One vaporization and condensation cycle is called a theoretical plate. The greater the amount of theoretical plates, the better the separation will be. In this experiment, there are two theoretical plates. The first plate is the initial distillation where three different fractions are collected over different temperature ranges. The first fraction is collected at 60-75℃, the second fraction is collected at 75-85℃ and the final fraction is collected at 85-105℃.
Molecules at higher temperature have more thermal energy. Introduction Chemical Kinetics, also known as reaction kinetics, is the study of rates of chemical processes. Chemical kinetics includes investigations of how different experimental conditions can influence the speed of a chemical reaction and yield information about the reaction’s mechanism and transition states, as well as the construction of mathematical models that can describe the characteristics of a chemical reaction (Clarke, 1974). Chemical kinetics deals with the experimental determination of the reaction rates from which rate laws and rate constants are derived. Relatively simple rate laws exist for zero-order reactions (for which concentration rates are independent of concentration), first-order reactions and secondorder reactions, and can be derived for others.
Introduction: The purpose of this experiment is to determine the empirical formula of magnesium oxide formed by the reaction of magnesium with oxygen. To work out formula by the experiment it is necessary to measure the exact masses of each element present in a sample of a compound. Knowing the masses of magnesium and oxygen and its molar masses it is possible to find how many moles of each element is present in the magnesium oxide. The number of moles then can be used to obtain a molar ratio, which gives us the empirical formula of the compound. During the combustion reaction the ribbon of magnesium metal is heated, it reacts with oxygen from the air in a crucible, producing magnesium oxide: magnesium + oxygen → magnesium oxide We measure the mass of magnesium we use for the reaction, and the mass of magnesium oxide produced at the end of it, then we can work out the mass of oxygen that has been combined with the magnesium.
Density Determination Introduction: The purpose of this lab is to identify several different substances by determine the density and other physical characteristics of the substances. Density is an important property of matter and may be used as a method of identification. The density of a substance would not change based on the mass or volume of the substance. Mass is the quantity of matter. In physics or chemistry, units such as kilograms (kg), grams (g) can be used to measure the mass of a substance.
Based on the Bayle’s Law, the pressure of the gas is inversely proportional to the volume with fixed temperature. Conclusion: Our experimental result shows the slope of our graph of Inverse Volume versus Pressure is 2330 + 15Kpa*ml. We used the slope divided by (R*T), then we are able to find value of n which is n=9.50*10^-4. Our graph is a linear line, which means the product of pressure and volume is a constant (value of slope). Thus we are able to find that the pressure of gas is inversely proportional to the volume with fixed temperature.
[2] to determine the Activation Energy. This equation is simply the equation of a line (y = mx + c) and from the graph the Activation Energy can easily be calculated. Procedure: As per lab manual. [3] Calculations: 0.4977 M sodium thiosulphate 1.01ml rough 1.04ml final volume of Na2S2O3 0.4977 mole/L -> 0.004977mol/ml x 1.04ml = 5.176 x 10-4 moles =
Abstract In this experiment, the purpose was to investigate the relationship between the vapor pressure of a liquid and its temperature. The purpose of the extension was to prove this relationship using the Clausius-Clapeyron equation, including data found during the main experiment procedure(s). The experimental results obtained supported our hypothesis in this procedure the relationship of vapor pressure to temperature was found. The hypothesis was that the two bore a direct relationship to each other, which means one increasing as the other increases. The data collected supports the original hypothesis.
By, solving the system of equations using linear algebra, the concentrations of the indicator and the conjugate base were determined. The Henderson-Hasselbach equation predicted that the pH for these solution plotted against the log of the ratio of the two species would yield a line whose Y-intercept equaled the pKa for methyl red. The value obtained was 4.96(1), which has a percent error of 1.9. Perhaps, if this were corrected for temperature there would be even greater agreement with the accepted value. INTRODUCTION The purpose of this experiment was to determine the pKa of an acid-base indicator (methyl red).
In the Rankine cycle, heat is added reversibly at a constant pressure but at infinite temperatures. If Tm1 is the mean temperature of heat addition as shown in Fig. 6, then the area under 4 and 1 is equal to the area under 5 and 6. Then, we found the efficiency of this cycle is Rankine = 1 – (T2/Tm1), Where T2 is the temperature of heat rejection. The lower is the T2 for a given Tm1, i.e.
Experiment 7 Formula of a Complex Ion by the Continuous Variation Method Objective: To determine the formula of a complex ion by the continuous variation method. Procedure: Refer to laboratory manual. Results and Calculations: 1. Calculate the molarity of both CuCl2 solution and the ethylenediamine solution. Number of moles of CuCl2 used = [pic] =[pic] = 0.127 moles Therefore, Molarity of CuCl2 = [pic] = [pic] = 0.063 mol/dm3 Number of moles of ethylenediamine used = [pic] =[pic] = [pic] = 0.1 mole Therefore, Molarity of ethylenediamine = [pic] = [pic] = 0.05 mol/dm3 2.