Chemical Reaction Lab

After the twenty minutes elapsed, the flask was cooled to room temperature and then titrated with the remaining NaOH until the colorless solution remained pink. The final volume was then recorded. While solution #1 was heating the same process was repeated with solution#2 and the second burette

The cooling time caused error when calculating the moles of water because the actual result was seven moles instead of five moles which was what was calculated. The calculations could have been potentially miscalculated particularly due to the significant figures used in the data. The method for this experiment can be improved by maybe using another object rather than the crucible to allow a faster cooling time that way the calculations for the analysis have less of a chance of

The Purpose of this experiment is to make the observation about a Chemical system and record exactly what was seen, paying attention to details. Then to design other experiments that will allow determination of which substances that are responsible for each of either the change in temperature, production of a precipitate , production of gas, distinct odor, and color change. Pre-Lab questions : There are 4 chemicals involved in this reaction. Name Them.

The amount of tablets did effect the temperature of the water. Our findings made our hypothesis incorrect. The temperature of the water did increase as the number of the tablets increased also. In this experiment, the finding were quite surprising, simply because I thought that the temperature of the water will decrease as the amount of the number of tablets increased. In the real world I feel like this information would be beneficial, because it shows the reaction of an acid plus a base mixed with water.

Record in data table 1. Calculate the average heat (q) by averaging trials 1 and 2. Record in data table 1.

Doing this would improve the accuracy of the results. 3. Build up of soot on base of beaker. The build up of soot on the base of the beaker could have potentially hindered the amount of heat energy transferred to the water in the beaker, thus reducing the accuracy of the experiment.

Another error was that we did not measure the temperature of the water while it was boiling for the first trial. We used the boiling point of water, 100℃. Another possible error was that when measuring the temperature of the water in the calorimeter for the first trial, the thermometer was touching the bottom of the calorimeter instead of just the water. The lab procedure could have said to make sure that the thermometer touches

For our experiment, we first filled three beakers up with water in different temperatures, such as; warm, room temperature, and ice. We then added three drops of red dye and placed one stick of celery in each beaker with water and red dye. We then waited 10 minutes, took the temperature again, which showed change and then we waited 10 more minutes. After

Experiment/Result/Analysis: In activity 17.8.1, we related volume and temperature, we had a empty beaker with air and a temperature probe in it, sealed with a rubber stopper that was connected to a syringe. We placed the beaker in cold water with a immersion heater and recorded the data on LoggerPro. As the water heated up, we observed that the pressure of the air remained constant because the temperature is also changing. We fit our data with a linear curve and concluded that the change in volume is directly proportional to the change in temperature.

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.

I thought that most of my results were very accurate. However there were a number of points out of place that I could improve on. On the '250ml experiment ' the reading between six and eight minutes appeared to be incorrect compared with the average heat loss in the same experiment. This could have been

Temperature: I can’t control the room or water temperature of the area studied. This may influence the amount of dissolved oxygen in water. However, as the measure are done at the same time I expect the temperature to be similar.

The change in the solution depends on the chemical being added. [1] “ For a exothermic reaction the  increase in temperature will cause the reverse reaction to occur. This causes a decreasing amount of the products and increases the amounts of reactants. Lowering the temperature will produce the opposite response.” As seen in the results, when the mixture was heated it produced less product.

During the experiment, the samples are placed in the water bath. The water tank has a large volume and it is an open system. The temperature of the water inside is difficult to keep constant. That makes the reaction in the sample cannot perform well at a suitable temperature, which is the body temperature. As there is a difference in the temperature, the reaction completeness in each sample may not be the same. The products formed may not be completed. That means there are some reactants were at complex form. This affects the result of the experiment. We cannot have an accurate measure of each sample. Thus, the accuracy of the experiment is not good enough.

• The water must then be heated to 70oC (the first temperature for the experiment)