2 M Naoh Reaction Lab

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

The energy is given out when forming the bonds between the new water and carbon dioxide molecules. The amount of energy produced by such exothermic reactions can be calculated by using the formula Mass of the substance x rise in temp x SHC (specific heat capacity). The

In this experiment, multiple titrations were performed in order to accurately identify the unknown concentration of HCl that was present in a solution. Specifically, the strong base NaOH was used to accomplish this. In addition to this, the NaOH was standardized, and from this, the concentration of NaOH was also determined. Experimentation called for no repetition, however, if the experiment were repeated, a more effective method of measuring the KHP and NaOH compounds could have been used. Also, the experiment could have allowed for a more precise method of depositing the NaOH solution into the solutions obtained in Parts A and B. Consistent, accurate amounts of NaOH were hard to obtain, so a more effective drip method

The ring stand was set up along with a clamp to hold the temperature probe. A hot plate was placed underneath, leaving enough space between the two to fit a beaker. 50mL of 3M NaOH was poured into a 250ml beaker. After adding a stir bar, the beaker was placed on the hot plate. 3.750 grams of NaAIO2 was added to the beaker and the thermometer was then lowered in. Caution was used in making sure the thermometer did not touch the bottom of the beaker.

The hydrochloric acid had been sitting in room temperature for much longer then the water which came from the tap right before the trials. To control both of the liquids, 300 mL of each liquid should be poured into individual beakers around 24 hours before the experiment. If the two beakers are in the same temperature for 24 hours and have the same volume, then they will both have acutely similar temperatures, by the time of the experiment. If the temperature is controlled, the experiment and results can be much more

In class this year we investigated sodium reactions in three entirely different experiments. In the first of the experiments, our teacher drop sodium metal into a glass bucket of water and stood behind an extremely thick piece of plastic for protection. The sodium reacted as soon as the protective layer around the metal dissolved into the water and then the sodium exploded and caught fire, this created heat and light. This reaction made sodium hydroxide and hydrogen gas (NaHO and H). In the second of the experiments, we all split up into groups of around three or four and went over to our own separate benches for each group. We all then took turns to pick up the sodium with metal tongs and placing it in the blue part of the Bunsen burner flame

From one stable compound comes multiple products caused by the rearrangement of the reactant. If one were to do the calculations for the combustion reaction, the units would be in joules and negative, indicating it is an exothermic reaction. Such calculations are vital to maximize output and feed consumption.

This experiment is focused on heat of combustion using hydrocarbons as fuel. All three fuels produce combustion reactions which are exothermic. When bonds are formed or broken the most common form of energy released or taken in is heat energy. Heat of combustion is a way of measuring how much energy is output from a combustion reaction, the energy that is output is usually in the form of heat.

Reactions only occur when particle of the reactant collide with a certain minimum kinetic energy. This energy is also known as activation enthalpy this energy must be supplied to the reactant to enable the bonds to stretch and break and the new bonds to form in the product. Most collisions do not result in a reaction, only the collision with enough activation enthalpy will react to produce the product. (1)(2)

In Part A of the experiment, 100 mL of 6 M HCl was diluted with 200 mL of deionized water to make 2 M HCl. The acid was added to the water to ensure that flash-boiling did not occur. Next, 100 mL of 3 M NaOH was diluted with 50 mL deionized water to make 2 M NaOH. The base was added to the water to ensure that flash-boiling did not occur. The solutions were then cooled down to room temperature. The LabQuest was setup by plugging it in, plugging in the temperature probe to Channel 1, and changing the interval to 15 s/sample.

The objective of this experiment is to prove Hess’ Law, which states that the change in enthalpy for any chemical reaction depends on its products and reactants and it does not depend upon the pathway or the number of steps involved in the reaction between the reactant and product.

It is the heat energy released that we are concerned with, the amount released in this reaction will provide us with the calorific value for each fuel.

The hot plate was set on the base of the ring stand with both utility clamps attached to the ring stand. They were attached so that one was hanging over the hot plate, while the other clamp faced directly away from the hot plate. After the initial setup was done, a graduated cylinder was used to measure out 100.00ml of distilled water into a beaker. For the three non-control tests, glucose and table salt were added to the distilled water at this step. Before placing the beaker of solution onto the hotplate, 1.61 grams of

The stand, clamp mat and a 250mL conical flask were set up as demonstrated in figure 1. A burette was rinsed with 10 ml of 1.0M NaOH(aq), and made sure the end of the burette and the flask were about 5cm away. Checked the stopcock of the burette and made sure it was shut, then a funnel as used to fill the burette with 0.1M NaOH(aq) until the reading is between 0 and 1mL. This was recorded as initial value. A 20ml pipette was rinsed with 5mL of HCI, and then the 20mL of HCI was transferred to the conical flask using the pipette. 5 drops

500 mL of distilled water was measured and put to a beaker. 4.2 mL of concentrated HCl was added carefully and slowly to the beaker. The solution was stirred and then transferred into a labelled storage bottle.