At 23.0 °C and a pressure of 719 torr, a gas was found to have a density of 4.92 gL1. Calculate its molar mass. i g/mol

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: 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: What is the temperature, in Kelvins, of a 0.333-mol sample of a gas that has a pressure of 48.1 kPa…

A: The temperature is determined using the following equation P×V= n×R×T Where P is the pressure in…

Q: if the density of an ideal gas at STP is found to be 1.96 g/L, what is the molar mass?

A:

Q: What is the pressure, in kPa, of a gas sample with a pressure of 1127 mmHg?

A: Given information: Pressure of gas sample = 1127 mmHg

Q: Convert 747.6 mmhg to atm

A: 1 atm = 760 mm Hg  Thos conversion factor will be used to convert mm Hg to atm

Q: A sample of oxygen gas, which is saturated with water vapour, is kept in a 10 L vessel at 30° C and…

A: Given, Total pressure, (PO2 + PH2O) = 758 Torr Pressure of water vapor, (PH2O) = 31.8 Torr

Q: A 0.112 g sample of gas occupied 81.8 cm3 at temperature 127 °C and a pressure of 1 atm. Calculate…

A: The ideal gas equation, PV = nRT  and n = mass of the gas (m)/Molar mass of the gas (M) PV = (m/M)…

Q: At what altitude does the atmospheric pressure drop from 760 Torr to 560 Torr at 25°C? (Molecular…

A: Given, initial pressure =760 torrand final pressure =560 torrtemperature =25 °Cmolecular weight of…

Q: What is the volume occupied by 1.24 mol of a gas at 35oC if the pressure is 96.2 kPa? What is the…

A: This is given by equation of state for ideal gas i.e.  PV = nRT On combining all the gas laws a…

Q: What is the density of a gas with a molar mass of 163 g/mol at 25C and 1.00 atm?

A: Given information: Molar mass = 163 g/mol Temperature (T) = 25 °C Pressure (P) = 1.00 atm

Q: What is the mass, in grams, of 13.88 L of nitrogen gas (N2: 28.00 g/mol) at STP?

A: Introduction: The gases which follows Charle’s law, Boyle's law, Gay-Lussac’s law, and Avogadro’s…

Q: Consider a 1.53-L sample of gaseous SO2 at a pressure of 5.6 x 103Pa. If the pressure is changed to…

A: At constant temperature: P1V1 = P2V2 P1 = initial pressure; V1 = initial volume; P2 = final pressure…

Q: A 0.704-g sample of a colorless liquid was vaporized in an evacuated 250.-mL flask at 121°C to give…

A: Given information: Mass of sample = 0.704 g Pressure (p) = 786 mmHg Volume (V) = 250 mL Temperature…

Q: Gas Z was collected over water at 21°C on a day when atmospheric pressure was 757 torr. The volume…

A: The pressure in the collection tube is due to water vapor and the gas Z. Since, the total pressure…

Q: Calculate the molar mass of a gas that has a density of 1.70 g/L at STP

A:

Q: How many molecules are there in an ideal gas with a volume of 6.28 L at STP?

A: We have the ideal gas equation PV=nRT...................1 We know that, the ideal gas is at STP…

Q: What pressure in atmospheres corresponds to 720.3mm Hg?

A: We have to convert the unit of given pressure (720.3 mmHg) from mmHg to atmosphere.

Q: What is the mole fraction of O2 in a gas mixture with a total pressure of 750 torr when the partial…

A: Given,The total pressure = 750 torr,The partial pressure is 125 torr.

Q: A gas sample weighing 19.66 g occupies a volume of 7.85 L at STP. What is the molar mass of this gas…

A: The ideal gas equation is given as:

Q: One molecule of hemoglobin will combine with four molecules of oxygen.  If 1.00 g of hemoglobin…

A: Given that, Volume of oxygen=1.53 mL=0.00153L (since 1 L=1000mL) Temperature =370C=273.15+37=310.15K…

Q: What is the molar volume of Ne gas under the conditions of temperature and pressure where density is…

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Q: At 600. K how many moles of gas are in a 1.00 L cylinder at atmospheric pressure?

A: The moles of gas is determined by using the ideal gas equation PV = nRT.

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: The partial pressures of CH 4, N 2, and O 2 in a sample of gas were found to be 135 mmHg, 508 mmHg,…

A: Given : Partial pressure of CH4 = 135 mm Hg Partial pressure of N2 = 508 mm Hg And partial pressure…

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: For the given reaction, what volume of NO₂ can be produced from 0.80 L of O₂, assuming an excess of…

A:

Q: What is the density of sulfur dioxide gas at 795 torr and 25 oC?

A:

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

A:

Q: In a mixture of helium and chlorine, occupying a volume of 12.8 L at 605.6 mmHg and 21.6oC, it is…

A: Given information:Volume = 12.8 LPartial pressure of chlorine = 143 mmHgPressure = 605.6…

Q: 238.15L of gas at 841.5 torr and 85.1°C is heated until the temperature reaches 134.1°C.  and the…

A: According to the ideal gas law, the volume of a gas is directly proportional to the number of moles…

Q: Calculate the density of Xenon gas at a pressure of 742 mmHg and a temperature of 450C. The molar…

A:

Q: At 618 mm Hg, a sample of nitrogen gas occupies 490 mL.  What volume does the gas occupy if the…

A: We know Boyle's Law states that, "The absolute pressure(P) exerted by a given mass of an ideal gas…

Q: What is the mass of chlorine gas present in 17.0 L at a pressure of 98.5 kPa and a temperature of…

A: This problem will be solved using ideal gas equation which is given as PV= nRT  Where, P = pressure…

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 mixture contains sulfur hexaflouride at a pressure of 2.64 atms and diphosphorus pentoxide at…

A: given, A gas mixture contains sulfur hexafluoride at a pressure of 2.64 atm and diphosphorus…

Q: The density of a gas is 1.74 g/L at 31oC and 592 torr.  Calculate the molar mass of this gas. R =…

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Q: Calculate the partial pressures of carbon dioxide and argon when the total atmospheric pressure is…

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Q: A 14.36 mol sample of argon gas at 95.98 °C occupies 24.00 L. What is the pressure in kPa? Provide…

A:

Q: The mole fraction of Ar in a mixture of gases is 0.829 with a partial pressure of 0.341 atm. What is…

A: The partial pressure of an individual gas is equal to the total pressure multiplied by the mole…

Q: 62.0 g of nitrogen at 100oC is in a 155.0 L container. How much nitrogen, in grams, must be removed…

A: Answer is explained below.

Q: What is the mass (in g) of a 28.2 L sample of carbon dioxide gas at a temperature of 30.0 oC and a…

A:

Q: The molecular weight of a gas that has a density of 6.75 g/L at STP is __________ g/mol.

A: At stp pressure is one atm

Q: The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine…

A: Given, Volume of N2 at STP = 1580 LVolume of H2 at STP = 4240 LWe know that, at STP 1 mole of a gas…

Q: From data gathered by Voyager 1, scientists have estimatedthe composition of the atmosphere of…

A: Given information: Total pressure = 1220 torr Percent of nitrogen = 82% Percent of argon = 12%…

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: 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: The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine…

A: We have to calculate the volume of Reactant left.

Q: What is the molar volume of Xe gas under the conditions of temperature and pressure where its…

A: Let volume of gas = 1 L Mass of Xe = density * volume              =     6.7 g/L * 1 L…

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.