While a few errors were made that caused the molar mass of the butane gas to be slightly off, the values from each trial were within reasonable error. The experiment could be repeated with more success if an apparatus was used to hold the graduated cylinder in place because it would prevent small amounts of butane gas from escaping from the cylinder. In conclusion, the molar mass of a gas can be accurately calculated by using Dalton’s law and Archimedes’ principle. References 1. Britannica, T. E. E. Archimedes' principle https://www.britannica.com (accessed Mar 10, 2018).
Kalambate, Rajaram N. Gawade, Shailesh. B. Khandekar, “Performance Analysis Of Vapour Compression Refrigeration System By Using R134a And Blend Of R290 And R600a”, Journal of The International Association Of Advanced Technology And Science Vol. 16 | March 2015 Issn-3347-4482. 2) Sreejith K., “Experimental Investigation of A Domestic Refrigerator Having Water-Cooled Condenser Using Various Compressor Oils”,International Journal Of Engineering And Science Vol. 2, Pp 27-31, 5 February 2013.
The temperature of the solution affects how much of the solute is dissolved by the solvent but increasing the temperature does not always increase the solubility. The solubility is measured in terms of concentration of an ion that is present in a smaller ratio in solution. On the other hand, solubility equilibrium refers to the equilibrium between the dissolved salt (ions) and undissolved salt that usually exists in a saturated solution or a solution of a sparingly soluble salt. Solubility curves are used to show how the solubility of a substance changes with temperature. The reaction study is in the solubility of naphthalene, C10H8 in diphenylamine, C12H11N, which can be written (for a saturated solution) Naphthalene (pure solid) ↔ Naphthalene (solution, mole fraction on X) The equilibrium constant for this reaction is, K = a_(Naphthalene(solution))/a_(Naphthalene (solid)) ……………….Eq.1 The activity of a pure solid is unity, so Anaphthalene(solid) = 1 If we assume the solution is ideal, the activity of naphthalene in the solution is equal to its mole fraction: anaphthalene(solution) = X, therefore the equilibrium constant is K = X.
This could solved by careful attention to the temperature of the solvent. Also the time of the Erlenmeyer flask in the hot bath during the synthesis of aspirin could have been more than 10 minutes which could have led to more impurities. Also some of the crude aspirin fell on the table. This could be also a factor for a low percent yield. Careful transfer and keen observation is recommended and could possibly lead to a higher percent yield.
E. DRIOLI, M.C. CARNEVALE, A. FIGOLI, and A. CRISCUOLI, “Vacuum membrane dryer (VMDr) for the recovery of solid micro particles from aqueous solutions”, Journal of Membrane Science, Volume 472, 15 December 2014, Pages 67-76. CHE-HSIN LIN, CHING-HSIU CHEN, “Sensitivity enhancement of capacitive type photo-resistor- based humidity sensors using deliquescent salt diffusion method”, Sensors and Actuators B: Chemical, Volume 129, Issue 2, 22 February 2008, Pages
The local Nusselt number of different values of , is shown in Figure.12. T he local Nusselt number decreases with increasing P r for air, water in the case of cooling of the plate. The effects of the phase angles ω t on the average values of the skin friction are shown in Figure.13. The average skin friction decreases with increasing phase angle. The effects of the phase angles ω t on the average values of the Nusselt number are shown in Figure.14.
Beaker 2 cooled by 2.9°C (from 27.9°C to 25°C) and temperature in Beaker 1 fell by 1.9°C (from 29.9°C to 28°C). The cause of this result is the plastic wrap which did not allow the temperature to cool down quickly. In the second part of this experiment, greenhouse gasses were introduced to Beaker 1 by exhaled air. The exhaled air contained Carbon dioxide (CO2) and water vapor (H20). When Part II ended, one cardinal problem was noticed.