The experimenter used 3 identical plastic cups and filled one with room temperature tap water, one with warm tap water and one with boiling tap water. Each cup was placed into the freezer and was checked every 15 minutes for signs of freezing. The experimenter found that the room temperature water showed the first signs of freezing and in the final outcome froze solid before the water in the other cups. His findings showed that water containing impurities, such as tap water, will freeze faster based on a lower starting temperature. The second case study was covered in an article by Science News.
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?
If contact was liquefied gas thaw the frozen parts with lukewarm water. If it was a burn cool infected area with cold water but do not remove clothing adhering to the skin. 1005- Ammonia; toxic and corrosive gas. Isolate any spill at least 100 meters in all directions. first aide move victim to fresh air, administer o2, DO NOT use
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.
Some might think that by squeezing the bottle, Mr. Squiddy would go up with the water however, he would go down due to the pipette being used. The pipette had a little air bubble at the top of it, when the bottle was squeezed the water filled into the pipette creating an increase in pressure and a subsequently decrease in volume causing Mr. Squiddy to sink. When released, the high pressure subsided and he floated back up. In the crushing cans demo the cans were heated up with a little water inside and set to boil until steam appeared. Once the can was hot enough it was quickly placed in a bowl of ice cold water and the can crushed itself.
Answer = The weather would be calm in decreased temperatures because you don’t see condensation or evaporation happening when the temperature is cooler. The weather would produce more condensation and more evaporation if the temperatures increased. I think this because let’s say you have a cold can of soda. When you take it out of the refrigerator it’s cold. After a few minutes you start to see the condensation forming on the outside of the can as the can’s temperature changes because it’s no longer in the refrigerator.
Experiment Colligative Properties & Osmotic Pressure Karen Curry 1/19/2014 1:00pm Abstract The purpose of this experiment is to understand and compare the difference of the freezing points between pure solvents in a solution and a non-volatile solute. Secondly, osmosis is demonstrated in a permeable membrane in this case a dialysis tubing and a less permeable membrane with a much harder shell like the egg. Experiment and Observation Starting with Part I of this experiment I gathered together all my items I needed. Small rubber band, salt, tap water, distilled water, 1/8 teaspoon measuring spoon, crushed ice, beaker 100 mL plastic, stopwatch-digital, test tube 13 x 100 mm, digital thermometer, well plate-24. First I made a water bath by filling the 100 mL beaker with cool tap water.
NCSU – Dept. of Chemistry – Lecture Demonstrations Gas Law / IMF Collapsing Metal Can (Boyle’s Law) Description: A metal can is crushed when immersed in cold water. Materials: Empty soda can Ice water Procedure: Add 15 mL of water to aluminum can and bring to a vigorous boil. Quickly invert the can and submerge it into the beaker filled with ice. At this point the can will collapse.
What is the pressure that is used to put the carbon dioxide into the bottle in the first place? The bottle manufacturers design the bottle to hold about 20 atmospheres of pressure before they burst. Some other things to experiment with: How would results of this experiment change if you used a very cold soda? Could you measure the pH of the soda before and after you de-fizzed it? How would you expect it to