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College Physics
11th Edition
ISBN: 9781305952300
Author: Raymond A. Serway, Chris Vuille
Publisher: Cengage Learning
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An ideal gas at 20∘C consists of 2.2×1022 atoms. 1.4 J of thermal energy are removed from the gas.What is the new temperature in ∘C?
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- An 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_forwardA monoatomic gas is at a temperature of 325K. What is the internal energy of one atom of the gas?arrow_forwardThree moles of an ideal gas at 135C and 0.5 atm is allowed to expand 1 atm at a constant pressure to a volume twice as large. What is the new temperature?arrow_forward
- An ideal gas with y = 1.67 is initially at 2°C in a volume of 8 L at a pressure of 1.00 atm. It is then expanded adiabatically to a volume of 8.5 L. What is the final temperature of the gas? -20°C -23°C 2.5°C -8.9°C 68°Carrow_forwardProblem #1: An ideal gas of initial volume V=1m^3, initial temperature T=1000C and initial pressure P=10,000 Pa is heated up to a final temperature T=3000C and allowed to expand into a final volume V=3m^3. What is the final pressure?arrow_forwardTwo ideal gases have the same mass density and the same absolute pressure. One of the gases is helium (He), and its temperature is 131 K. The other gas is neon (Ne). What is the temperature of the neon?arrow_forward
- A 0.75 m3 container of an ideal gas at atmospheric pressure is at a temperature of 40 oC and contains heat energy Q. The gas is heated so it now contains heat energy 1.75Q. The temperature of the gas is nowarrow_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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