A sample of an unknown gas is found to have a density of 2.60 g/L at a pressure of 0.926 atm and a temperature of 31 °C. Assume ideal behavior. The molar mass of the unknown gas is g/mol.

Q: A 1.35 g sample of an unknown gas at 43 ∘C and 1.10 atm is stored in a 1.45 L flask. What is the…

A: The density is calculated by using given mass and volume.

Q: A sample of xenon gas occupies a volume of 6.95L at 431K. If the pressure remains constant, at what…

A: Initial volume, V1 = 6.95 L Initial temperature, T1 = 431 K Final volume, V2 = 3.77 L Final…

Q: The pressure required to decrease the volume of a gas at 1.25 atm by 25% at constant temperature is…

A: Given: pressure=1.25 atmdecrease in volume=25% To find: Pressure required to decrease the volume of…

Q: An unknown gas at 67.1 ∘C and 1.05 atm has a molar mass of 28.01 g/mol. Assuming ideal behavior,…

A: We will is use ideal gas equation to get the density.

Q: If gaseous mixture is made of 2.41 g of He and 2.79 g of Ne in an evacuated 1.04-L container at 25…

A:

Q: If the initial temperature of an ideal gas at 2.250 atm is 62.00 ∘C, what final temperature would…

A: Given : Initial temperature of gas = 2.250 atm  Initial temperature of gas = 62.00 oC And final…

Q: A sample of helium gas at a pressure of 923 mm Hg and a temperature of 72 °C, occupies a volume of…

A:

Q: If a gas occupies 120 L at 9 atm, what volume will it occupy at standard pressure?

A:

Q: A 3.55 g sample of an unknown gas at 23 ∘C and 1.05 atm is stored in a 3.05 L flask. What is the…

A:

Q: A 6.96 gram sample of an unknown gas is found to occupy a volume of 2.10 L at a pressure of 912 mmHg…

A: Given that: mass of sample = 6.96 g volume of gas = 2.10 L pressure of gas = 912 mmHg temperature =…

Q: A large flask with a volume of 936 mL is evacuated and found to have a mass of 134.66 g. It is then…

A: step 1: Here, given as the: Thus, the mass of gas is 1.38g. Now, to calculate the molar mass,…

Q: Determine the final pressure of a gas, initially at 3.0 L, 2.2 atm, and 72oC, which undergoes a…

A:

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 certain mass of nitrogen gas occupies a volume of 2.47 L at a pressure of 2.72 atm. At what…

A: Given that Initial pressure = P1 = 2.72 atm Initial volume = V1 = 2.47 atm Final volume = V2 = 4.85…

Q: A gas sample containing 0.6838 moles is trapped in a chamber with a volume of 7.557 liters.  If the…

A: n = 0.6838 molV = 7.557 LT = 298.17 K

Q: A certain mass of nitrogen gas occupies a volume of 3.88 L at a pressure of 6.54 atm. At what…

A: At constant temperature conditions the P and V are inversely proportional to each other. That is P x…

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…

A:

Q: What volume is occupied by a 1.02 mol sample of hydrogen gas at a temperature of 0 °C and a pressure…

A: The ideal gas equation is PV = nRT P = pressure of gas  V = Volume of gas  n = number of moles of…

Q: A 1.75 g sample of an unknown gas at 47 C and 1.00 atm is stored in a 1.85 L flask. What is the…

A:

Q: 2.58 gram sample of an unknown gas is found to occupy a volume of 1.53 L at a pressure of 687 mmHg…

A: Given that:  Mass of gas = 2.58g Volume(V) = 1.53L P = 687 mmHg = 687mmHg×1atm/760mmHg = 0.9039atm T…

Q: A 1.95 g sample of an unknown gas at 61 ∘C and 1.00 atm is stored in a 1.45 L flask. What is the…

A: Given information:Mass of sample = 1.95 gTemperature = 61 °CPressure of gas = 1.00 atmVolume of…

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

A:

Q: At 1.00 atm and 4.67 °C, a 2.72 g sample of gas occupies a volume of 1540 mL. Calculate the molar…

A: Given - - > P = 1 atm T =4.67 °C = 277.82 K V=1540 ml =1.54 L m = 2.72 g R = 0.08206…

Q: A sample of hydrogen gas at a pressure of 903 torr and a temperature of 26.9°C, occupies a volume of…

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

Q: If we have a sample of gas at 1.67 atm and 76.3°C, what would happen to the temperature if the…

A: The question is based on the concept of Gay-lussac's law.   it states that for a given amount of gas…

Q: A  2.75 g gas occupies 450 mL at 37 0C and 1.50 atm. What is the molar mass of the gas?

A:

Q: An unknown gas at 49.1 C and 1.05 atm has a molar mass of 30.07 g/mol. Assuming ideal behavior, what…

A: The formula required to determine the density of gas with ideal behavior is as follows,

Q: The following are a list of parameters of a gas in a sealed container: Initial Pressure = 1.50 atm…

A: Initial Pressure = 1.50 atm Initial volume = 2 L Initial temperature = 27 °C     ( 0°C = 273.15 K  )…

Q: An unknown gas at 21.1 °C and 1.05 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior,…

A:

Q: A 2.05 g sample of an unknown gas at 59 ∘C and 1.10 atm is stored in a 2.85 L flask. What is the…

A: Given,Mass of the sample = 2.05 gVolume is 2.85 LTemperature = 273.15 K + 59 = 33.152 KPressure =…

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:

Q: Determine the mole fraction of each gas in a mixture whose partial pressures are 0.467 atm of He,…

A: Given, a mixture of gas of He, Ar and Xewhose partial pressures are 0.467 atm of He, 0.317 atm of…

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

A:

Q: What volume does 0.118 mol of helium gas at a pressure of 0.97atm and a temperature of 305K occupy

A: Applying ideal gas equation PV = nRT

Q: A sample of an unknown gas is found to have a density of 1.97 g/L at a pressure of 0.762 atm and a…

A:

Q: An unknown gas at 73.1 ∘C and 1.05 atm has a molar mass of 44.10 g/mol. Assuming ideal behavior,…

A: Ideal gas equation is the equation which obeys all gas laws under all condition of temperature and…

Q: A gas sample with a mass of 11.2 g exerts a pressure of 1.05 atm at 22.0ºC and a volume of 2.79 L.…

A:

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: 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 1.58 gram sample of an unknown gas is found to occupy a volume of 0.886 L at a pressure of 658 mm…

A: Molar mass of unknown gas can be calculated by using ideal gas equation.

Q: What volume is occupied by a 1.38 mol sample of helium gas at a temperature of 0 °C and a pressure…

A:

Q: At 1.29 atm and 29.54∘C, a 3.14 g sample of gas occupies a volume of 1.70 ×103 mL. Calculate the…

A: Given, P= 1.29 atm  Mass = 3.14 g Volume = 1.70 ×103 mL T = 29.54∘C

Q: A gas occupies 1.40 L at 0.90 atm. What pressure would it exert if the volume were allowed to…

A: P1V1 = P2V2

Q: A flask with a total volume of 0.0300 L is found to contain 0.04120 g of an unknown gas when the…

A:

Q: Assuming that a 800 mg gas occupying a volume of 1,100 ml at a pressure of 1,600 mmHg and a…

A: Volume = 1100ml = 1.1L  Pressure = 1600 mmHg = 2.1052 atm  T = 75oC =  75 + 273K = 348K  Gas…

Q: A gas at 34C and 1.75 atm has a density of 3.4 g/L. Calculate the molar mass of the gas?

A: The ideal gas equation is given by,                               PV = nRT Where, P is the pressure…

Q: A 3.85 g sample of an unknown gas at 73 °C and 1.05 atm is stored in a 1.35 L flask. What is the…

A:

Q: A 1.05 g sample of an unknown gas at 61 "C and 1.05 atm is stored in a 2.55 L flask. What is the…

A: Mass per unit volume is known as density. S.I unit of density is g/cm3 or kg/m3. Other units of…

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…

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.