n (3) Solutions of aqueous sodium hydroxide and hydrochloric acid react to form water and aqueous sodium chloride. co NaOH(s) → Na+(aq) + OH–(aq) ∆H1 = ? Chemistry with Vernier py In this experiment, you will use a Styrofoam-cup calorimeter to measure the heat released by three reactions. One of the reactions is the same as the combination of the other two reactions. Therefore, according to Hess’s law, the heat of reaction of the one reaction should be equal to the sum of the heats of reaction for the other two.
Results: Zinc Metal - Iodine - Iodide + Triodide + Zinc Ion + Focus Questions: 1. Is there a way to put energy into Zinc Iodide in order to regain the elements, zinc and iodine? If there is a way, how does it happen? Yes, this can be done through electrolysis using a battery and exposed wire tips. Take sample of Zinc Iodide and dissolve in solution.
Name: 6.03: Calorimetry Data and Observations: Part I: Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations that you made over the course of part I. (4 points) I observed that when the metal is placed inside the calorimeter, it transfers heat to the water making the water increase temperature while the metal will decrease temperature. I also noticed that the system was the metal and the surroundings is the water, this is because the water is taking in the heat from the metal making the water warm. Metal Name Mass of Metal Volume of water Initial temp.
A2a. Experimental Design: By using commonly available materials and accurate measuring tools the experiment will allow others to obtain similar results. Connect the multimeter to the two ends of the coil of wire and vary the temperature of the coil of wire. Materials: Precision multimeter to measure resistance Digital timer to measure time periods Multimeter test clips 1000 foot coil of wire (28 gauge) High-precision digital thermometer 1 liter plastic vessel Tap water: Room temperature Ice/Water mix
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.
Carefully immerse the electrons in the solution. Turn the function knob to “pH”. Turn the standardize knob until the meter indicate the exact pH of the buffer solution. Record the pH at which the meter is standardized. Titrating HCl solution with NaOH solution Obtain 25mL of 0.100M HCL solution
What is a spectrophotometer? A spectrophotometer is an instrument used in laboratories that measures the absorbance of materials within the ultraviolet and visible light spectrum. It works by passing light through the material and measures the amount of light absorbed; the higher the concentration, the more light is absorbed. This technique was extremely useful in this lab because by measuring the absorbance of the copper solution, the concentration of copper was determined and the percentage of copper within the penny was calculated. Materials: * Spectrophotometer * 15 M NH3 * 0.40 M Cu2+ Solution * 8 M HNO3 Procedures: Figure out the optimal wavelength for the spectrophotometer.
This happens inside of the mitochondria. • What is the role of the electron transport system? Include the reactants and the products. Where does it occur? The role of the of the electron transport system is to turn the electrons given off from the other two processes and turn them into ATP.
DataQuest Properties of Solutions: Electrolytes and Non-Electrolytes 22 In this experiment, you will discover some properties of strong electrolytes, weak electrolytes, and non-electrolytes by observing the behavior of these substances in aqueous solutions. You will determine these properties using a Conductivity Probe. When the probe is placed in a solution that contains ions, and thus has the ability to conduct electricity, an electrical circuit is completed across the electrodes that are located on either side of the hole near the bottom of the probe body (see Figure 1). This results in a conductivity value that can be read by a datacollection interface. The unit of conductivity used in this experiment is the microsiemens per centimeter, or µS/cm.
,, II I Quantitative Measurements of the Solute Since the solute is the species involved in chemical transformations, our goal will be the determination ot"the number of moles of solute in a particular solution. To be definitive, you want to carry out a reaction that involves zinc iodide. Instead of getting the zinc iodide in the solid state, you go in the .lab and there is a flask that contains zinc iodide diss91ved in water (in the solution state). What might the label on the flask say that will tell you how much iodide there is in the water? · There are numerous measures of the amount of solute in solvent.