What are the identities of the substances found after electrolysis and heating? The identities of the substances found were Iodine, Iodide ion (I-), Triodide ion(I3-), Zinc metal and Zinc ion(Zn2+) Post Lab questions: 1. What did this experiment convincingly show about the composition of the white solid? I put that the experiment showed us the white substance was comprised of Zinc ions and iodide ions, and that the two ions and be separated back into their respective elements 2. During the electrolysis, a gray solid formed on the negative wire of the battery and the dark red solution formed at the positive wire of the batter.
Lesson 13.6 Changes of physical state: * necessary to draw a temperature-energy graph to see the change in temperature with a constant application of heat Heat of fusion - the amount of heat required to melt 1.00 g of substance. substance changing from a solid to a liquid. Heat of vaporization - the amount of heat required to vaporize 1.00 g of a substance. substance changing from a liquid to a gas. heats of vaporization and condensation are equal.
1 q= Cs x g x T Q represents heat. Specific heat (Cs) is multiplied to the mass (g) and temperature change that occurred in the reaction. ( T). Specific heat is defined as the amount of energy required to raise the temperature of 1 g of a substance by 1 K, under a constant pressure. Considering the fact that substances have differences, the specific heat varies depending on what substance is being heated.
Afsana Islam CHEM 106 – LAB Lab Report #4 03/02/2015 Focus Questions: Is mass conserved in the chemical reaction that you studied in lab? The mass of the zinc and iodine were definitely conserved. The mass did not change much after the chemical reaction occurred. Raw Data: Experiment # Mass of “R” boiling tube Mass of Zinc used in Mass of Iodine used in Mass of excess zinc and “R” boiling tube after r/h/c Mass of excess zinc and “R” boiling tube after r/h/c a 2nd time Mass of “P” boiling tube and boiling chip Mass of “P” boiling tube, boiling chip, and zinc iodide after h/c Mass of “P” boiling tube, boiling chip, and zinc iodide after h/c a 2nd time 1 40.63g 2.00g 3.00g 40.83g 40.83g 41.46g 45.29g 45.29g 2 40.63g 1.00g 2.00g 41.09g 41.09g 42.25g 44.60g 44.60g
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.
Simple and Fractional Distillation of Cyclohexane and Toluene Purpose: The purpose of this experiment was to become familiar with the processes of simple and fractional distillation. In this experiment a mixture of two volatile compounds, cyclohexane and toluene, were separated with the process of distillation. Distillation relies on each compound having distinct and separate boiling points. The pure products were analyzed with gas chromatography to determine the success of the distillation. Introduction: Distillation is the process of heating a liquid until it boils, then condensing and collecting the resulting hot vapors.
The reaction that occurred with this step was displacement and metathesis in the form of gas formation. The balanced equation of this step looks as follows: CuSO4aq+Zns→Cus+ZnSO4(aq) Once this step was finished, the remaining copper was retrieved. First, to recover the copper HCl was added to remove all the zinc. When this happened, a yellow tint was observed in the liquid, as well as bubbling as the zinc was broken down. Once the copper dried out, it was weighed and came to a total of 240 mg.
Copper Cycle Lab Purpose: In this experiment the student will gain familiarity with basic lab procedures, some chemistry of a typical transition element, and the concept of percent yield. Equipment: Balance (2) 250 mL beakers Evaporating dish Stirring rod Hotplate 100 mL grad cylinder Weighing paper Materials: 0.5 g of copper wire 2.0 M H2SO4 (aq) Acetone Conc. HNO3 (aq) 3.0 M NaOH Granular zinc Introduction: Understanding the type of reaction taking place is an important part of predicting the products of a reaction. Common chemical reactions can be described as synthesis, decomposition, single replacement, double replacement, combustion, or oxidation and reduction reactions. Each of these types of reactions behaves in a similar fashion.
Thermal runaway reaction occurs when the heat generated by a reaction goes beyond the heat removal caused by the available cooling capacity. Heat is accumulated leading to a gradual rise in the temperature of the reaction mass; this causes an increase to the rate of reaction and increases the speed of rate of heat generation. [1] Why are thermal runaway reactions dangerous on industrial scale? Thermal runaway reactions are always said to be dangerous on an industrial scale since the reactions go faster in an industry where they tend to reach higher temperatures. As you would already know that exothermic reactions tend to release quite a large amount of heat, so when the reaction mixture gets very warm, a very hot exothermic reaction begins.
Aluminum, for example, expands twice as much as iron when both are heated the same amount. Rubber and water are two common substances that differ from most others in their response to heat. Rubber contracts when heated. Water loses volume when its temperature rises from 0° C. to 4° C. (32° F. to 39° F.). It expands when its temperature rises above 4° C. (39° F.).