5. i) Using the ideal gas law, find the number of air molecules per unit volume in air at 25 ◦ C and atmospheric pressure.
ii) Assuming air to be 80 % N2 and 20 % O2, show that the average molecular weight of dry air is around 28.8 grams per mol.
iii) Combine this with the result from part i) to calculate the density of dry air at 25 ◦ C.
5. i) Using the ideal gas law, find the number of air molecules per unit volume...
Use the ideal gas law to calculate the volume occupied by 1.00 mol of ideal gas at 1.00 atm pressure and 10.0°C. Given that the average molecular weight of air is 28.9 g/mol, calculate the mass density of air, in kg/m3at the above conditions.
A hot air balloon has a volume of 2000 m3 when fully inflated and the air inside the balloon is at atmospheric pressure (101,000 Pa). What is the mass of hot air inside the balloon if its temperature is 120°C? (Assume a molecular weight of 28.8 g/mole for air, which is about 80% N2 and 20% O2.)
The Ideal Gas Law 4 of 8 Review | Constants I Periodic Table The ideal gas law describes thee relationship among the pressure P. volume V. number of moles n and absolute temperature T'of an ideal gas Here is the relationship expressed mathematicaly Part A PV-nRT How many air molecules are in a 14.0 x 12.0 x 10.0 ft room (28.2 L 200 C and ideal behavior 1 ft? Assume atmospheric pressure of 1.00 atm a room temperature of where...
According to the ideal gas law, a 0.9054 mol sample of krypton gas in a 1.023 L container at 274.0 K should exert a pressure of 19.90 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. % According to the ideal gas law, a 9.344 mol sample of oxygen gas in a 0.8267 L container at 500.1...
The density of nitrogen gas (N2) at standard temperature and pressure (STP, 0°C and about 1atm) is 1.25 kg/m3, while the density of liquid nitrogen at atmospheric pressure is 0.81 x 103kg/m3. Let D denote a typical distance between nitrogen molecules in its gas (i) Assuming that the nitrogen atoms in the liquid are basically touching each other, esti- ii) Using the ideal gas equation of state determine the volume of 1 mole of gas at STP. phase and d...
The ideal gas law describes the relationship among the volume of an ideal gas (V), its pressure (P), its absolute temperature (T), and number of moles (n): PV=nRT Under standard conditions, the ideal gas law does a good job of approximating these properties for any gas. However, the ideal gas law does not account for all the properties of real gases such as intermolecular attraction and molecular volume, which become more pronounced at low temperatures and high pressures. The van...
9. Pressure at Mt. Everest If we rearrange the ideal gas law to be in terms of density: pR and also consider the affects of the buoyancy force: apE, we can combine these equations to find the atmospheric pressure as a function of height above the ground. Do so to find the air pressure at an elevation of 8838 meters, close to the peak of Mt. Everest. You can assume that g is constant all the way up and so...
At what pressure, in atmospheres, would the number of molecules per unit volume in an ideal gas be equal to the number density of the conduction electrons in copper, with both gas and copper at temperature T = 400 K?
Air a. What is the volume of air in the room where you are right now? (You can measure the length, width, and height of the room with a measuring tape, or you can estimate these quantities. Just make sure you convert your answer to SI units.) b. What is the temperature in this room? (in SI units) c. Look up the current barometric pressure in your area, and convert it to SI units. d. Use the information from steps...
Empirical Gas Laws, Ideal Gas Law, Dalton's Law of Partial Pressures 3. A Mexible vessel is filled to a certain pressure with 12.00 L of gas. Under conditions of constant temperature and moles of gas, how does the volume of the gas change when the pressure of the gas is decreased by a factor of three? 4. A gas occupies a volume of 2.75 L at 350. mmHg and 200°C. What is the volume of the gas at 550. mmHg...