One mole of an ideal gas is held at a constant pressure of 1 atm. Find the change in volume (in liters) if the temperature changes by 25°C.

The volume of an automobile tire is 2.5 × 10−2m3 . the pressure of the air in the tire is  3 atm and the temperature is 37C ◦ . what is is the mass of air in grams ? The mean molecular mass of air is 29g.                                     1 atm = 1.01  × 105 Pa ;    Calculate to 2 decimals.

A mole of gas has isobaric expansion coefficient dV/dT = R/p and isochoric pressure-temperature coefficient dp/dT = p/T . Find the equation of state of the gas.

(a) 0.3740 moles of krypton gas is placed in a 9.75 L container at 239 K. Find the pressure of the gas in bar? (b) What is the average kinetic energy per mole of krypton gas atoms featured in the previous part? Report your answer in J/mol.

A basketball is pressurized to a gauge pressure of PG = 55 kPa when at the surface of a swimming pool. (Patm = 101 kPa). The ball is then submerged in the pool of water which has a density ρ = 1000 kg/m3. Assume the ball does not change in mass, temperature, or volume as it is submerged. Calculate the absolute pressure inside the basketball in kPa when it is at the surface.  Write an equation for the pressure difference ΔP between the inside and outside of the ball when it is submerged a distance y below the surface of the water.  Solve the pressure equation for the depth (in meters) at which the pressure difference between the inside and outside of the ball will become zero. At this depth the pressure inside the basketball is the same as the pressure outside the ball.

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A bubble of air is rising from the sea floor, from a depth of about 500 m. At this depth the pressure is 5.1*106 Pa (about 50.3 atm) and is at a temperature of about 7.0° C. It rises to the surface with the atmosphere, at a temperature of 20° C. If the bubble is observed to have a volume of 4 cm³ at the surface, what was its volume at the sea floor? Assume the number of moles of gas in the bubble is constant. B.

A 10.0 L container contains a certain gas at a temperature of 25.0◦C and pressure of 9.50 atm. Calculate the number of moles of gas in the container.

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.

A sealed 19 m3 tank is filled with 7,011 moles of ideal oxygen gas (diatomic) at an initial temperature of 292 K The gas is heated to a final temperature of 490 K. The atomic mass of oxygen is 16.0 g/mol. The final pressure of the gas, in MPa, is closest to: answer round to 4 sig.fig