Enthalpy Lab Report Essay

The main objective of this experiment is to differentiate between a physical change and a chemical change.

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.

When the zinc was dropped in the hydrochloric acid, the substance began bubbling vigorously, forming a precipitate. Eventually, the zinc dissolved completely. After the lit wooden splint broke the surface of the test tube, there was a loud popping noise. The gas that was released was hydrogen from the acid and the popping noise was a result of the Hydrogen being burned up by the fire creating a small explosion. Two chemical changes occurred in this test: one with the formation of a precipitate (a textbook sign of a chemical change), and the other when the explosion

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

Station two: Station two shows that when a beaker full of cold water is placed over a hot candle flame, many observations take place signifying a chemical reaction, as well as a

In order to complete this lab students must have a well rounded understanding of the science concepts of the phase of gas and the properties of a gas, the experiment apparatus and how it works, the environment of the procedure including standard temperature and pressure and kinetic molecular theory. To complete the calculations students must understand stoichometry and conversion factors. A gas is a phase of matter that has no shape, no set volume, is easily compressed, and is less dense then both solids and liquids. When matter changes its state, gases can be formed. When liquids vaporize and when solids sublimate gases are formed. In the Molar Volume of a Gas Lab the gas is formed when a measured amount of Zinc metal is combined with five milliliters of Hydrochloric Acid the single replacement reaction occurs causing zinc metal to displace the hydrogen and form hydrogen, a gas and zinc chloride, a salt. In this reaction a gas is formed and bubbles of hydrogen are seen. The apparatus needed for this experiment consists of a small tub of water, graduated cylinder

In the lab, Molar Volume of an Ideal Gas, different amounts (in mL) of 6 M HCl were added into a beaker with various amounts (g) of zinc (Zn). In the first test, 10 mL of HCl were added into a beaker with 0.25 g of Zn. The moles of zinc reacted were 0.00382, and this is the same number for the moles of hydrogen produced. In the second test, 10 mL of HCl was added as well as 0.5 g of Zn. The total moles of zinc reacted were 0.00765 and 0.00765 moles of hydrogen were produced. In this reaction zinc was the limiting reactant. The percent error in the reaction was 0.083%.

The purpose of the experiment is to determine if Hess’ Law works in a laboratory experiment consisting of four different reactions. During the first reaction, cold water was placed into a calorimeter and continually mixed with a stir bar. Hot water was then added into the calorimeter while the probe recorded the temperature readings throughout the reaction. The temperature change was then used to find the specific heat of the calorimeter. The same process was used in the second, third, and fourth reactions of hydrochloric acid and sodium hydroxide, ammonium chloride and sodium hydroxide, and ammonia and hydrochloric acid respectively in order to determine the heats of reaction.

In this lab, we will be learning about endothermic reactions and exothermic reactions through experiments involving temperature probes. The first reaction we will be performing involves citric acid and baking soda, and the second reaction involves magnesium metal hydrochloric acid. The two reactions for this are:

The experiment performed showed how the molar volume of hydrogen gas was determined, by reacting a strip of magnesium metal with a leftover of hydrochloric acid, after pressure was equalized underwater, creating H2, or otherwise known as Hydrogen gas. The equation that was formed during the reaction included a single replacement reaction represented in the formula of: Mg(s) + 2HCL (aq) = MgCl2 (aq) + H2 (g). The H2 was collected using a gas tube, also known as the eudiometer. The molar volume of H2, Hydrogen Gas, is determined by calculating the volume occupied by a sample containing a known number of moles of hydrogen is measured. Since the volume will be measured under laboratory conditions of temperature and pressure, the measured volume

Have you ever been sitting there and just wondered about various things dealing with some things in chemistry known as calorimetry or thermochemistry? No, yes, maybe, well whatever your answer you were really thinking yes so I’m going to explain these topics to you in this paper, and teach you how they work so you can figure these things out if you ever run into them I a real life situation.

In this report I am going to use heat of formation to calculate the absorbed or released energy

Thermogenics is defined as using sure food supplements to burn fat. Nearly seven out of ten Yankee adults are thought of overweight and about 3 out of ten are obese. The typical dieter has tried over 7 diets and usually quits as a result of it simply seems too laborious to lose weight. The answer may lie in Thermogenics.

Have you ever wondered why a fire burns orange, or why a lighter burns blue towards the bottom of the flame? If we take a quick step back, this is mostly due to a chemical reaction that is known as the “specific heat”. This must be achieved (as well as the other two properties that every fire is required to possess in order to burn) in order for a flame to become present. After this specific heat is reached, a chemical reaction occurs and turns the fuel source of the fire into a vapor. The aspects that are required for a flame to be created are a heat source, some sort of fuel, as well as some sort of oxidizing agent. The only way that a change in flame color can be observed is by manipulating the fuel source. After we manipulate the source

Figure 1 depicts the cycle used in this experiment and its individual control volumes. The system uses water and refrigerant 134-a as the working fluids. The cycle operates between two different pressures, the high pressure of the condenser and the low pressure of the evaporator. The condenser is used to remove sufficient energy from the refrigerant to transform it completely into liquid. The evaporator is used to vaporize the refrigerant by adding energy supplied by the warm water. The throttling valve serves the purpose of reducing the pressure of the refrigerant resulting in isenthalpic expansion. The compressor supplies energy to the refrigerant, and under ideal conditions works in a quasistatic adiabatic manner.