b. Once again, place assembly in water bath and begin to heat c. When acetamide has begun to melt, record the temperature. d. Let assembly cool down and record temperature when acetamide begins to recrystallize. e. Repeat process two more times. Data: Data Table 1 | | | Rubbing Alcohol Trial # | Boiling Point | Percent Error | 1 | 79.5 C | 3.52% | 2 | 84.0 C | 1.90% | 3 | 83.5 C | 1.30% | Data Table 2 | | | | Acetamide Trial # | Melting Point | Freezing Point | Percent Error (Melting Point) | 1 | 79.5 C | 57.5 C | 3.50% | 2 | 80.5 C | 59.5 C | 0.60% | 3 | 78.0 C | 61.0 C | 3.70% | Observations: It was observed that thermometer placement could affect the readings in the water bath.
: V (6.0) Pressure ((4.18) *Raised back up to 398.: V (6.0) Pressure (5.51) -Temp. : 349 V (6) P (4.85) -Temp 145 V (6) P (2 point 06) -361 V 6 P 4. 9 -528 P 7.29 -102 P 1.45 -318 P 4.38 -565 P 7.86 -188 P 2.58 -460 P 6.35 -77 P 1.09 IDEAL GAS LAW 1) What is the relationship between pressure and temperature at constant volume? At a constant volume, as the temperature increases, the pressure also increases. 2) Using this data, predict at what temperature the pressure will exceed 10 units If the pressure is 10.1 units, the temperature would be around 732 ° .
a. decreasing the temperature b. changing the concentration of A c. changing the concentration of B d. changing the concentration of C e. letting the reaction go on for a long time 4. The gas phase reaction A + B C has a reaction rate which is experimentally observed to follow the relationship rate = k[A]2[B]. If the concentration of A is tripled and the concentration of B is doubled, the reaction rate would be increased by a factor of ____. a. 6 b.
(Divide the mass of the liquid calculated above by the volume of the liquid.) Trial 1: 10.5 / 8.7 = 1.21 Trial 2: 11 / 8.5 = 1.29 Trial 3: 11.4 / 8.8 = 1.30 Part II: Density of Irregular-Shaped Solid Calculate the volume of the irregular-shaped solid for each trial. (Subtract the volume of the water from the total volume of the water and solid.) Trial 1: 50.7 - 50.2 = .5 Trial 2: 50.7 - 50.2 = .5 Trial 3: 50.5 - 50.1 = .4 Calculate the density of the irregular-shaped solid for each trial. (Divide the mass of the solid by the volume of the solid calculated above.)
20. mol H2 reacts with 8.0 mol O2 to produce H2O. Determine the number of grams reactant in excess and number of grams H2O produced. Identify the limiting reactant. 8.1 g H2 , 2.9 x 102 g H2O 17. How many litres of O2 gas are required to produce 100. g Al2O3?
The new pressure in a closed container if a 5.0L volume of gas at 2.5atm has its volume increased to 7.5L. b. The new volume of gas (at constant T and P) if 2.0mol of He in a 3.0L container has another 3.0mol of He placed into the container. Answers: a. (5.0L)(2.5atm) = (7.5L)(P2) P2 = 1.7atm b.
Part E – Deriving a solubility curve Aim: To be able to calculate the solubility of the compound in a certain amount of water as the temperature increases or decreases. Hypothesis: As the water increases, the solubility decreases and the substance’ saturation would get lower. And as the volume increases, the substance won’t separate to the water anymore which makes it dissolved forever without getting crystallized when the water cools down. Apparatus & Method: [refer to the sheet p. 64] Result: Temperature | Volume [ml] | Solubility [g/100g] | 65 ̊ C | 5 ml | 130.44 g | 46 ̊ C | 8 ml | 81.525 g | 39 ̊ C | 11 ml | 59.29 g | 28 ̊ C | 14 ml | 46.586 g | 22 ̊ C | 17 ml | 38.36 g | 16 ̊ C | 20 ml | 32.61 g | 12 ̊ C | 23 ml | 28.35 g | 12 ̊ C | 26 ml | 25.08 g | The solubility was calculated with the formula of: Solubility=6.522gml of waterx 100 The solubility of Potassium Nitrate is directly affected by the temperature of the solution. As the temperature of the solution rises, the solubility of Potassium Nitrate increases.
Bring the contents of the distillation flask to a gentle reflux (i.e., vapors are condensing in the first ¼ to 1/3 of the vertical condenser and dripping constantly back into the flask below). Maintain this reflux for 10 minutes, then increase the heat in order to distill the liquid into the collection flask, then the column, and even the distillation head with aluminum foil (shiny side IN). Continue distillation of the cyclohexene product until the volume in the distillation flask is reduced to about 1 mL. Ask the instructor to assist you in removing the heat source and sand bath for the almost empty flask; use Ove Gloves and/or clamps to avoid burns. |
This initiation was evident by cloudiness and graying of solution as well as the evolution of bubbles off the surface of the metal. The flask became warmer anddid not need additional heat because of the exothermic nature of the reaction. The remaining bromobenzene solution was added dropwise at a rate that kept the contents in the flask gently boiling. Asthe magnesium disintegrated, the contents turned from gray to dark brown to brownish red and finally
How many moles of hydrogen gas can be produced when 10.0 g of Zn react with excess HCl? (Hint: you must write a balanced chemical reaction first.) 2. If the pressure is 1.2 atm and the temperature is 20.0ºC, what volume of hydrogen is produced in prelab question #1? 3.