a) Find the difference of molar-specific heats C₂-C₁, for the gas covered by the equation of state: (P+) (V - b) = RT
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- The molar specific heat at constant pressure of an ideal gas is (7/2)R. The ratio of specific heat at constant pressure to that at constant volume is (a) 7/5 (b) 8/7 (c) 5/7 (d) 9/7If one mole of a monoatomic gas of (y = 5/3) is mixed with one mole of diatomic gas, then the (y = 715) value of y for the mixture will be, (a) 1.5 (b) 1.54 (c) 1.4 (d) 1.45The molar heat capacities at constant volume of Ne and N2 at 298 K are 12.47 J mol-1 K1 and 20.79 J mol-1 K-1 respectively. Give an explanation of these values based on statistical mechanics.
- The temperature at state A is 20.0ºC, that is 293 K. During the last test, you have found the temperature at state D is 73.0 K and n = 164 moles for this monatomic ideal gas. What is the change in thermal energy for process D to B, in MJ (MegaJoules)?Q.44 A gas is enclosed in a cylinder of volume Vo fitted with piston of cross-sectional area A and mass m. Atmospheric pressure is Po. Adiabatic exponent of gas is y. The piston is slightly depressed and released. (A) Time period of oscillation of piston if the process is isothermal is 2π (B) Time period of oscillation of piston if the process is adiabatic is 2π (C) Time period of oscillation of piston if the process is isothermal is 2π (D) Time period of oscillation of piston if the process is adiabatic is 2π mVo VA²Po ymVo A²Po mVo AP mVo √ YA²Po PoIf we know that the internal energy of the monoatomic ideal gas remains constant during the process in B to C, what must be the pressure Pc at point C in terms of the original pressure P0.
- A good explanation would be really helpfulYou would like to raise the temperature of an ideal gas from 295 K to 960 K in an adiabatic process. a)What compression ratio will do the job for a monatomic gas? b)What compression ratio will do the job for a diatomic gas?A flexible box contains 5.60 grams of nitrogen gas (N2) which is maintained at a constant pressure of 1.35 x 10$ Pa. The box is placed over a fire, causing the volume to increase from 0.00200 m3 to 0.00300 m³. Find the increase in temperature of the gas. (For N2 molar mass M = 28 grams.)