can be determined u mple procedure. To determine the values of the properties of
ID: 999503 • Letter: C
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can be determined u mple procedure. To determine the values of the properties of interest transitionfrom State l to State ll plus for the SPONTANEITY OF A PROCESS experimentally using a mamic properties associated with a spontaneous simple you will use some important state function. Consider three States of a system: State I enthalpy change associated with the transition from State I to ic relationships 1. The path independence of State II, and State lIll. The enthalpy change associate ependence of any state function. Consider three States of a system: Sta Statead State Ill T State IlI equals the sum of transition from State II to State IIl sum, of H for the 2. The relationship between G, and Kn 3. The relationship between G and G. 4. The relationship thatexists between G, aH, T, and s at constant T o apply the important themodynamic relationships, we will make some approximations. You e important thermodynamic rela will calculate a value for G based on solubility data at 17 C and25 C, while the experimental emperature will be between 17 C and 25'C. Because of approximations we make, the calculated thermodynamic values will be slightly different than their actual values. We are more interested in exploring the relationship between the properties than in obtaining precise Urea, H2NCONH2, is an important organic compound. Ure product of the me is excreted in human urine. Urea is also historically important because it H2N was the first organic compound to be synthesized from chemicals not directly derived from living organisms. Urea was synthesized from ammonia and carbon dioxide and can be hydrolyzed by certain enzymes, such as urease, a is an encd nimals. About 25 g of urea per day back to ammonia and carbon dioxide. You will investigate the dissolution of urea in an adiabatic calorimeter. Enough solid urea will be dissolved to give a solution that is approximately 1.5 M urea. For an adiabatic process, we would expect a temperature change to occur, ie ,aT T' - T, 0. You will be asked to determine the enthalpy change for the isothermal dissolution of urea, aHuo. Isothermal processes have AT = 0, but we expect a temperature change in our experiment. How will we calculate Hao when we experimentally determine aHad? We can define State I to be solid urea and water at temperature T: State lI is defined as a 1.5 M urea (aq) solution at temperature T and State Ill is defined as a 1.5 M urea (aq) solution at temperature Ti. The pressure is the same for all three states. The following diagram illustrates the relationship between the three states State II: urea (aq) at T AHad State 111 State l urea (s) + H20 (1) at T urea (aq) at T A transition from State I to State Ill represents the isothermal dissolution of solid urea to form a 1.5 M solution, so the enthalpy change is tso. The experimental process is an adiabatic SPONTANEITY EXP. NOTESExplanation / Answer
First you try to understatnd all the thermodynamic, extensive functions(DeltaE,DeltaH,DeltaG,DeltaA) and their physical meaning with a small example each.
1) write down their mathematical equations how they are related to eachother and practice the equations again and again. You need to know about only four functions as I mentioned above.
2) Try to understand how these four equations are related to the laws of thermodynamics. At this point, you will have better clarity.
Then separate all the equations accordingly.
Since, forexample entropy is concept of second law of thermodynamics, again you write down all the equations how they are related to the entropy.(solve few problems on it)
Do everything one by one carefully because here units were also most important. Do some excersizes on conversion of units.
All the best.
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