College Physics
11th Edition
ISBN: 9781305952300
Author: Raymond A. Serway, Chris Vuille
Publisher: Cengage Learning
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- A canister with a piston contains 1.05 kg of air at 30.0°C and 1.25 x 105 Pa. Energy is transferred by heat into the system as it expands and the pressure rises to 4.25 x 105 Pa. Throughout the expansion, the relationship between pressure and volume is given by P = cv1/2) where C is a constant. Air may be modeled as a diatomic ideal gas with a molar mass of M = 28.9 g/mol. Determine the following. (a) initial volume (in m3) 0.01477 The ideal gas law may be used to describe the air in any state, Since we want the initial volume, we should use the pressure and temperature for the initial state. How can you determine the number of moles of air from the total mass and the molar mass? m3 (b) final volume (in m) m3 (c) final temperature (in K) K (d) work done on the air (in J) (e) energy transferred by heat (Enter the magnitude in MJ.) MJarrow_forwardAn ideal gas is heated at a constant pressure of 1.80 x 10 Pa from a temperature of -73.0°C to a temperature of +27.0°C. The initial volume of the gas is 0.100 m³. The heat energy supplied to the gas in this process is 40.0 kJ. What is the increase in internal energy of the gas? -8.95:kJarrow_forwardDuring a long sleepless night, you wonder about the thermodynamic properties of the air in your room. If your room has a volume of 24 m3, the pressure is 9.9x 104 Pa and the temperature is 20°C, what is the total translational kinetic energy of the air molecules in your room?arrow_forward
- At 100°C the rms speed of nitrogen molecules is 576 m/s. Nitrogen at 100° C and a pressure of 2.5 atm is held in a container with a 10 cm x 10 cm square wall. Estimate the rate of molecular collisions (collisions/s) on this wall. Express your answer in collisions per second. ► View Available Hint(s) the rate of collisions = Submit VG ΑΣΦ ? collisions Sarrow_forwardAn ideal gas consists of 2.50 mol of diatomic molecules that rotate but do not oscillate. The molecular diameter is 118 pm. The gas is expanded at a constant pressure of 1.79 x 105 Pa, with a transfer of 150 J as heat. What is the change in the mean free path of the molecules?arrow_forwardThe mean free path is the average distance traveled by a particle between collisions with other particles. Calculate the mean free path of air at room temperature, T = 67.0 °F. Air is mostly nitrogen, so assume that the collisions are between moving N₂ molecules. The diameter of N₂ is d = 1.87 × 10−¹0 m and the gas is at atmospheric pressure, P = 101325 Pa. λ = marrow_forward
- 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?arrow_forwardA cylinder of cross sectional area 0.0287 m^2 is filled with an ideal monoatomic gas. A mass of 47.4 kg is placed on top of the piston which is free to move without friction. The piston starts 0.61m above the base of the cylinder. The gas in the piston is initially at a temperature of 454.0 K and the pressure in the lab is 100kPa.How many moles of gas are in the cylinder?arrow_forwardConsider a monatomic gas whose molecules have an average kinetic energy of 30.0 eV. What is the temperature of the gas?The temperature of the gas isarrow_forward
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