Write a hypothesis on what you think will happen when mixed. 3. Combine the substances; record observations. Hydrochloric Acid and Magnesium 1. Add hydrochloric acid to a test tube.
Objectives: The purpose of this lab is to observe the reaction of crystal violet and sodium hydroxide by looking at the relationship between concentration and time elapsed of the crystal violet. CV+ + OH- CVOH To quantitatively observe this reaction of crystal violet, the rate law is used. The rate law tells us that the rate is equal to a rate constant (k) multiplied by the concentration of crystal violet to the power of its reaction order ([CV+]p) and the concentration of hydroxide to the power of its reaction order ([OH-]q). Rate = k[CV+]p[OH-]q To fully understand the rate law, concentrations of the substances must be looked at first. The concentration is measured in molarity.
The test for Sodium Bicarbonate included mixing that with HCl. After doing this experiment bubbles would form in the solution. This was CO2 being released. This reaction is a way of testing for Sodium Bicarbonate. BACKGROUND: For these experiments a 96-well plate was used.
The purpose of this lab was to find the molecular weight of two unknown substances by analyzing the freezing points in cyclohexane and to provide a visual representation of the freezing point depression effect. The theory of this lab is; by using measurements of mass of the unknown substances (solute) in correlation with the mass of the cyclohexane (solvent) and the freezing point constant of the solvent, you could determine the molecular weight of the solute by using the same math involved in deciding the freezing point of the solution/ The theory behind the visual of the FPD effect is that if one was to record the freezing point of a solution and two solutions of the same substances with more solute, one would see a visible drop in freezing point. The equations you needed for this lab were the freezing point formula for organic substances (ΔFp=(m)Kf) and the
In our lab we use a more sophisticated one which included a lid on the cup with an inserted thermometer and a stirrer. Thermochemistry is the study of the heat released or absorbed as a result of chemical reactions. The measurement of the total energy of a thermodynamic reaction is called enthalpy (q). This is the basis for Hess’s law which states that if two reactions are combined to yield a third reaction, the sum of the first two is equal to the third. The energy change is the same whether the process occurs in one step or many.
Stoichiometry is a section of chemistry that involves using the relationships between reactants or products in a chemical reaction to determine the desired quantitive data. 4. Using the balanced chemical reaction between Sodium carbonate and Calcium Carbonate given in page 92 of your lab manual (first paragraph of procedure), find the mass of Sodium Carbonate (in grams) needed in reaction? Na2CO3(aq)+CaCl22H20(aq)-CaCO3(s)+2NaCl(aq)+2H2O Date:_____3/30/2015____________ Name______Chloe Flake______________ 1. Title: 1pt Stoichiometry Of A Precipitation Reaction 2.
| Chemistry Coursework | How does the concentration of Hydrochloric Acid affect the rate of reaction between Hydrochloric Acid and Sodium Thiosulfate? | | | Initial Planning The aim of my coursework is to investigate the variables that increase the rate of reaction. There are several equations that can be investigated. The main 3 equations are: 1) Hydrochloric Acid + Marble Chips Calcium Chloride + Water +Carbon Dioxide 2HCl (aq) + CaCO3 (s) CaCl2 (aq) + H2O (l) + CO2 (g) 2) Hydrochloric Acid + Magnesium Magnesium Chloride + Hydrogen 2HCl (aq) + Mg (s) MgCl2 (aq) + H2 (g) 3) Hydrochloric Acid + Sodium Thiosulfate Sodium Chloride + Sulfur Dioxide + Sulfur + Water HCl (aq) + Na2S2O3 (aq) NaCl (aq) + SO2 (g) + S (s) + H2O (l) In equation 1, the CO2 produced is monitored over a certain period of time. The more CO2 produced over this time, the higher the rate of reaction.
Born- Haber cycle 1. The lattice enthalpy of magnesium chloride, MgCl2, can be determined using a Born-Haber cycle and the following enthalpy changes. |Name of process |Enthalpy change/kJ mol-1 | |Enthalpy change of formation of MgCl2 |-641 | |Enthalpy change of atomization of magnesium |+148 | |First ionization energy of magnesium |+738 | |Second ionization energy of magnesium |+1451 | |Enthalpy change of atomization of chlorine |+123 | |Electron affinity of chlorine |-349 | a) Define, using an equation with MgCl2 as an example, what is meant by the term lattice enthalpy. b) Construct a Born-Haber cycle for MgCl2, including state symbols, and calculate the lattice enthalpy of MgCl2. c) Explain why the lattice enthalpy of NaBr is much less exothermic than that of MgCl2.
The first example is calculating empirical formulas from percent compositions using the percents of the different elements. Empirical formulas of compounds are also determined through quantitative analysis by using the masses of each element in the equation3. Lastly, this experiment uses the method of finding empirical formulas through combustion analysis. The empirical formula of magnesium oxide is found from the combustion of magnesium1. The four chemical equations that result when metal magnesium is heated in a closed crucible that becomes gradually exposed to the oxygen in the air are shown in table
Title: SOME AQUEOUS SOLUTION CHEMISTRY OF COPPER(II)ION Aims: 1. To make the synthesis of Copper(II) Sulfate Pentahydrate and determine the theoretical yield as well as the percent yield of CuSO4.5H2O 2. To observe a series of reactions with copper (II) ions using different reagents. Results & Questions: A. Synthesis of Copper(II) Sulfate Pentahydrate. 1.