Alcohol Combustion

The dependent variable in the experiment was the temperature and energy absorbed by the water.

I will measure these individual alcohols by mass which will be measured in grams, I'll be making two readings of each alcohol before the experiment and after, which would tell me the mass lost and how much heat is produced. Dependent Variable, the things that I'll be measuring would be the temperature (oC) increase at the start and the final resting point once combustion has been stopped of each different alcohol being lit to heat the water in the copper calorimeter, and the mass before and after the experiment of alcohols. Fixed Variables, the things that I have chosen to keep the same in each individual experiment to keep it a fair test, is to keep the same amount of water being heated, the same copper calorimeter, as it may vary in conductivity, the height of the calorimeter, and the same amount of time for each

9. The accepted value for the density of water is 1 g/mL and the accepted density for isopropyl alcohol is 0.786 g/mL. Determine the percent error between your calculated densities and the accepted values for both water and isopropyl alcohol. Record the percent error in Data Table 4.

Weight 10 dry post-82 pennies which get 52.31g, using 30ml initial volume measuring the volume of 10 pennies, record the data 7.0ml. Using equation Density= Mass/Volume, get the density of the pre-82 pennies is 7.47g/ml. Then calculate the error%=0.08%, and the deviation%=5.53%.

There were three different runs in order to have comparable data and to increase the validity of the experiment. The first run gave 39% of Sodium Bicarbonate. The second run gave 34% of Sodium Bicarbonate while the third one gave 39%, which is the same as the first run. The average percentage was 37% which is much lower than the manufacturer's percentage of 59%. The percent error came out to be -37%.

A scale conversion is calculated and the measurements from each thermometer are examined to see how closely correlated they are. _M___

8. Analyze: How does the standard deviation relate to the consistency and range of a data set?

There are only 25 numbers in the sample collected. For purposes of analysis, it will be considered that the process itself is normally distributed, and its standard deviation is unknown. Under these conditions, the formula that gives the confidence interval is:

Volume of water This was kept constant by using a 200 ml beaker to fill up the jars used in the experiment. The uncertainty of the volume of the water was: +/- 10 ml

Therefore, a theoretical uncertainty value that accommodates both uncertainties of the measurement and the equipment is calculated. The theoretical uncertainty calculation is primarily based on the propagation of error formula. The theoretical uncertainty calculation is as follows.

The room temperature was measured throughout the lab and kept constant at 24°C (+/- 1°C), as the lab was conducted during the same time of

Even though the result of an experiment is accurate and matches the literature value, it does not mean that there were no mistakes made. As the difference of the percentage uncertainty and the percentage error suggests there were random errors made. First of them was the heat energy lost to the surrounding environment during the experiment process taking place. This caused the recorded highest temperature to be smaller than the actual highest temperature that was meant to reach. This could have been prevented by adding in more and perfect

The aim of this experiment was to test the heat of combustion over a period of time, and the energy required to combust alcohols with different carbon chain levels. It was hypothesised that the higher the carbon chain of the alcohol present, the faster the heat of combustion will occur. Meaning more energy will be released for a higher carbon chain. After calculating the results from the experiment it was found that the hypothesis was partially supported. The reasoning for this is as the alcohol that posses a higher carbon chain, generally increased there reaction rates. However there were a few exceptions to this rule.

To achieve this, the final value from each thermocouple was set to be equal to the warm water bath temperature (370C), and the initial reading was set equal to the ice water bath temperature. Thus, for each thermocouple an equation was obtained using the two points to convert voltage readings to temperature. An example of the calibration for one of the thermocouples is shown in Appendix II.

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