A gaseous compound has a density of 1.51 g/L at 23.9 °C and 1.24 atm. What is the molar mass of the compound?

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: Write the equation for the reaction between propene and hydrogen bromide, in the presence of an…

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Q: What is the density (units of g/L) of NH3 gas (17.031 g/mol), at a temperature of 536 K and a…

A: Given -> Molar mass of NH3 = 17.031 g/mol  Temperature (T) = 536 K  Pressure (P) = 8.84 atm…

Q: How many gas molecules are present in 745 mL of propane (C3H8) at 26 °C and 364 torr pressure?

A: Volume = 745 mL            { 1 mL = 10-3 L }  Volume = 745 × 10-3 L  Volume = 0.745 L  Temperature =…

Q: The partial pressures of H2 gas and O2 gas in a mixture are 2.35 atm and 1.09 atm, respectively.…

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Q: What is the molar mass of 2.6 g of a gas that occupies a volume of 680 mL; 0.85 atm and 28oC?

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Q: A gas cylinder contains 2.2 mol of N2, 3.3 mol of O2 and 4.4 mol of Cl2. What is the partial…

A: The partial pressure (Pa) of a gas 'a' in a mixture is given by: Pa=χa×PT Here PT is the total…

Q: A sample of nitrogen gas is 1.05 L at -58 °C and 1 atm. What is the gas volume when it is heated to…

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Q: What would be the density (in g/L) of a sample of NH₃ gas at 70.0 °C and 2.50 atm of pressure?

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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.

Q: Use the ideal gas law to calculate an unknown property. A sample of O₂ gas has a volume of 811 mL,…

A: Given - Volume of O2 =811 mL = 0.811 L  (1L = 1000ml) Pressure of O2= 41 mmHg  Temperature =13.6 °C…

Q: A gas with a mass of 95.14g occupies 48.8L at 659mmHg and 25.3°C. What is its molecular weight? Use…

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Q: What volume is occupied by 5.8 g of propane gas, CaHs, at 35 °C and 1.15 atm pressure?

A: Given: Mass of propane i.e. C3H8 = 5.8 g. Temperature = 35 oC And pressure = 1.15 atm.

Q: What would be the density of a sample of CO2 gas at 70.0 degrees celcius and 2.50 atm of pressure?

A: The expression of density can be derived from ideal gas equation. PV = n R T PV = (m / M) RT d =…

Q: A 4.5 L gas cylinder contains 39.0 g of carbon dioxide (CO2) and 45.0 g of oxygen (O2) at 25 °C.…

A: Given volume of gas = 4.5 L Temperature = 25°C mass of oxygen(O2) = 45 g mass of carbon dioxide…

Q: If 3.47 g Ar are added to 4.74 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: The pressure exerted by Ar is, PV = nRTP = nRTV ......(1) No. of moles of Argon = 3.47g/(40gmol-1) =…

Q: If 3.75 g Ar are added to 4.26 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: Given mass of argon = 3.75 g Molar mass of argon = 39.95 g/mol Number of moles of argon (n) =…

Q: When some magnesium nitride, Mg3N2 reacts with water, 22 ◦C and 0.985 atm total under pressure 758…

A: The reaction of Mg3N2 with water is given as:            Mg3N2 + H2O → MgOH2  + NH3 The balanced…

Q: The total pressure of a nitrox II gas mixture for scuba diving is 2.432 atm. If the oxygen in the…

A: Given, Total pressure of a nitrox II gas mixture = 2.432 atm. Partial pressure of oxygen gas = 570…

Q: The total pressure of a mixture of gases is 0.486 atm. If the mole fraction of helium in the mixture…

A: The partial pressure of a gas  is equal to the total pressure (a mixture of gases) multiplied by the…

Q: A mixture of neon and methane gases contains neon at a partial pressure of 406 mm Hg and methane at…

A: Relation between Mole fraction and Partial pressure:  χA = nAnT = PAPT

Q: A sealed flask contains 3.1 L of a gas at 2.4 atm and 22.7 °C. If the density of the gas is 9.7 g/L,…

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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 1.65 g/L at 27.7 °C and 1.51 atm.What is the molar mass of the…

A: Here we are required to find the molar mass of the gaseous compound.

Q: What is the density (in g/L) of hydrogen gas at 19.0 ∘C and a pressure of 1665 psi ?

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Q: If 4.27 g Ar are added to 3.96 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: Temperature = 27.0 °C = 27.0 + 273.15 =300.15 K Volume = 2.00 L Pressure of He = 3.96 atm Mass of Ar…

Q: If 3.87 g Ar are added to 2.64 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: The number of moles of argon is calculated as follow 1 mole of argon = 39.95 g X mole of argon =…

Q: If 25.0 g O2 at STP is heated to 100.0°C, what is its new volume?

A: At STP Temperature(T1)=273.15K Pressure(P1)=1atm Weight=25gm T2=100°C V2=?

Q: If 1.58 g Ar are added to 3.61 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

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Q: What is the temperature, in kelvins, of 0.60 mol of a gas that occupies 2.8 L at a pressure of 4.1…

A: An ideal gas obeys the ideal gas equation which is, PV = nRTwhere,P = Pressure of gasV = Volume of…

Q: If a gas remains at constant pressure while its volume increases from 0.25Liters to 500 mL when its…

A: Given data contains, Initial volume is 0.25 L. Final volume is 500 mL=0.5 L. Final temperature is…

Q: What is the molar mass of an unknown gas with a density of 5.35 g/L at 1.00 atm and 25.0 °C?

A: SOLUTION: Step 1: The ideal gas equation is PV =nRT. Where,

Q: gaseous compound has a density of 1.78 g/L at 24.3 °C and 1.56 atm. What is the molar mass of the…

A: Given , density = 1.78 g/L Temperature = 24.3 °C = 24.3 + 273 = 297.3 K  Pressure = 1.56 atm  Molar…

Q: A sample of CO2 gas at 373.15 k has a volume of 250 mL at 1 atm. How many moles of CO2 are present?

A: We have temperature as 373.15 K, volume as 250 mL, pressure as 1 atm . We have to predict the moles…

Q: A sample of hydrogen gas at a pressure of 1.09 atm and a temperature of 29.6 °C, occupies a volume…

A: Since you have posted multiple questions, we will provide the solution only to the first question as…

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: A 33.9−L volume of methane gas is heated from 26°C to 66°C at constant pressure. What is the final…

A: Given  Initial Volume ( V1 ) = 33.9 Liter  Initial Temperature ( T1 )  = 26 ℃…

Q: If 3.23 g Ar are added to 4.22 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

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Q: If 1.52 g Ar are added to 3.41 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

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Q: A mixture of carbon dioxide and helium gases at a total pressure of 798 mm Hg contains carbon…

A: In the Question-1 we want to determine the mass of the Helium in grams. You can see step by step…

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.