Endothermic Reaction Lab

Is this reaction endothermic or exothermic? What does that mean and how do you know? (~3 sentences)

Abstract: An ice calorimeter was used to study the reaction of magnesium metal and 1.00M

The aim of the lab was to determine the molar enthalpy of the combustion of magnesium using values from reactions between magnesium and magnesium oxide in hydrochloric acid solution using Hess’s Law and Calorimetry. The calculated molar enthalpy of the combustion of magnesium from this experiment was -633.6KJ/mol. This result was found by putting a known mass of magnesium metal as well as magnesium oxide powder into a concentration of HCl. Firstly, a styrofoam calorimeter was used to determine the standard reaction temperature of magnesium metal and hydrochloric acid. Next, calorimetry was again used to determine the reaction temperature of magnesium oxide and hydrochloric acid. Lastly, the thermochemical equations for the two

At the beginning of lab eight it was hypothesized that the reaction between 60 mL of soda, .5 g of pop rocks , and 20 mL of .64 M HCl was a exothermic reaction. It was also hypothesized that lethal dose of pop rocks and soda would be fairly high. This hypothesis was based on prior information and estimation of the lethal dose ratio. After calculating the heat released (q) and finding -1.0506 J it was determined that the chemical reaction between pop rocks and soda is exothermic. The reaction was also considered exothermic due to heat being released and the temperature increasing.This part of the hypothesis was found to be correct , however the second part of the hypothesis was incorrect. After calculating the LD50 ratio the lethal dose for pop rocks was 3.59 g and the lethal dose for soda was .413 g. The lethal dose of the soda and pop rocks was significantly lower than expected.

Is A+C a chemical reaction? Yes, because of serval chemical changes happening to the solution before and after. I came to this conclusion by using three pieces of evidence. The three pieces of evidence were a ph imbalance, a dramatic density rise, and a change in electroconductivity.

What is the percentage yield of the reaction of iron and copper chloride when steel wool and copper chloride dehydrate are used as reactions?

Endothermic reactions are accompanied by the absorption of heat. The dissolving of ammonium nitrate in water is an example of an endothermic reaction. The solution resulting from this mixture is colder than either the ammonium nitrate or the water. This is the simple explanation of what happens in an instant ice pack. The more detailed information will be discussed in the following paragraphs.

Because the value in the theoretical mass of CO_2 lost in the first run was 0.566 g and the mass obtained from the experiment was 0.618 g. This shows that 0.618 g was close to the theoretical value and it had a 9.11% error. On the other hand, the values of sodium carbonate had a greater percent error (22.2% and 39%) which meant that there was a big difference between the theoretical expectation and the actual mass obtained. Some discrepancies that could of cause the values to differ are the grams of NaHCO_3 and Na_2 CO_3 added to the beakers because some values were close to one gram or a little more than a gram. Another discrepancy is that some of the HCl might have stayed in the volumetric pipette; therefore this would of affected the weighted mass of the beaker with the

In the last reaction with metal, a magnesium ribbon strip will be added to one in a half inches of hydrochloric acid. Another tube will be added on top to trap the gas from the magnesium ribbon reacting in the first tube. After the reaction, a wooden splint will be lighted in the opening of the test tube on the top. Furthermore, in the step of testing for gaseous products within decomposition reactions, a test tube containing ten grams of ammonium carbonate will be inserted into the Lab-Master heater set to seventy degrees Celsius, which can be increased over time. After the production of ammonia, cobalt chloride paper will be inserted in the tube.

3. The third source of error is not knowing for how long to exactly heat the magnesium until it no longer ignites and forms into a white powder of magnesium oxide. In the procedure, it is stated for how long to heat the magnesium, but as the lab went on, it is realized that the magnesium had to be heated for a longer time. This could mean that the magnesium could have been not heated long enough or too little for it to be fully converted into the magnesium oxide product effecting the final results of the lab by having smaller

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

    In this lab, a calorimeter was used to find the enthalpy of reaction for two reactions, the first was between magnesium and 1 molar hydrochloric acid, and the second was between magnesium oxide and 1 molar hydrochloric acid. After the enthalpy for both of these were found, Hess’ law was used to find the molar enthalpy of combustion of magnesium, using the enthalpies for the two previous reactions and the enthalpy of formation for water. The enthalpy of reaction for the magnesium + hydrochloric acid reaction was found to be -812.76 kJ. The enthalpy of reaction for the magnesium oxide + hydrochloric acid reaction was found to be -111.06 kJ. These two enthalpies and the enthalpy of formation for water were manipulated and added together using Hess’s law to get the molar enthalpy of combustion of magnesium. It was found that the molar enthalpy of combustion of magnesium was -987.5 kJ/mol. The accepted enthalpy was -601.6 kJ/mol, which means that there is a percent difference of 64%. This percent difference is very high which indicates that this type of experiment is very inefficient for finding the molar enthalpy of combustion of magnesium. Most likely, a there are many errors in this simple calorimeter experiment that make it inefficient for finding the molar enthalpy of combustion of magnesium.

Endotherm are animals that regulate internal temperature at a range dispie ambient temperature changes. This research will aid to identify how different ambient temperature will affect the mice’s metabolic rate. Previous research suggest that thermo neutral zone is the range which endotherm conduct metabolic with least stress. However to understand the exact relationship between the change in ambient temperature on endothermic metabolic rate, metabolic system measurement would be carried out to measure the ambient temperature and oxygen percentage. The hypothesis was that as the mices experiences ambient temperature outside of their thermal neutral zone, then they will intake more oxygen because more metabolic activities need to take place

Introduction: Every chemical change is accompanied by a change in energy usually in the form of heat. If heat is evolved, the reaction is exothermic, and if heat is absorbed, the reaction is endothermic. The energy change of a reaction that occurs at constant pressure is called the heat of reaction or the enthalpy of reaction (ΔHr). This quantity of heat is measured experimentally by allowing the reaction to occur in a calorimeter. In this experiment you will determine the heat of neutralization when an acid and a base react to form 1 mole of water. In a perfect calorimeter, heat is exchanged only between the reaction and the calorimeters water. Technically, some heat may may be absorbed the calorimeter. All calorimeters exchange some heat with its environment. This amount of heat is called the calorimeters heat capacity (the amount of of heat required to raise its temperature 1∘Celsius). We are going to “pretend” that our calorimeter is the perfect calorimeter.

Overall, the experiment succeeded that the metals show the theoretical properties. Differences existed in the mathematical calculation of the actual length. These differences, however, it can be accounted for by experimental error; more over there are uncertainty on purity of the