On a hot summer day, the density of air at atmospheric pressure at 34.5°C is 1.1866 kg/m³. (a) What is the number of moles contained in 1.00 m³ of an ideal gas at this temperature and pressure? mol (b) Avogadro's number of air molecules has a mass of 2.82 x 10-2 kg. What is the mass of 1.00 m³ of air? (Assume air is an ideal gas.) kg (c) Does the value calculated in part (b) agree with the stated density of air at this temperature? (Consider that it does if the values are within 10% of each other.) Yes O No

On a hot summer day, the density of air at atmospheric pressure at 35 °C is 1.1455 kg/m3.  What is the number of moles contained in 1 m3 of ideal gas at this temperature and pressure?  Avogadro’s number of air molecules has a mass of 2.85×10-2kg. what is the mass of 1 m3 of air? Does the value calculated in part (B) agree with the stated density of air at this temperature?

An industrial firm supplies compressed air cylinders of volume 0.25 m3 filled to a pressure of 20×106 Pa at 17 ºC. Calculate the number of moles of air in each cylinder.

Suppose the amount of air in a person's lungs is 1.75 L. Calculate the number of moles of air molecules in the person’s lungs when the pressure there is atmospheric pressure. Note that the air is at 37.0°C (body temperature).

You have a container of neon (Ne) gas at 290 K. The volume of the container is 0.1 m3 and the pressure is 2.1 atm. a) How many Ne atoms are in the container? b) How many moles of Ne are in the container?

On a chilly 10°C day, you quickly take a deep breath—all your lungs can hold, 4.0 L. The air warms to your body temperature of 37°C. If the air starts at a pressure of 1.0 atm, and you hold the volume of your lungs constant (a good approximation) and the number of molecules in your lungs stays constant aswell (also a good approximation), what is the increase in pressure inside your lungs?

(a) A rigid tank contains 1.50 moles of carbon dioxide, which can be treated as an ideal gas, at a pressure of 22.7 atm. While the tank and gas maintain a constant volume and temperature, a number of moles are removed from the tank, reducing the pressure to 5.10 atm. How many moles are removed? mol (b) What If? In a separate experiment beginning from the same initial conditions, including a temperature T, of 25.0°C, half the number of moles found in part (a) are withdrawn while the temperature is allowed to vary and the pressure undergoes the same change from 22.7 atm to 5.10 atm. What is the final temperature (in °C) of the gas? °C