Consider a closed, isolated system that consists of two substances 1 and 2 that both have constant volume and have constant volume heat capacities over the relevant temperature range: Cv1 = 1J/K and Cy2 = 2J/K. Substance 1 is initially prepared at T1,0 100K, while substance 2 is initially prepared at T2,0 200K. Suppose instead that we want to cool substance 1 from T, . 100K to Tf = 90K.
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Why is this process impossible for a closed, isolated system?
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- Define isobaric,isochoric, isenthalpic,and isothermal. Can achangein a gaseous system be isobaric, isochoric,and isothermal at the same time? Why or why not?One mole of a monatomic ideal gas begins in a state withP 5 1.00 atm and T 5 300 K. It is expanded reversiblyand adiabatically until the volume has doubled; then it isexpanded irreversibly and isothermally into a vacuumuntil the volume has doubled again; and then it is heatedreversibly at constant volume to 400 K. Finally, it is compressed reversibly and isothermally until a inal state withP 5 1.00 atm and T 5 400 K is reached. Calculate DSsysfor this process. (Hint: There are two ways to solve thisproblem—an easy way and a hard way.)In a certain ideal heat engine, 10.00 kJ of heat is withdrawn from the hot source at 273 K and 3.00 kJ of work is generated. What is the temperature of the cold sink?
- A sample of a serum of mass 26.6 g is cooled from 290 K to 275 K at constant pressure by the extraction of 1.05 kJ of energy as heat. Calculate q and ΔH and estimate the heat capacity of the sample. report here the heat capacity = ________ J/k/g. 3 sig. numberA 2.5 mol sample of an ideal gas with a molar specific heat Cv=5/2R always starts at pressure 1.50*105 Pa and temperature 350K. The gas is compressed adiabatically to 200kPa. Final pressure Pf = 200kPa Final volume Vf = 39.5L Final temperature Tf = 380K a) Determine the change in internal energy of the gas (ΔEint, in J). b) Determine the energy added to the gas by heat (Q, in J). c) Determine the work done on the gas (W, in J).A closed cylinder contains 1.0 mole of ideal monatomic gas at 300 oC and 4.0 bar.Insulating the cylinder so that there is no heat exchange with the surroundings, the gas isexpanded to 200 oC and 1.0 bar producing 1247 J of work.a) Is this process reversible or irreversible?b) What is the change in enthalpy (∆H) of the gas?c) What is the change in internal energy (∆U) of thegas?
- You have a gas held isothermally at 297 K whose volume changes from 0.2 m^3 to 9.0 m^3, what is the change in internal energy? Use the fact that the internal pressure of this gas is approximately constant at 100 MPa under these conditions.For a given process( adiabatic, isothermal and isobaric). What would W, heat Q and internal energy of a system be? Write an expression for their relationship as well100 g of liquid benzene at 298 K is isothermally and reversibly compressed from 1 atm to 4 kbar. Calculate a. the heat absorbed by the liquid. b. the work done and c. the change in internal energy. Given: density ρ=0.879 gcm^-3 coefficient of thermal expansion α=1.24x10^-3 K^-1 compressibility coefficient κ=9.6x10^-5 atm^-1
- Everything needed is included Consider the reversible and isothermal compression of 2.0 moles of ammonia (NH3 (g)) from an initial volume of 10.0 L to a final volume of 1.00 L, at a constant temperature of 298 K: 6a. Calculate the work w and heat q associated with this change in volume, considering NH3 to be an ideal gas. 6b. Calculate the work w (but not the heat) using the virial equation of state, with second virial coefficient B = −0.297 L/mol for NH3 at this temperature (and ignoring any higher coefficients).It has been experimentally determined that the heat of combustion of benzene at constant volume is: ΔU ° rxn = -3265.6 kj, at 298K and the heat of combustion at constant pressure is: ΔH ° rxn = -3261.9 kj. C6H6 (l) + 15/2 O2 (g) → 6 CO2 (g) + 3 H2O (l) If we consider that substances in the gas phase behave as ideal gases, responding as appropriate: i) Does the system experience expansion or compression? justify mathematically.Physical chemistry - please refer to pics Now, consider 2.0 moles of methane (CH4 ), initially at 273 K, that is reversibly and adiabatically compressed from an initial volume of 10.00 L to a final volume of 2.00 L. 3a. Determine the final temperature, considering the gas to be described by the ideal gas equation of state. 3b. Determine the work required w, the associated heat flow q, and the internal energy change ∆U for the gas between the initial and final states.