with an ideal gas (Cv = 2.5R) at 501K and 1.1 bar. Calculate the entropy changes asked in below. When an axial mixer is installed in
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. A rigid container (0.066 m3) is filled with an ideal gas (Cv = 2.5R) at 501K and 1.1 bar. Calculate the entropy changes asked in below. When an axial mixer is installed in a container and 15,000 J of work is applied to the gas under the insulation process, what is the entropy change of the gas?
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- In this question, we derive the entropy of an Ideal Gas. a) By considering a constant volume process, show that the First Law, dE dQ dW can be written as nCydT=dQ – dW. dV b) Using the Ideal Gas Law, show that this expression can be written as nCv dT dQ - nRT V. c) By dividing by T, and defining d.S of dQ T Tf AS = ff d = nCv In +nRln Ti = dQ as usual, show that the change in entropy, AS, can be written as:A 2.00-mol sample of H2 gas is contained in the left side of the container shown below, which has equal volumes on the left and right. The right side is evacuated. When the valve is opened, the gas streams into the right side. (a) What is the entropy change of the gas? (b) Does the temperature of the gas change? Assume the container is so large that the hydrogen behaves as an ideal gas. (Wouldn't the temperature decrease because the temperature in a vacuum would be really cold?)We trapped 28 kg of dry air, and it initially has standard pressure and temperature. The trapped air parcel rises in the atmosphere until the temperature is 188 K. What is the change in entropy if the pressure decreases by 28% after the parcel rises?
- One mole of an ideal gas is used as the working substance of an engine operating in the cycle shown in the figure below. BC and DA processes are reversible adiabatic.a) Is the gas monoatomic, diatomic or triatomic?b) What is the efficiency and engine?Suppose a heat engine design makes a square on a PV diagram, using a monatomic gas. The high pressure is 3P and low pressure is P. The high volume is 3V and low volume is V. What is the efficiency of the heat engine?A box contains 100 gas molecules all released on the left side of the box. What is the initial entropy of all the gas molecules on one side? You can calculate the number of microstates (left/right distribution of molecules) possible by the equation W = N! / ( nL! * nR!,) where N is the total number of molecules and nL is the number on the left and nR is the number on the right. What is the entropy of the most disorganized distribution of gas molecules?