4. The kinetic theory of gases predicts that, at a given temperature, a) All of the molecules in a gas have the same average speed. b) All of the molecules in a gas have the same average energy. 1 c) Light gas molecules have lower average energies than heavy gas molecules. d) Light gas molecules have higher average energies than heavy gas molecules. 5. According to the first law of thermodynamics, if the gas compressed adiabatically its temperature will: a) Increase. b) Decrease. c) Not change. d) None of the above. The boundary work W, for an isochoric process is: a) Positive. b) Negative. c) Zero. d) None of the above.

4. The kinetic theory of gases predicts that, at a given temperature, a) All of the molecules in a gas have the same average speed. b) All of the molecules in a gas have the same average energy. 1 c) Light gas molecules have lower average energies than heavy gas molecules. d) Light gas molecules have higher average energies than heavy gas molecules. 5. According to the first law of thermodynamics, if the gas compressed adiabatically its temperature will: a) Increase. b) Decrease. c) Not change. d) None of the above. The boundary work W, for an isochoric process is: a) Positive. b) Negative. c) Zero. d) None of the above.

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

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20. The kinetic molecular model of an ideal gas shows that * 1 average translational kinetic energy of a molecule is inversely proportional to the absolute temperature average translational kinetic energy of a molecule is directly proportional to the absolute temperature average translational kinetic energy of a molecule is not dependent to the absolute temperature average translational kinetic energy of a molecule is equal to the absolute temperature 21. The first law of thermodynamics helps us understand the relationships 11 among which three quantities? Heat, work, and internal energy O Heat, work, and external energy O Heat, work, and entropy O Heat, work, and enthalpy
QUESTION 16 Which of the following statements is not true according to kinetic theory? a. Electrical attractions and repulsions between the molecules must be accounted for in the total energy of the ideal gas. b. The energy of an ideal gas only depends on the kinetic energy of the gas. C. The average energy of a molecule in an ideal gas is evenly distributed between the different degrees of freedom of the molecule. d. The molecules in an ideal gas undergo elastic collisions. e. The molecules in an ideal gas only interact during collisions.
Learning Goal: To understand the ideal gas law and be able to apply it to a wide variety of situations. The absolute temperature T, volume V, and pressure p of a gas sample are related by the ideal gas law, which states that PV = nRT Here n is the number of moles in the gas sample and R is a gas constant that applies to all gases. This empirical law describes gases well only if they are sufficiently dilute and at a sufficiently high temperature that they are not on the verge of condensing. In applying the ideal gas law, p must be the absolute pressure, measured with respect to vacuum and not with respect to atmospheric pressure, and I must be the absolute temperature, measured in kelvins (that is, with respect to absolute zero, defined throughout this tutorial as -273°C). If p is in pascals and V is in cubic meters, use R = 8.3145 J/(mol · K). If p is in atmospheres and V is in liters, use R = 0.08206 L atm/(mol-K) instead. Part A A gas sample enclosed in a rigid metal container at…
6. According to the first law of thermodynamics, applied to a gas, the increase in the internal energy during any process: A. equals the heat input minus the work done on the gas 1 B. equals the heat input plus the work done on the gas C. equals the work done on the gas minus the heat input D. is independent of the heat input E. is independent of the work done on the gas
2. How do you define Zeroth Law of Thermodynamics?
5. An ideal gas is confined to a container with adjustable volume.The number of moles and temperature are constant.By what factor will the volume change if pressure doubles
7. Containers A and B in the figure to the right hold the same gas. The volume of B is four times the volume of A. The two containers are connected by a thin tube (negligible volume) and a valve that is closed. The gas in A is at 300 K and pressure of 1.0 × 10³ Pa. The gas in B is at 400 K and pressure of 5.0 × 105 Pa. Heaters will maintain the temperatures of A and B even after the valve is opened A 300 K Valve B 400 K a) After the valve is opened, gas will flow one way or the other until A and B have equal pressure. What is the final pressure? b) Is this a reversible or an irreversible process? Explain..
1. Two monoatomic ideal gases A and B are at the same temperature. If 2 g of gas A has the same internal energy as 0.2 g of gas B. (a) Calculate the ratio of the number of moles of each gas. nA nв (b) Calculate the ratio of the atomic masses of the two gases. MA MB =
D. 0.2971_kg/mol B. 0.3026_kg/mol 0.0834 kg/mol E. 0.09617 kg/mol C. F. 0.1538_kg/mol 1--1 What is the average kinetic energy of a molecule of oxygen gas (0₂) at a temperature of -25°C? 8 O 16.00 3. 5.061E-21 J D. 6.398E-21 J 5.041E-21 J 5.137E-21 J E. 4.368E-21 J F. 5.862E-21 J [carpet-5] A. B. C. 1--1
6 The diagram below depicts an ideal monatomic gas which is compressed isobarically at p = 1.05×10° Pa from state A (V₁ = 7.49×10 -3 m³) to state B (V₂ = 3.33×10 m³) where its temperature becomes T 3 B = 336°C. Its pressure is then increased at constant volume from state B to C and finally expanded isothermally until it returns to its initial state A. How much work is done by the gas and what is its temperature when it expanded during the isothermal process? с Pc B -A PA PB VB = VC VA The temperature of the gas during the isothermal process is 1370°C and the work done by the gas is 4105 kJ. The temperature of the gas during the isothermal process is 755.7 K and the work done by the gas is 2264 kJ. The temperature of the gas during the isothermal process is 1097°C and the work done by the gas is 6.375 kJ. The temperature of the gas during the isothermal process is 482.6 K and the work done by the gas is 2.834 kJ.
A piston is resting halfway into a cylinder containing gas in thermal equilibrium. The layer of molecules next to the closed end of the cylinder is suddenly flash-heated to a very high temperature. Which best describes what happens next? a. The high temperature molecules push out the piston until their energy is reduced enough that the system is in equilibrium. b. The molecules with the highest temperature bounce off their neighbors, losing energy to them, and so on until the system is at a new equilibrium with the piston moved out. c. The molecules with the highest temperature bounce offb their neighbors, losing energy to them, and so on until the system is at a new equilibrium with the piston where it started. d. The high temperature molecules push out the piston until their energy is reduced enough that the system is in equilibrium, and then the piston gets sucked back in.
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