of N2 = 1.23 mol moles of Ar = 0.0234 mol Total pressure = 2.60…

Q: A 1.35 g sample of an unknown gas at 53 °C and 1.05 atm is stored in a 2.75 L flask. What is the…

A: Given: Pressure = 1.05 atm  Volume= 2.75 L  R = gas constant = 0.0821 L atm mol-1K-1 T = temperature…

Q: A sample of argon gas at standard pressure occupies 1000 ml. At constant temperature, what volume…

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Q: 2. A sample of gas occupies a volume of 10.5 L at 700 mmHg and 100°C. What would the new pressure…

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Q: A flask contains 1000 ml of a pure diatomic gas 646 mm Hg and 20 degrees mass of gas is 1.13 g. What…

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Q: A commercial airliner has an internal pressure of 1.00 atm and temperature of 25° C at takeoff. If…

A: According to ideal gas law-PV = nRTWhereP – Pressure of the gasV- Volume occupied by gasn- Moles of…

Q: A gas mixture is made by combining 8.5 g8.5 g each of Ar,Ar, Ne,Ne, and an unknown diatomic gas. At…

A: According to ideal gas law PV = nRT where P = pressure V = volume n = moles R = gas constant =…

Q: A 1.95 g sample of an unknown gas at 67 °C and 1.05 atm is stored in a 2.05 L flask. What is the…

A: The molar mass of a chemical compound is defined as the mass of a sample of that compound divided by…

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: 2. You have a 965 mL sample of methane at 92°C and a pressure of l.29x10° torr. A. How many moles of…

A: Volume of methane = 965 mL = 0.965 L Temperature = 92 oC = 273.15 + 92 = 365.15 K Pressure = 1.29 x…

Q: 4. A certain quantity of helium gas is at a temperature of 27°C and a pressure of 1.00 atm. What…

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Q: What is the total pressure in atmospheres of a gas mixture that contains 1.00 g H2 and 8.00 g Ar in…

A: Mass of H2 = 1 g Molar molar of H2 = 2 g mol-1 Mass of Ar = 8 g Molar molar of Ar =  40 g mol-1…

Q: 1) At 1.35 atm and 4.33 ∘C, a 3.91 g sample of gas occupies a volume of 1930mL. Calculate the molar…

A: From idea gas law,we know PV=nRT  Where P = Pressure  V = Volume of gas n = number of moles of gas R…

Q: A 2.35 g sample of an unknown gas at 51 °C and 1.05 atm is stored in a 1.35 L flask. What is the…

A: Given, mass of a unknown gas sample (m) = 2.35 g Temperature (T) = 51°C = (51 + 273.15) K = 324.15 K…

Q: Assuming that a 1.5 g gas occupying a volume of 500 mL at a pressure of 2.5 atm and a temperature of…

A: Consider the given information is as follows; Mass of gas = 1.5 g Volume = 500 mL = 0.5 L Pressure…

Q: What volume would 15.2 g of a gaseous compound occupy at STP if its molecular weight is 44.0 g/mole…

A: Concept is based on ideal gas:

Q: g/mol. The molecular weight of a gas that has a density of 4.1 g/L at STP is

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Q: 64. What is the pressure in millimeters of mercury of 0.0115 mol of helium gas with a volume of 214…

A: The pressure of the helium gas can be calculated by using the ideal gas equation. The ideal gas…

Q: What is the molar mass of an unknown gas with a density of 1.90 g/L at 1.00 atm and 25.0 °C?…

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

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

Q: Consider the astronaut being supplied with He and N2. The density of helium at STP is 0?179g/L and…

A: It is given that density of helium at STP is 0.179g/L and oxygen is 1.43g/L (a) According to…

Q: A 1.95 g sample of an unknown gas at 67 °C and 1.05 atm is stored in a 2.05 L flask. What is the…

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Q: What was the initial temperature in Celsius?

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

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: 0.374 m3 of hydrogen was observed at −7.0 oC and atmospheric pressure (105 Pa). The relative…

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Q: Air is approximately 78% nitrogen, 21% oxygen, and 1% argon (note that unless stated explicitly, gas…

A: Given data,Percentage of N=78%Percentage of O=21%Percentage of Ar=1%Average volume=400mLInitial…

Q: Consider a gas of volume 250 mL and a temperature of 29°C. What is the volume of this sample if the…

A: Consider a gas of volume 250 mL and a temperature of 29°C. The volume of this sample is to be…

Q: A 2.65 g sample of an unknown gas at 21 °C and 1.10 atm is stored in a 1.05 L flask. What is the…

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Q: 10. A 3.00-g sample of a mixture of K½O and BaO is placed in 600.0 cm³ vessel containing SO3 gas at…

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Q: 4 C3H5N3O9(l) + 6 N2(g) -> 12 CO2(g) + 10 H2O(g) + 1 O2(g) a. If 2.00 x 102 g worth of…

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Q: What volume in liters (L) of air measured at 1.00 atm would have to be put into a car tire with a…

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

Q: If the density of a gas is 1.2 g/L at 745 mmHg and 23.5◦C, what is the molar mass of the gas?

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

Q: Assuming that a 1.5 g gas occupying a volume of 500 ml at a pressure of 1.75 atm and a temperature…

A: Given: Mass of gas = 1.5 g. Volume of gas = 500 mL = 0.500 L…

Q: An unknown gas at 79.1 ∘C and 1.10 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior,…

A: Ideal gas equation. PV=nRT. P is pressure. V is volume. n is number of moles. R is gas constant. T…

Q: What is the molar mass of a gas that has a sample mass of 3.17 g and occupies a volume of 548 mL at…

A: Mass of gas sample (mgas) = 3.17 g Volume occupied by sample (Vgas) = 548 mL or 0.548 L Conversion:…

Q: 4. What volume would be occupied by a gas that has a pressure of 0.950atm if its volume was 1.50L at…

A: Given: Case I:Volume of gas, V1= 1.50LPressure of gas,P1=1.16 atmCase II:Volume of gas, V2=…