a 5.16 L quality of a gas measured at STP has a mass of 37.3 g. what is the molar mass of the compound?

Q: An 0.642 mol sample of nitrogen gas at a temperature of 19.0°C is found to occupy a volume of 27.5…

A: so in this we use PV=nRT V=27.5 l T=19+273=292 K n=0.642 mol P= nRT/V     = 0.642*(0.0821 L atm…

Q: 6. What is the density of Xe gas at STP?

A:

Q: If 10.0 L of a gas at STP has a mass of 19.5 g, calculate the molar mass of the gas

A:

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: Which of the following gases does not occupy a volume of 1.00 L at STP? a) 0.18 g He. b) 2.69x1022…

A:

Q: determine the volume (in mL) of 0.500 g of fluorine gas at STP.

A: Given :- mass of F2 gas = 0.500 g  To calculate :- volume of gas in mL (at STP)    At STP , 1 mol…

Q: 4 447.9 780.7 115.5 71700 703 669 5 cm3 10 cm3 20 cm³ 09.1 726.0 411.1 796 822 20 cm3 10 cm3 5 cm3…

A: Boyle's law confirm this experiment .  At constant temperature the pressure of gas is inversely…

Q: A gas sample at STP contains 1.47 g oxygen and 1.66 g nitrogen. What is the volume of the gas…

A: We are given the mass of two gases , we have to find the volume at STP

Q: A mixture of oxygen and carbon dioxide gases contains oxygen at a partial pressure of 583 mm Hg and…

A: The mole fraction of oxygen and carbon dioxide is calculated as,

Q: What is the molar mass of a gas if 18.0 L of the gas at STP has a mass of 41.6 grams?

A:

Q: If the mole fraction of He in a gas mixture is 0.597 and the total pressure of the gas is 843 mmHg.…

A: According to Dalton's law of partial pressure,In a mixture of non reacting gases the total pressure…

Q: A sample of gas at 29.8ºC has a volume of 6.4 L and exerts a pressure of 762 mm Hg. How many moles…

A:

Q: If 1.36 g of a gas occupies a volume of 1.00 L at 0.984 atm and 30 C, what is the molar mass in…

A: From ideal gas law, we know that  PV = nRT Where  P = pressure of the gas V = volume of gas n =…

Q: A balloon contains 50.0 L of CO2 at STP. What will be the mass of the gas inside the balloon?

A: At standard temperature and pressure,  T = 0 degree C = 273.15 K P = 1 atm V = 50.0 L (volume of…

Q: What volume of O2(g) iş consumed in the combustion of 75.6 L C3H8 (g) if both gases are measured at…

A: In the combustion reaction propane (C3H8) reacts with oxygen to form carbon dioxide and water. The…

Q: If a gas mixture of O2 and N2 has a total pressure of 750 torr and the partial pressure of nitrogen…

A: Dalton's Law of partial pressures states that total pressure is equal to the sum of partial…

Q: What is the density of Xe gas at STP?

A: The ideal gas equation is, PV=nRT ..........(1) where P is pressure, V is volume, n is count of…

Q: A 25.00 g sample of a pure gas fills a 5.6 L balloon at SATP. Calculate the molar mass of this gas

A:

Q: 4. At temperature 500 °C, what is the volume of occupied 4.2 grams carbon dioxide gas at STP?

A: Number of moles is calculated by dividing given mass with molecular mass.

Q: A sample of gas at 33.9ºC has a volume of 10.3 L and exerts a pressure of 782 mm Hg. How many moles…

A: To solve this problem, we need the universal gas equation which is given as follows: PV=nRT Here, P…

Q: What volume does 4.0 moles of a gas occupy at STP?

A: Mole concept is to be applied. As per mole concept 22.4 L of a gas at S.T.P is occupied by 1 mole of…

Q: If the density of an ideal gas at STP is found to be 2.86 g/L,2.86 g/L, what is its molar mass?

A:

Q: Define molar volume and lists its value for a gas at STP.

A: STP represents the standard condition of temperature and pressure.

Q: At STP, 4.510 liters of a gas has a mass of 3.231 g. Calculate the molar mass of the gas.

A:

Q: How many He atoms are in 49.5 L of He gas at STP?

A: Given, volume of He = 49.5 L

Q: 24. At STP, 4.510 liters of a gas has a mass of 3.231 g. Calculate the molar mass of the gas.

A: Given volume of gas = 4.510 L  Mass of gas = 3.231 g

Q: Define molar volume and give its value for a gas at STP.

A: At STP(standard temperature and pressure), the molar volume refers to the volume occupied by one…

Q: If a gas sample weighed 3.97 grams occupies 2.768 liters at STP what would be the molas mass of this…

A: Calculation for number of moles:At STP, 1 mole of any gas occupies 22.4 Litre of Volume

Q: The mass of 1.12 L gas at STP is found to be 6.23 g. What is the molar mass of gas Y ?

A: Given data is: Volume of gas = 1.12 L  Given mass = 6.23 g The procedure to finding the molar mass…

Q: The volume of a gas at STP is 488. mL, Calculate its volume at 22.5 atm and 323 K.

A:

Q: What volume of carbon dioxide is produced at STP when 255.45 g propane is reacted with 650.0 L…

A:

Q: A gas sample at STP contains 4.28 g of ammonia gas, NH3. What is the volume of the ammonia gas

A: The question is based on the concept of ideal gas equation. We have to calculate volume of the gas…

Q: At STP, 0.284 L of a gas weighs 0.401 g. Calculate the molar mass of the gas.

A: Ideal gas equation is,

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.