Fill the burette with 0.005mol dm-3 potassium manganate(VII) solution. 6. Pour some of the thyme extract solution into a 250cm3 plastic beaker. 7. Using a measuring cylinder, add 50cm3 of 1.0mol dm-3 sulphuric(VI) acid to the thyme extract in the conical flask.
Find the volume of 2.40 mol of gas whose temperature is 50.0 °C and whose pressure is 202 kPa. 6. How many moles of gas are contained in a 50.0 L cylinder at a pressure of 10100 kPa and a temperature of 35.0 °C? 7. Determine the number of grams of carbon dioxide in a 450.6 mL tank at 1.80 atm and minus 50.5 °C.
7. How did Fahrenheit make thermometers smaller? Used mercury 9. What strange twist did Anders Celcius incorporate into his thermometers? He placed the his temperature scale at o degree for the boiling point, and ent downward and placed the freezing point at 100 degrees 10.
| 2.91V | 0.06A | 3. | 4.07V | 0.09A | 4. | 5.01V | 0.10A | 5. | 6.02V | 0.13A | 6. | 6.99V | 0.14A | 7.
The following mistakes were made when carrying out the experiment. What effect does each have on the calculated molar mass? Be specific. For example, too large because… Only part of the pipet was immersed in the boiling water, so the temperature in part of the pipet was less than that of the water bath. If the temperature was less than the water bath in some places because only part of the pipet was immersed in the boiling water, the molar mass calculated would become lower.
Questions: A. The Alkali and Alkaline Earth Metals in the main group elements. B. Sodium C. Color may look different to different people, slightly subjective. Another would be that some ions my produce the same flame color and not all may produce a flame color.
3. The fuels had a very strong scent when exposed by burning or opening the lid of the spirit lamp. QUANTITATIVE DATA: TABLE 1: Table of results showing the initial, final and average changes in mass of the alcohols after 100cm3 of distilled water was heated over a 10-minute period. Alkanol | MASS/g | | Trial 1 | Trial 2 | Average Change in Mass/g(±0.002g) | | Initial Mass/g (±0.001g) | Final Mass/g(±0.001g) | Change in Mass/g(±0.002g) | Initial Mass/g(±0.001g) | Final Mass/g(±0.001g) | Change in Mass/g(±0.002g) | | Methanol (A) | 211.196 | 206.740 | 4.456 | 206.740 | 202.336 | 4.404 | 4.430 | Ethanol (B) | 224.763 | 221.965 | 2.798 | 221.965 | 219.328 | 2.637 | 2.718 | Propanol (C) | 206.376 | 204.541 | 1.835 | 204.541 | 202.691 | 1.850 | 1.843 | But-1-ol (D) | 240.198 | 238.799 | 1.399 | 238.799 | 237.194 | 1.605 | 1.502 | Pentanol (E) | 216.526 | 215.132 | 1.394 | 215.132 | 213.642 | 1.490 | 1.442 | Hexanol (F) | 212.494 | 211.222 | 1.272 | 211.222 | 209.882 | 1.340 | 1.306 | Heptanol (G) | 207.233 |
4. Chlorine, Cl 2, is a strong oxidizing agent found in bleach. 10.0 cm3 of bleach solution was added to 25.0 cm3 of 0.4M Sn2+ solution acidified with sulphuric acid and made up to 100 cm3. 10.0 cm3 of the resulting solution containing the unreacted Sn2+ was titrated against 0.02M K2Cr2O7. Given that 11.40 cm3 of K2Cr2O7 was required for complete oxidation, a) Calculate the numbers of moles of Cr2O7- used.
Materials: 250mL Beaker Test Tube Calorimeter Burner, Ring Stand, and Wire Gauze Thermometer Balance Procedure: 1. Prepare an appropriate data table. 2. Fill the 250mL beaker about half full. Place it on the stand and begin heating it to the boiling point (100 degrees Celsius).
Isolation of Caffeine from Tea CHEM243A 2-23-11 Abstract: The purpose of this experiment was to isolate caffeine from a tea bag. Once isolated, the caffeine was purified using sublimation. The percent recovery was calculated to be 83.3%. The melting point of the original substance was 51ºC-139ºC. Since it was inaccurate, the melting point of another group’s sample was recorded.