Statistical Thermodynamics and Kinetics System †MyAssignmenthelp

Question: Discuss about the Statistical Thermodynamics and Kinetics System. Answer: Intoduction: A sample of Benzoic acid of 1 to 1.2 grams was weighted. The sample cap was pre-weighted. The instructions given below was followed using the figure 5.1; The die was set over the receiving cap with three parts resting on the base of the press. The plug was dropped into the die.The die, cup, and plug were transferred onto the anvil while holding one finger against the bottom of the cup to keep it and the plug in place. The die was filled with the roughly weighed sample. The charge was compressed by pushing the lever down. The die was raised or lowered by screwing the anvil up or down until firm pressure was acquired to push the lever through its full stroke (Paula, J. 2010). The lever was raised, the die was slid from the anvil and the cup and plug removed. The cup and die were returned to their original position on the anvil and the plug was gently dropped into the top of the anvil above the pellet.The level was brought down gently to eject the pellet into the cup. Care was taken not to move the level through a full stroke to avoid crushing of the pellet. The lever was raised and parts slid from the anvil. The pellet cup was taken and weighed accurately on balances. Handling of the cup with fingers was avoided as much as possible.The cycle was repeated starting at step 1 for each pellet required. The huge knurled cap was taken out of the bomb and the inside part of the bomb was carefully extracted and put on the special holder provided.The already weighed-sample and cup were placed in the yoke.An ignition wire that had already been cut was used to securely tie each arm of the electrodes allowing a loop between that ensured the wire touched the surface of the pellet. Caution was taken or ensure it did not touch the sides of the metal cup. All parts assembled were put on the lower part of the bomb and pressed down ensuring that the O-ring had fitted well (Bettelheim.F.A. 1971). The knurled cup was tightened making it hand tight.NOTE: it was inevitable for the electrode connections to be placed at 90 from the holes in the cap to facilitate clearance of the electrodes by means of the transport clamp after connection. The hose was attached from the regulator on the oxygen tank to the head of the bomb.The safety valve on the bomb was opened by turning the knurled knob to the left 1-2 times. The cylinder was opened by turning the cylinder valve. The valve was not opened completely. The small knob on the regulator that was black was turned to allow gas movement into the bomb very slowly. The large gauge on the regulator was watched.The bomb was supplied with oxygen for about 15 seconds. The knurled knob was turned down on the safety valve and pressure in the bomb was allowed to build up to about 25 atmospheres. The regulator knob was quickly closed. It was necessary that the pressure in the bomb did not exceed 30 atmospheres.The black lever found below the regulator knob was depressed and any pressure in the line of the bomb was released. A one-way valve in the bomb prevented pressure loss (Reid, P. (2013.)). The hose connection to the bomb was unscrewed and the bomb was carefully placed out of the way of the bench top. The hot and cold water taps were fully turned. At the top of the Calorimeter. The balance knob was turned to O position. The jacket temperature control was turned to minimum. The switch was turned to run position. The power switch was turned on. The controller was run for about 5 minutes to realize some extent of equilibrium. When stabilizing the controller, the stainless still container was filled with deionized water: The weight of the dry container was tarred off and recorded. 20000.2g of deionized water was added to the container (Reid, P. 2013.). The temperature was checked with a lab thermometer so that it lied between 19.5 g to 21C. This was placed in a calorimeter so that it sat on the proper pins in the bottom of the cavity. The special wire holder was used to lower the bomb part way into the water. The leads were attached to the electrodes and slowly lowered the bomb into the water so that it settled on the raised portion of the container. The clamp was removed from the bomb and any water droplets that would have adhered into the clamp were shaken off. The thorough scrutiny was done to ensure there were no bubbles, an indicator that there would have been a leak in the bomb assembly. The cover of the calorimeter was closed and the thermometer was lowered and stirred into position. The solution was allowed to attain equilibrium for about 5 minutes. The temperature on the bucket thermometer was read to discover fluctuation. After the temperature had stabilized, the balance knob was adjusted until the jacket temperature was exactly the same as the container. This had to be done slowly to avoid overshooting the jacket temperature. As the two temperatures approached each other, the white and orange lights interchanged on and off. When the container and jacket temperatures were same, the balance knob was locked and read with the magnifier. The container temperature was measured to the nearest thousandth degree (Nibler.J.W. 1989.). The ignite button was depressed at the front of the calorimeter. After ignition, the container and jacket temperatures begin to rise. Two methods could be used in carrying out standardization and determination. Allowing temperature of the container to rise to the highest. Allowing temperature to rise for a specific time and reading the temperature after this time. For laboratory purposes, this is proffered over the other. The calorimeter was allowed to run for strictly 10 minutes and the temperature rose on the container thermometer. The calorimeter was opened and the stainless still tank was removed. The balance knob was turned back to one and the switch was put at plunge position. The knurled knob on the top of the bomb was slowly turned to allow the pressure inside the bomb is released. The large retaining ring was removed and the bomb open. Remove the small pieces of wire that have not been burned in the bomb and record the total length. The procedure was repeated with benzoic acid and twice with naphthalene. The following were off before leaving; Taps, The calorimeter, Valve on the oxygen tank, Emptying of the oxygen bomb, Denver 5kg balance. The calorimeter is a device used in measuring the amount of heat involved in a physical or chemical process. For instance, when an exothermic reaction occurs in a calorimeter, the heat produced by the reaction is absorbed by the solution which increases its temperature. When the amount of heat involved in a chemical reaction is to be determined in Benzoic acid, the Benzoic acid is burnt in a calorimeter. Benzoic acid is a colorless crystalline solid and simple aromatic carboxylic acid.Its name is derived from its only source known as the gun Benzoic. The chemical formula for Benzoic acid is C7H5O2 =specific heat capacity (Refers to the amount of heat needed to raise the mass by 1 Kelvin or simply the heat capacity per unit mass of a material). The calculated value is -3226.999.The equation relating energy to specific heat capacity is E=m. Where the m= mass of the substance in kg, C= the specific heat capacity in J/, = The temperature change in degrees Celsius. Resonance energy for Naphthalene is 61kCal/mol this value is shifted by around five times -28.6 which is equal to -143.0 kCal/mol. During calculation of the resonance energy of Naphthalene, the enthalpy from the experiment is measured by combustion reaction. The enthalpy of formation for Naphthalene is not measured. The combustion reaction is represented by the equation; In the calculation of the resonance energy, the enthalpy of formation of Naphthalene can be compared with that of bond energies. When using bond energy, for instance, the calculations are done in the gaseous state, therefore, the gaseous state of Naphthalene is; (g) The data below were used to draw the graph of the average conductivity against concentration. No Concentration Average conductivity 1 0.5 622.5 2 1 12.4 3 5 60.3 4 10 1.185 5 20 2.322 References. Atkins, P.; de Paula , J. (2010). Physical Chemistry. W.H Freeman and Company. Bettelheim.F.A. (1971). Experimental Physical Chemistry. Saunders golden series. Engel, T; Reid, P. (2013.). Thermodynamics, Statistical, Thermodynamics, and kinetics. Pearson Education Inc. Shoemaker, D.P, Garland,.C.W.; Nibler.J.W. (1989.). Experiments in Physical Chemistry. McGraw Hill Inc.