Question3: Experiment 3 The unknown acid sample was 1 • Monoprotic Acid Trails Initial NaOH solution (mL) final NaOH solution (mL) The volume of NaOH to titrate the acid (mL) Amount of Unknown Acid sample 1 (g) The moles of the Unknown Acid (mol) Molar mass of the Unknown Acid (g/mol) A 3.38 28.31 24.93 0.150 0.0026 57.69 B 0.18 29.32 29.14 0.175 0.0029
The control in the experiment is water. Units used while timing the productivity of gas from an Alka-Seltzer tablet in different temperatures is, seconds. In order to find out if temperature controls the rate of chemical reaction, whether hot water is a more effective way to make the gas produce at a faster speed, it would be necessary to compare the results of different temperatures at the end of each trial. In order to do this the scientists will measure the volume of gas that is produced within a 10 second interval time after the tablet begins to react.
The hypothesis made, the density calculated in the experiment will stay the same because the density of the unidentified object will never change, was supported. The results support the hypothesis because in every trial the density always came out to 9g/mL. In trial one the mass was 71.16g, the volume was 8mL, and the density was 8.895g/mL, but when rounded to the proper sig fig came out to 9g/mL. In trial two the mass was 71.12g, the volume was 8mL, and the density was 8.89g/mL, but when rounded to the proper sig fig came out to 9g/mL. In trial three the mass was 71.14g, the volume was 8mL, and the density was 8.8925g/mL, but when rounded to the proper sig fig came out to 9g/mL. When averaged the mass was 71.14g, the volume was 8mL, and the density was 9g/mL. Errors that could have occurred are, not calculating the density correctly, not completely submerging the unidentified object with water in the graduated cylinder to get the volume, not rounding the sig figs correctly when finding the density, not measuring the unidentified object’s mass in grams, not measuring the unidentified object’s volume in milliliters, and not writing the correct units with the proper number or not the correct unit at all.
The specific heat of three elements were tested zinc, copper, and lead. The experiments ran from Monday to Thursday and allowed a precise amount of heat to be determined. The experiment had multiple errors which were caused by random errors not systematically errors. In order to combat this, certain items were kept same. This was called a control.
On January 18, 2015, the New England Patriots and the Indianapolis Colts played in the AFC Championship game in a chilly temperature of 51°F. The Patriots were accused of cheating when, at half time, 11 of their 12 game balls were found to be two pounds psi less than the regulation size of 12.5 to 13.5 psi. Although the balls are gauged 2 hours and 15 minutes prior to the game, they are returned to the teams before the game started. Based on extensive research and data, the Patriots’ balls were tampered with prior to the game. Objects with gaseous interiors have a tendency to decrease in pressure when exposed to cold temperatures but the decrease will only be minor.
The first experiment was a Synthesis reaction, this was done by burning the substance magnesium; the substances reacted to form one compound, which ended up being heavier than the first original mass of the magnesium, the final product was known as magnesium oxide. The second experiment that was conducted was the Decomposition reaction, which actually eliminated chemical elements by burning them off, therefore reducing the weight of the final product by 1.673 grams. The third experiment was known as single displacement, by adding the chemical hydrochloric acid to zinc it created a chemical reaction which actually increased the temperature, as well as the pressure within the flask. The last experiment that was conducted was known as double displacement, this experiment involved the exchange of bonds, between the two sodium hydroxide and nickel. The Nickel was forced to group together when it was placed into the sodium hydroxide, instead of mixing with the compound it would rather keep to
Once the material was acquired, 1.0094 grams of Aluminum were weighed and then transferred to a 250mL beaker. The 250mL beaker continued to remain in use for the next few steps. 1.4M KOH solution was added to the Aluminum sample that was previously obtained. For gas to escape the lab, there was a fume
For this lab the knowledge to tell the difference between a chemical and physical changes was needed. To tell this the knowledge of the five signs of a chemical change was needed. These five signs are color change, odor change, production of bubbles/gas, production of heat/light, and the production of precipitate. Also prior to the lab one question was provided that needed to be answered. This question was what chemical must be present for a color change.
Eudiometer Experiments in Elemental Effervescent Expansions Joe Williamson and Ethan Kang Mar 13, 2023 Purpose: The purpose of the gas laws lab was to calculate the volume of gas produced from a specific mass of magnesium ribbon. It also aims to use gas laws to determine the theoretical yield and volume of hydrogen gas produced at STP. Procedure: Gather Mg ribbon, string, a 2000-mL beaker, a Eudiometer, a 100-mL beaker, 50-60 mL distilled water, and HCl.
There will be less magnesium to react and release energy so the enthalpy of combustion will be lower. (i) Another source of error is the uncertainties and imprecisions of the lab equipment. Because of the simple calorimetry apparatus used during the process, heat may have been lost to the surroundings which results in inaccuracies in temperature and mass measurements. In addition, another source of error results from the temperature probe’s use as a stirring rod. (j) % difference =
Interestingly enough, Boyle's gas law, Gay-Lussac's gas law, and Avogadro's gas law are connected in a way similar to how branches are connected to a tree. If the Ideal gas law can be considered the 'trunk' of the tree, then Boyle's, Gay- Lussac's , and Avogadro's gas laws are the 'branches'. To better understand this analogy, it is important to understand how each of the laws can be derived from the Ideal Gas Law. Gay-Lussac's law states that the pressure of an ideal gas is directly proportional to its temperature in kelvin, assuming that the amount of gas and the volume of the gas remain constant. The equation for Gay-Lassac's law would look something like: V = T k, where V is volume, T is temperature, and k is a constant.
To determine the rate of reaction there are many method to be used for example, measuring the mass after the product has been added and measuring the difference in mass on the duration of a digital scale. Another method, which will be used in this experiment is using a gas syringe to measure the volume of the gas which has been produced. The cylinder inside, will be pushed out to show a quantitative presentation of the volume produced by the reaction. Hypothesis
IV. Data and observations Mass of beaker (g) 174.01 Mass of beaker + NaOH pellets (g) 174.54 Mass of NaOH pellets 0.53 TRIAL 1 TRIAL 2 Mass of potassium acid phtalate (KHP) (g) 0.15 0.15 final buret reading (ml) 30.75
℃^(-1)×6.40℃±3.1 %=1337.6 J±4.06 % ∆H=(-1337.6 J±4.06 %) /(0.025 mol ±0.16 %)= -53504 J m〖ol〗^(-1)±4.22 % ∆H=-53504 J m〖ol〗^(-1)±4.22 %÷1000=-54 kJ m〖ol〗^(-1)±4.22 % Conclusion and
The graph shows the average volume of hydrogen that was produced from the 3 trials and the average volume of oxygen that was produced from the 3 trials across the voltage. I added the volumes of hydrogen in each trial and I divided them by 3 to get the average and I made the same thing for the volume of oxygen. The graph shows that the volume of hydrogen produced during the experiment is twice as much as the volume of oxygen. For example using the third data when I used 11 volts the average volume of hydrogen that was produced was 5.8 cm3 and the average volume of oxygen produced was 2.9 cm3
