• How does gas becomes ideal gas? • How does the work done in the following processes; a. Isobaric b. Isentropic c. Isothermal
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- 4) A ground source heat pump heats a building by extracting heat from the ground and pumping it into the building. Define: Qc = heat extracted from the ground, Qn= heat pumped into the building, W = electric energy used by the heat pump, Tc= temperature of the ground, T = temperature of building (Qc, Qn, and W are positive by definition). Assume Tr > Tc. a) Draw a diagram showing energy flow in and out of the heat pump. b) Write a general expression for the change AS in the entropy of the "universe", that is the heat pump plus the cold and hot reservoirs, in terms of the quantities defined above. Now assume ideal (reversible) operation, and take Te= 10 °C and Tp= 20 °C. What is the coefficient of performance (ČOP) of the heat pump? By what factor would this change if we had Tc = 0 °C instead?#10 As the temperature of a substance approaches absolute zero, the random motion of the molecules a decreases b increases c remains the sameA gas expands from 2.2 L to 3.6 L against a constant external pressure of 1.6 atm. What is the work done? A. -227 J B. 227 J C. 2.24 J D. -2.24 J
- > The following gives the calorimetric values for water at various phases: . Latent heat of fusion for water: 3.33 E5 J/kg • Specific heat capacity for ice: 2,220 J/kg"C • Specific heat capacity for liquid water: 4,186 J/kg C A 15-g sample of ice at -20.0 °C is converted to liquid water at 15.0 °C. Using the values from the table above, calculate the heat required for that conversion O 4,500 J O 6,600 J O 7,800 J O 9,500 J5) A mole of diatomic oxygen molecules and a mole of diatomic nitrogen molecules are at STP. Which statements are true about these molecules? (There could be more than one correct choice.) A) Both gases have the same average momentum per molecule. B) Both gases have the same average molecular speeds. C) Both gases have the same average kinetic energy per molecule. D) Both gases have the same number of molecules.An ideal gas is heated from 25.0°C to 335°C under a constant pressure of 2.81 kPa. i. If its initial volumeis 1.45m?, what is its final volume? ii. If the change in internal energy is 5.84kJ, how much heat is added to the gas? Assume any kinetic and potential energies are negligible. ii. What type of a process is this? Given: • Energy balance on a closed system at steady state AU + AE + AE, = Q – W, where U stands for internal energy, E for kinetic energy, E, for potential energy, Q for heat flow and W for work done by the system. PV = nRT, R = 8.314 = 8.314: T(K) = T(°C) + 273.15; 1N = 1 m: 1 Pa = 1. m³Pa mol K mol K %3D Constant P: W = P(V; - V.); Constant T: W = NRTIN