Neutralization Reaction

Using a thermometer we observed the measurement of the water “H2O” in the beaker, and it resulted in an initial temperature of 20 ⁰ C.

he experimental variable in this experiment was the changing number of Alka Seltzer tablets that were put into the 250mL beaker of vinegar. Some of the control variables in this experiment were that the same beaker and thermometer were used for each trial, the same type of vinegar and Alka Seltzer were used for each trial, and the same amount of vinegar. The original Hypothesis was that more Alka Seltzer would increase the temperature of the vinegar was not correct. After analyzing the data it can be seen that for the first trial the temperature did not change as it stayed at 24 degrees Celsius before and during the reaction with 1 tablet, also for trial two with two tablets the temperature stayed the same at 23 degrees Celsius and did

If the two solutions are not at the same temperature a correction must be made to find the correct change in temperature. This is done by using an equation where the initial volume and temperature of NaClO is multiplied together and the initial volume and temperature of Solution “A” is multiplied together, and the two answers are added and then divided by 50

An Investigation into the Enthalpies of the Combustion of Alcohols = == == == ==

In order to measure the heats of reactions, add the reactants into the calorimeter and measure the difference between the initial and final temperature. The temperature difference helps us calculate the heat released or absorbed by the reaction. The equation for calorimetry is q=mc(ΔT). ΔT is the temperature change, m is the mass, c is the specific heat capacity of the solution, and q is the heat transfer. Given that the experiment is operated under constant pressure in the lab, the temperature change is due to the enthalpy of the reaction, therefore the heat of the reaction can be calculated.

This reaction is exothermic, meaning it releases heat when reactants are converted into products. The negative change in enthalpy (∆H° = -36,757 J) for this reaction indicates that the reaction is losing heat to its surroundings.

When the volumes of NaOH and CH3COOH were equal, the temperature increased by 5 degrees celsius. When we performed a second trial and added 15 mL of NaOH and 5 mL of CH3COOH, the temperature only showed an increase

In relation, a second heating may not have been performed. This would affect the results because if there is additional water, there is added mass which would also throw off the overall masses and ratios. This could be prevented if more time was given for the heatings. Lastly, when adding the HCl to the baking soda, the watch glass may not have been shielding the splattering coming from all the fizzing and this would result in a loss of mass and again, throw off the results. This could be fixed by using a taller dish or a crucible to prevent so much substance from

Some explanations could be the size of the paper around the probe was not consistent causing an error in the temperature change. Some ways to fix this error is to make sure the size of the paper is consistent in each trial. Also, volume of alcohol in the test tube was not consistent in each trial, it was approximately 2 cm. This causes errors because it can effect the change in temperature for each trial and effecting the average. An improvement is to measure 2 cm of alcohol exactly reducing any errors which will effect the

The literature value for the enthalpy change of the last reaction which was provided by our teacher is -97 kJ mol-1. Agreeing this value, our result can be considered accurate.

We will be using 6 different fuels to heat up 100ml of water, and find out the changes of the temperature. We will measure the temperatures of the water before and after the experiment. We will burn heat the water for exactly 2 minutes, and check the changes in temperature. The change in temperature will allow us to work out the energy given off the fuel by using this formula:

This experiment was performed to determine the heat of neutralization between Hydrogen chloride (HCl) and Sodium hydroxide (NaOH). A temperature probe was used to measure the temperature of the reaction when the base (NaOH) was poured into the acid (HCl). The data was collected on logged on LoggerPro.

Introduction: The theory behind this experiment is the heat of a reaction (∆E) plus the work (W) done by a reaction is equal to

6. Calculate the molar enthalpy in Joules per mole of NaOH for each reaction. Show work here and record your answer in Data Table 2.

Purpose: You will determine the molar heat of neutralization of 1.00 M HCL and 1.00 M NaOH in Kilojoules.