-We measured in each chemical and added water besides, HCl we added NaOH. Next, we measured the water temperature to begin with then added the substance to it to determine the finally temperature. We minus the initial and finally to decide if the reaction is exothermic and endothermic. 5. Describe the anticipated temperature change of a system in which an exothermic process is taking place.
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. What did the physicist Amonton contribute to the understanding of hot and cold? Amonton was doing heating, and cooling experiments. He saw that when he cooled the object that when the temp dropped so did the pressure. So he thought what would happen if you kept pushing the pressure back.
“Ice…Ice…Baby” “What is the quickest way to melt ice?” January 22, 2013 Abstract We choose to do this experiment in an attempt to discover what the quickest method for melting ice was. The purpose of this project was to find a way to melt the ice off the glass of a car windshield during the cold winter months. Our hypothesis was; if we added water to the ice it would melt quicker then adding either air or salt. The independent variable of the experiment was the molecular structure of the water found in the form of an ice cube. The dependent variable was the “amount” of time it took for all 3-ice cubes to melt.
Where did the heat the flow from (What happened to the temperature of the ice after salt was added?) 3. What is the minimum temperature that pure water can exist as a liquid at standard pressure? 4. What do you think would happen to the temperature of the ice if you added 6 tablespoons of salt instead of 2 tablespoons?
Abstract The focus of this experiment was to analyze the kinetics of a nucleophilic substitution. A mixture of 0.3622-M 1-bromopropane and 0.3622-M potassium hydroxide in an 90:10 ethanol/water solvent provided the reactants for a SN2 reaction to occur in a temperature controlled bath at 50.0˚C. The disappearing reactant was found by titrating timed aliquots during the reaction and then measuring the concentration of hydroxide. The k-value was found to be 0.0202 M-1Min-1. Using the linear form of the Arrhenius equation the activation energy was calculated to be 19.9 kcal/mol.
Describe the three freezing points. Is there a relationship between the amount of solute in the solution and the freezing temperature? Yes, the more solute the colder the temperature is B. What are some practical applications of freezing point depression? The longer the time, the colder it gets Data Table 4.
(4 points) q = m × c × Δt Given: q=? m = 34.720g c = 4.18 j/(g x °C) Δt = 41.6°C - 25.2°C = 16.4°C q = (34.720g) (4.18 j/(g x °C) (16.4°C) q = 2380.13j You are trying to figure out the energy change of the water which is the surroundings in the lab. To do that you must take the mass of the metal, which for me was Aluminum, and multiply it by the heat capacity of the water, which was given, then multiply that by the change in temperature, which is the final temperature of the mixture
Measure the time it takes to completely dissolve. Record time in data table. Cold Water: Fill beaker with 80mL if ice water. Use thermometer to record temperature of water. Record the temperature.
The purpose of this lab was to find the molecular weight of two unknown substances by analyzing the freezing points in cyclohexane and to provide a visual representation of the freezing point depression effect. The theory of this lab is; by using measurements of mass of the unknown substances (solute) in correlation with the mass of the cyclohexane (solvent) and the freezing point constant of the solvent, you could determine the molecular weight of the solute by using the same math involved in deciding the freezing point of the solution/ The theory behind the visual of the FPD effect is that if one was to record the freezing point of a solution and two solutions of the same substances with more solute, one would see a visible drop in freezing point. The equations you needed for this lab were the freezing point formula for organic substances (ΔFp=(m)Kf) and the
5. Record the data in a chart with the times. Experiment Basically the experiment is on what household items can insulate and hold the circulation of cold air inside the ice box which allows freezing points or melting points to take course. Data/ Graphs Ice Boxes | Test 1(none) | Test 2 (salt) | Test 3(Sugar) | Cardboard | 7:14.8 | 12:52.7 | 8:35.2 | Paper | 9:28.4 | 12:14.8 | 7:43.6 | Aluminum Foil | 16:35.1 | 17:21.6 | 13:17.8 | Time Graph Observations When I experimented I noticed that one of the ice boxes melted quickly than the others, which could mean that those ice boxes vents heat. The substance added to the ice box could have either helped it stay cool or melted it quicker.