Lab Report

The initial concentrations of the reactants in Table 1—that is, [Fe3+] and [SCN–] prior to any reaction—can be found by a dilution calculation based on the values from Table 2 found in the procedure. Once the reaction reaches equilibrium, we assume that the reaction has shifted forward by an amount, x. Notice from Table 1 that the value of x is simply equal to the equilibrium concentration of FeSCN2+(aq), or that x = [FeSCN2+] at equilibrium. The equilibrium value of [FeSCN2+] is determined spectroscopically using Beer’s Law. Its initial value in the table is zero because no FeSCN2+(aq) is added to the initial solution. Finally, the equilibrium concentrations of the reactants, Fe3+(aq) and SCN–(aq), are found by subtracting the equilibrium concentration of FeSCN2+(aq) from the initial concentrations of Fe3+(aq) and SCN–(aq), as shown in the table above. Once all the equilibrium values are

Reaction 2 - 1.Used a Beral- type pipet, added about 2mL (40 Drops) of 1M hydrochloric acid solution to a small test tube.

The mole is a convenient unit for analyzing chemical reactions. Avogadro’s number is equal to the mole. The mass of a mole of any compound or element is the mass in grams that corresponds to the molecular formula, also known as the atomic mass. In this experiment, you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride, determine the number of moles of iron used up in the reaction of iron and copper (II) chloride, determine the ratio of moles of iron to moles of copper, and determine the number of atoms and formula units involved in

Abstract: This two part experiment is designed to determine the rate law of the following reaction, 2I-(aq) + H2O2(aq) + 2H+I2(aq) + 2H2O(L), and to then determine if a change in temperature has an effect on that rate of this reaction. It was found that the reaction rate=k[I-]^1[H2O2+]^1, and the experimental activation energy is 60.62 KJ/mol.

An association between enzyme production, gene copy number, and gene evolution was explored by conducting analysis of the salivary amylase enzyme, AMY1A gene copy number, and the ancestral starch consumption in Homo Sapiens (Tracey 2017, p.22). It was hypothesized that the relative amount of starch consumption was very high for my personal ancestral diet, thus my AMY1 diploid gene copy number in my genome and salivary amylase concentration would be significantly higher than the population mean. With a population of 28 subjects (n=28), individual saliva samples were collected and compared to a calibration curve to determine the approximate amylase concentration by analyzing absorbance values. Individual samples of buccal cheek cells were

The yield of following reactions for methane is related to the temperature and the amount of natural gas. The mass balance for free carbon and hydrogen is mentioned as

Therefore, the hypothesis of this experiment is that by heating the hydrated copper (II) sulfate, converting

The rate of a reaction varies at different temperatures and reactant concentrations. In this experiment, the orders and dependence of the rate constant of the products used are determined by the following chemical reaction:

Koczanski, Krystyna; Xidos, James D. CHEM 1300 Laboratory Manual; UMSU Copy Centre: Winnipeg, MB, Canada, 2013, pp

The literature value for the enthalpy change of the last reaction which was provided by our teacher is -97 kJ mol-1. Agreeing this value, our result can be considered accurate.

The formation constant of FeSCN+2(aq) was determined through the use of the visible spectrophotometric measurements. This was then used to determine the enthalpy or ΔH° and entropy or ΔS° of the reaction. The adjusted Kc experimental value was determined to be 148 ± 7.2 compared to the known value of 146. This shows a percent error of 1.37% which is good. Enthalpy was determined to be -6.44 ±……. kJ/mol compared to the known value of -4.66 kJ/mol. This shows a percent error of 38.2% which show poor accuracy. The experimental value of entropy was determined to be 20 ± …..kJ/mol compared to the known of 25.81 kJ/mol at 298.15

In the fourth reaction, 15 mL of 6.0 M sulfuric acid was added to the copper (II) oxide while stirring. The balanced equation for this reaction is as follows:

Purpose: To measure the heats of reaction for three related exothermic reactions and to verify Hess’s Law of Heat Summation.

Two catalyst reactants are used in the experiment, thiosulfate and starch, to dictate the time of reactions.

To find the value of the pre-exponential factor, ������������ , and activation energy, ������, would require linearizing the Arrhenius equation given as: k = k o ������ −������������ , where R is the gas constant and T is the temperature the given k is at in degrees Kelvin. Equation 8 is linearized by taking the natural log of both sides: ln(k) = ln(k o ) − E . RT