1) A 3.00-mol sample of an ideal diatomic gas in which the gas particles both translate and rotate is initially at 600 K. Energy is then added thermally to the sample until its temperature is 1000 K. Assume that at the temperatures higher than 1000 K, the particles also vibrate, at the temperatures lower than 1000 K, the particles do not vibrate. The sample is then heated to 1200 K.
Part A:- How much thermal energy does the sample absorb? Express your answer with the appropriate units.
1) A 3.00-mol sample of an ideal diatomic gas in which the gas particles both translate...
Consider 2.32 moles of an ideal diatomic gas at 25.0°C. (a) What is the total heat capacity of the gas if the molecules do not vibrate? at constant volume J/K at constant pressure J/K (b) What is the total heat capacity of the gas if the molecules do not translate or rotate, but do vibrate about their molecular axes? at constant volume J/K at constant pressure
A 2.00 mol sample of a diatomic ideal gas expands slowly and adiabatically from a pressure of 5.04 atm and a volume of L2 Lto a final volume of 30.8 L (a) What is the final pressure of the gas? 1.44 atm (b) What are the initial and final temperatures? initial 385.72 final 269.39 (c) Find Qfor the gas during this process. 0 (d) Find ??¡nt for the gas during this process. What is the relationship between the internal energy...
A diatomic ideal gas expands from a volume of VA-1.00 mºto V, - 3.00 m along the path shown in the figure below. The initial pressure is PA-2.00 x 10 Pa and there are 67.3 mol of gas. P(10%Pa) 4.00 8.00 2.00 1.00 1.00 2.00 3.00 100V (m) (a) Calculate the work done on the gas during this process. (b) Calculate the change in temperature of the gas. (c) Calculate the change in internal energy of the gas. (Take the...
Which is the least true statement for the Ideal Gas Law A. particles can be diatomic B. The system is in equilibrium C. It works best at lower temperatures D. The temperature must be in Kelvin or Celsius
0.06 mol of an ideal diatomic gas held in the apparatus shown to the right is initially uninsulated, at room temperature (290K), and atmospheric pressure. The piston has an initial height of 20cm. i. Masses are slowly added and exert an average force of 1000N as the piston travels a total distance of 10cm. ii. Fixing the pin, a flame is applied to the cylinder. iii. Once the thermal energy of the gas has increased by 593J, the flame is...
The temperature of 5.58 mol of an ideal diatomic gas is increased by 31.1 ˚C without the pressure of the gas changing. The molecules in the gas rotate but do not oscillate. (a) How much energy is transferred to the gas as heat? (b) What is the change in the internal energy of the gas? (c) How much work is done by the gas? (d) By how much does the rotational kinetic energy of the gas increase?
a 2 mol sample of diatomic ideal gas is expaning slowly and adiabatically from a pressure eof 5.05 ATM and a volume if 13 literally to a final volume of 29.4 liters. what is the pressure? what is the initial and final temperatures? what is q for gas during this process? what is the change in E int of the gas drluring the process? what is the W on the gas during the process
A 0.450-mol sample of an ideal diatomic gas at 372 kPa and 312 K expands quasi-statically until the pressure decreases to 147 kPa. Find the final temperature and volume of the gas, the work done by the gas, and the heat absorbed by the gas if the expansion is the following. (a) Isothermal final temperature _______ volume of the gas _______ work done by the gas _______ heat absorbed _______ (b) adiabatic final temperature _______ volume of the gas _______ work done by the gas _______ heat absorbed _______
k How much thermal energy must be added to 7:10 moles of a diatomic ideal gas to raise its temperature 22.1 K? A) 32603 B) 1960) C) 6523 D) 4570
6. (10 marks) A sample of 3.00 mol of ideal gas with Cv,m = 2.5R undergoes the change of states shown in the following P-T diagram (a + b → → a). Calculate the amount of expansion work (w) involved in each segment. P (atm) irreversible 1.50 reversible irreversible 1.001 - 400 600 T(K)