Exothermic Lab

This information has massively help to answer by explain the difference between endothermic and exothermic in common language which also helped me know why an exothermic reaction can be used to heat food but an endothermic reaction cannot.

There are new concepts that relate to this lab, such as exothermic and endothermic 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.

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

In this unit we have conducted research and experiments on our chosen reactions to create the highest exothermic reaction for the The Heat-and-Eat meal pack will use a chemical reaction that involves two reactants. Reactant 1 is a solid and Reactant 2 is a liquid.

In this experiment, we investigate the change in temperature caused by adding a chemical substance into the water and dissolving it. The results recorded in the table below show that our hypothesis is correct.

The difference between the potential energy of the products and reactants is released primarily as heat energy into surroundings. This transfer of energy increases the kinetic energy of these particles, increasing the average kinetic energy of the particles, thus increasing the temperature of the surroundings. This evidence of an exothermic

The decomposition of potassium nitrate is the only endothermic reaction. Endothermic reaction is a type of reaction where they have a positive enthalpy due to the energy gain in the beginning of the reactions. At the end of the reaction we end up getting an enthalpy of 13.22 KJ/Mole and end up with 62% experimental error. The highest error that we encounter in this lab was on the neutralization process. The reaction between the acetic acid and the sodium hydroxide end up producing up to the 99%. Experimental error. it might seem very hard to believe; however, we did a wrong experiment on the neutralization section of the lab. We used the strong acid and base combination in this reaction on the first trail. We reacted sodium hydroxide and hydrochloric acid together and we record the data. The reaction between the magnesium oxide and hydrochloric acid produced the enthalpy of -79.55and 86.7 experimental error. one big thing that seems to be constantly seen on this lab is that most of the reaction that is used on this lab were all exothermic except the potassium nitrate which was

From the results recorded it was identified that activity A and C had exothermic reactions, whilst activity B had an endothermic reaction. Each of the activities had initially begun with 23.4/8/9oC, however, within one minute of adding the 2nd reactants, the results began showing, as seen from the graph. Activity A and C had risen in temperature, with A gaining 4oC and in total of 2 minutes having the temperature of 27.9oC along with C increasing by 2.2oC and within 2 minutes of the experiment having the temperature of 26oC. Activity B however was the anomaly in the test, as the temperature went lower, by 1.9oC as within 2 minutes, the Ammonium Chloride and water had the temperature of 21oC. Furthermore the line graph shows Activity A and C

at each temperature was calculated resulting in negative values, signifying the reaction was spontaneous. As temperature increased thevalues got less negative. The values ranged from -579 kJ to -510 kJ. The smallestvalue was -579 kJ at 6.0 oC (279 K) and the largest was -75.3 at 55.0 oC (328 K). The only value that did not agree with the other numbers was thevalue at 55.0 oC (328 K) having the largest value of -75.3 (kJ), which resulted in some discrepancies in the graph and a really poor best fit line when observing the graph ofverses temperature for the Al/Mg cell in figure 1 making it difficult to observe any trends. The positivevalue for the graph indicates an endothermic reaction, therefore the surroundings loses heat and its entropy decreases as can be observed by the -value for the slope of the graph.

Endothermic reactions take energy in from its surrounding. (BBC, 2014) The opposite reaction, an exothermic reaction, releases heat due to a chemical reaction and gives energy. For a reaction to be endothermic, the enthalpy of the product must be higher than that of the reactants. (ChemWiki, 2015)

We already knew that exothermic means to exit or release heat energy. Endothermic means to absorb heat energy. Chemical reactions are when one thing changes into another but it cannot return to it’s original form. We read about instant hot packs and cold packs and how they are chemical reactions. When water mixes with different salt or some substances it can cause a decrease or increase in temperature. In our experiment our guiding question was which of the following substances would make an economical hot pack or cold pack? This goes to show how you can use your background information on endothermic and exothermic also chemical reactions to make and economical cold pack or hot pack you would have to think through what substance would work

In the reaction between HCl and NaOH, the temperature change was 13.474 °C for the first trial and 13.71 °C for the second

Purpose: This lab taught procedures for determining heat of capacity of a calorimeter and measuring enthalpy of change for three reactions. It also enforced methods of analyzing data obtained through experimentation and calculating enthalpy. These procedures are used in the branch of thermodynamics known as thermochemistry which is the study of energy changes that accompany chemical reactions. Concepts from this lab can be used to determine the potential energy of a chemical reaction. Much of the energy people depend on comes from chemical reactions. For example, energy can be obtained by burning fuel, metabolizing of food or discharging a batter.

In this experiment, 25mL of HCl will be mixed with 25mL of NaOH in a calorimeter. The temperature change of the solution will be measured and used to determine the heat released by the solution according to the formula q=mCspT. The mass of the solution will then be used to determine