An ideal gas sample of 2 moles initially at STP is isobarically
expanded
to twice its original volume. What must be its final
temperature?
a. 546 K
b. 137 K
c. 0 K
d. 819 K
In the previous question, by what factor does the internal
energy of the
gas change?
An ideal gas sample of 2 moles initially at STP is isobarically expanded to twice its...
a. 242 m/s b. 1.21 x 103 m/s c. 822 m/s d. 483 m/s 25. Is this rms speed the same or different from the nitrogen molecules in the sample? Explain. 26. An ideal gas sample of 11 moles initially at STP is isothermally compressed to half its original volume. What must be its final pressure? a. 4.8 atm b. 3 atm c. 2 atm d. 4 atm 27. In the previous question, by what factor does the internal energy...
A sample of n moles of a monatomic ideal gas is expanded isothermally and reversibly at a constant temperature T from a volume V to 3V. Note that since the temperature of the gas is constant, the internal energy will remain constant. a) Write an expression for the change in entropy ΔS for the system. b) The sample has 7 moles of gas and is kept at a temperature of 305 K. The volume is changed from 0.065 m3 to...
Two moles of an ideal gas initially has a temperature of 400 K and a volume of 40 Liters. The gas undergoes a free adiabatic expansion to twice its initial volume. a.) What is the entropy change of the gas? b.) What is the entropy change of the universe? explain please
6. (25 points) One mole of a monatomic ideal gas, initially at pressure P1 = 105 Pa and temperature T1 = 273 K undergoes an isovolumetric process in which its pressure falls to half its initial value. a) What is the work done by the gas? What is the final temperature? b) The gas then expands isobarically (constant pressure) to twice its initial volume. What is the work done by the gas? What is the final temperature? c) Draw a...
A piston reversibly and adiabatically contracts 3.88 moles of ideal gas to one-tenth of its original volume, then expands back to the original conditions. It does this a total of five times. If the initial and final temperature of the gas is 27.5 degree C, calculate (a) the total work and (b) the total change in internal energy for the overall process.
2. 0.5 moles of an ideal gas is initially at T, = 300 K in a volume Va=0.8 L. This gas has a y value of 9/7. It is taken around the cycle as shown: (1) expanded isothermally to volume Vo = 1.6 L, from a to b. (2) expanded adiabatically to T. = 275 K, from b to c. 0.8L (3) compressed at constant pressure to T, = 235.74 K, from c to d. (4) compressed adiabatically back to...
A flexible balloon contains 0.350 mol of an unknown polyatomic gas. Initially the balloon containing the gas has a volume of 6900 cm3 and a temperature of 30.0 ∘C. The gas first expands isobarically until the volume doubles. Then it expands adiabatically until the temperature returns to its initial value. Assume that the gas may be treated as an ideal gas with Cp=33.26J/mol⋅K and γ=4/3. What is the total heat Q supplied to the gas in the process? What is...
An ideal gas initially at 295 K undergoes an isobaric expansion at 2.50 kPa. The volume increases from 1.00 m^3 to 3.00 m^3 and 11.4 kJ is transferred to the gas by heat. What is the change in internal energy of the gas? kJ What is the final temperature of the gas? K At high noon, the Sun delivers 825 W to each square meter of a blacktop road. If the hot asphalt loses energy only by radiation, what is...
A 1.00 mole sample of an ideal monatomic gas, originally at a pressure of 1.00 atm, undergoes, undergoes a three-step process. (1) It is expanded adiabatically from T1 = 550 K, to T2 = 389 K; (2) it is compressed at constant pressure until the temperature reaches T3; (3) it then returns to its original temperature and pressure by a constant volume process. (a) Plot these processes on a PV diagram. (b) Determine T3. (c) Calculate the change in internal energy, the...
An ideal gas initially at 270 K undergoes an isobaric expansion at 2.50 kPa. The volume increases from 1.00 m3 to 3.00 m3 and 14.4 kJ is transferred to the gas by heat. (a) What is the change in internal energy of the gas? kJ (b) What is the final temperature of the gas? K