A sample of hydrogen sulfide gas occupies 267 mL at 35°C and 0.850 atm pressure. What is its volume at STP?

Q: What will be the density of SO2 gas at 0oC and 1 atm

A: Given- Temperature = 0℃ = 273k Pressure = 1atm  Gas constant = 0.082 L atm mol / K Molecular weight…

Q: How many moles of gaseous arsine (AsH3) occupy 0.170 L at STP? mol AsH3 What is the density of…

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Q: A 20.0-L cylinder containing 11.34 kg of butane, C4H10, was opened to the atmosphere. Calculate the…

A: An ideal gas is defined as the collisions between the molecules or atoms that are perfectly elastic…

Q: A 15.0 g sample of gas occupies 23.2 L at STP. What is the molecular weight of this gas?

A: Weight of gas = w = 15.0 g  Volume of gas = V = 23.2 L  R = 0.082057 L atm K-1mol-1  STP :-…

Q: What is the volume for 1.00 mole of gas at STP? _______L

A: Given that,  Number of mole of gas=1.00 mole Know that, standard volume= 22.4L / mol We know that,…

Q: A 1.65 g sample of an unknown gas at 45 °C and 1.10 atm is stored in a 1.25 L flask. What is the…

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Q: The density of chlorine gas at STP, in grams per liter, is approximately:     none of the given…

A: In this question, we want to determine the density of Chlorine gas at STP. You can see details…

Q: 1.50 L of gas at 2.25 atm pressure expands to a final volume of 8.10 L. What is the final gas…

A: The experimental gas law relating pressure and volume of gas is called Boyles law. It states that…

Q: A sample of gas occupies 4.23L at 3.46 atm. what is the volume at 2.25 atm? (assume T is a constant

A: Given P1 = 3.46 atm V1 = 4.23 L P2 = 2.25 atm V2 = ?

Q: potassium chlorate is needed to produce 20.0 mL of oxygen gas at 700. mmHg and 20. °C? 1leent dlaite

A: Volume = 20 mL = 0.020 L Pressure = 700 mm Hg     = 700/760 = 0.921 atm Temperature = 20 °c = 293 K…

Q: A gas at 813mmHg and 38 degrees celsius occupies a volume of 6.70L. Calculate its volume at STP.

A: Given Pressure of Gas =813 mmHg Temperature = 38o C Volume= 6.70 L To calculate Volume of the Gas at…

Q: What is the molar mass of a gas ?whose density at STP is 3.74 g/L g/mol 83.8 .A g/mol 5.99 .B g/mol…

A: STP( standard temperature and pressure) at STP the 1Mole of  a gas attains 22.4 Liter volume.   So,…

Q: What volume (in L) will 50.0 g of nitrogen gas occupy at 2.0 atm of pressure and at 65 °C? PV = nRT…

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Q: What is the mass (in grams) of 2.00 L of NH₃ at STP? R = 0.08314 L･bar/mol･K.

A: At STP, volume of 1 mole of a gas is 22.4 L Mass of NH3 =?

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

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Q: At 450 mm Hg and 72.0°C, a sample of carbon monoxide gas occupies a volume of 0.225 L. The gas is…

A: For such type of question we can use the direct formula of combined gaseous equation.  ( P1 * V1/ T1…

Q: A 1.65 g sample of an unknown gas at 55 °C and 1.00 atm is stored in a 2.45 L flask. What is the…

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Q: An ideal gas mixture having a temperature of 27 °C and a total pre contains 0.150 g H2, 0.700 g N2…

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Q: 8. (a) A 50.0 g sample occupies 11.2 L at STP. Calculate the molecular weight of this gas. (R =…

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Q: How many Lof chlorine gas are required to react with excess hydrogen gas to produce 64 L HCl gas at…

A: Given,  Volume of HCl gas  = 64 L We know, at STP 1 mole of any gas = 22.4 L   of volume

Q: How many miles of ozone occupy a volume of 3.36 L at STP?

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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: Burning one mole of propane in a gas grill adds 132 g of carbon dioxide (CO 2) to the atmosphere.…

A: At STP, 1 mole of a gas occupy 22.4 L of volume.

Q: An 8.00 g sample of gas occupies 22.4 L at 2.00 atm and 273K. What is the molar mass of the  gas? (R…

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Q: At 105.1 oC and 0.4500 atm pressure, a gas occupies a volume of 0.600 L.  How many liters will it…

A: Gas laws , PV = nRT  P1V1/T1 = P2V2/T2

Q: gas occupies a volume of 53.5 L and exerts a pressure of 695 mm Hg at 25.0 °C. What volume will the…

A: Given: Volume of gas = 53.5 LPressure = 695 mm HgTemperature = 25.0oC To find: Volume of the gas at…

Q: What mass of neon gas is required to fill a 5.00-L container to a pressure of 1.02 atm at 25 degrees…

A: According to the ideal gas law, PV = nRT where P = pressure in atm = 1.02 atm V = volume in L = 5.00…

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: gas at 1.02 atm and 35.0° C occupies a volume of 6.85 L.  Calculate its volume at STP.

A: Initial pressure(P1) = 1.02 atm Initial Volume(V1) = 6.85 L Initial Temperature(T1) = 35 +273= 308 K…

Q: Consider a 1.0-L container of neon gas at STP. Will the average kinetic energy, average velocity,…

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Q: 1.A sample of hydrogen fluoride gas occupies 1250 mL at STP. What is the pressure in mmHg if the…

A: Since you have posted multiple Ques.We will solve the first question for u. To get the remaining…

Q: A gas occupies 45.0 L at 2.00 atm pressure and 27°C. Calculate its volume at STP.

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Q: A 3.35 g sample of an unknown gas at 23 'C and 1.10 atm is stored in a 3.05 L flask. What is the…

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Q: A gas occupies a volume of 0.850 L at 74 °C and 1.00 atm pressure. What will be its volume at 0 °C…

A: The combined gas law expresses the relationship between the pressure, volume, and absolute…

Q: What mass (in grams) of CO₂ gas is contained in a 1.50 L flask of carbon dioxide at a pressure of…

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Q: 39. A 20.0-L cylinder containing 11.34 kg of butane, C4H10, was opened to the atmosphere. Calculate…

A: The ideal gas equation is shown below: PV = nRT Where; P = pressure of the gas V= volume of the gas…

Q: A 1.85 g sample of an unknown gas at 47 °C and 1.00 atm is stored in a 2.85 L flask. What is the…

A: Given: Mass, m =1.85 g Volume , V =2.85 L Pressure, P = 1.00 atm Temperature, T = 47 +273 = 320 K…

Q: A sample of gas at 9.18.5 mmHg occupying a volume of 13,02 L is transferred to a larger container of…

A: Given : Initial Pressure (P1) = 9.185mmHg 1 mmHg = 0.133322KPa Therefore, 9.185mmHg = 1.2245661KPa…

Q: If 0.211 g of gas occupies 204.5 mL at STP, what is the molecular weight of this gas? R = 0.08206…

A: We have to calculate the molar mass of gas.

Q: What is the pressure of a 1.5 L flask containing 0.60g of He at 27°C? (R= 0.0821 L atm/ mol K)

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

Q: What is the density of O2 gas in g/L at STP ?

A: Using the formula of density and ideal gas equation we can find density of O2 at STP.

Q: 1. A sample of gas occupies a volume of 0.65 L at 24°C and 1.02 atm. a. calculate the new volume at…

A: Volume = 0.65 L  Temperature = 24°C = 24+273 = 297 K  Pressure = 1.02 atm  a) at STP -  Temperature…

Q: During the decomposition of KClO3, 92.0 mL of gas is collected by the displacement of water at 250C…

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Q: A sample of a gas originally at 25 °C and 1.00 atm pressure in a 2.5 L container is allowed to…

A: For the phase change of the ideal gas the temperature, pressure, and volume of the initial state and…

Q: A 1.25 g sample of an unknown gas at 47 ∘C and 1.00 atm is stored in a 2.55 L flask. What is the…

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Q: A person accidentally swallows a drop of liquid oxygen, O2(l), which has a density of 1.149 g/mL.…

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Q: What mass (in grams) of CO2 gas is contained in a 1.50 L flask of carbon dioxide at a pressure of…

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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: Calculate the density of CO2 in g / L , at STP. Calculate number of moles of gas that occupies a…

A: here we are required to find the density of carbon dioxide at STP.

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.