Cold Water Lab

It occurs when there is an absence of seed crystal or nucleus (nucleation points) for the formation of a crystal lattice structure by water molecules. It is found out that hot water would supercool lesser than cold water (i.e. hot water freezes at a higher temperature than cold water). Auerbach (1995) found out that that the most probable freezing temperature, Tf of hot water at 90oC was at 0oC - -2oC, with a probability of 0.41, Whereas Tf of cold water at 18oC was at -4oC to -6oC, with a probability of 0.56[3] However, the reason behind supercooling on the Mpemba Effect was not determined. In fact, theoretically, hot water should supercool less than cold water, due to the fact that hot water contains lesser amounts of dissolved gases than cold water as these gases were driven off in the process of heating the water.

THE MPEMBA EFFECT Erin Splaine Deerfield School Grade 8 Abstract The reason for this experiment was to find a faster way to freeze water by simply changing the temperature. The way this was accomplished was by heating an amount of water while leaving an equivalent amount at room temperature, then freezing both amounts of water and determining which freezes first. The heated water ended up freezing completely first, even though the cooler water started to freeze first. These findings tell us that even though something may seem impossible, you never know for sure until you try. The most interesting part about this experiment was that even though the boiled water froze faster, it also melted faster, not retaining the cold for as long as the

Beaker 2 cooled by 2.9°C (from 27.9°C to 25°C) and temperature in Beaker 1 fell by 1.9°C (from 29.9°C to 28°C). The cause of this result is the plastic wrap which did not allow the temperature to cool down quickly. In the second part of this experiment, greenhouse gasses were introduced to Beaker 1 by exhaled air. The exhaled air contained Carbon dioxide (CO2) and water vapor (H20). When Part II ended, one cardinal problem was noticed.

The ice which is going from solid to liquid, is absorbing the heat energy from the other ingredients/ice cream. In addition, the ice is sprinkled with rock salt, which lowers the freezing point of the ice. The freezing point being when a substance becomes solid. When the ice melts, even more heat is absorbed from the the ice cream mixture. All of the heat that the ice absorbs makes the ice melt, lowering the freezing point;meanwhile, the ice cream mixture is changing from a liquid phase to the more solid form, ice cream.

This effect was created by adding water to a beaker of dry ice. When water comes in contact with dry ice (which is actually pure carbon dioxide), it forms little carbon dioxide bubbles that rise up to the surface, creating the effect of fizzy soda. When it reaches the top, a reaction occurs between the carbon dioxide and the air which makes the water in the bubbles very cold and creates a thick fog. This is what makes the dense smoke that pours out of the dry ice beaker. We also learned that dry ice is very cold and can burn you, so it is important to handle them with gloves or tongs.

The effect of the temperature on the reaction time of human hand responding to a sight stimulus Design Research Question: How does the temperature affect the reaction time of human hand in responding to a sight stimulus? Hypothesis: Temperature is an important factor in regulating blood supply and nerve signals. Lower temperatures decrease the nerve signals from brain to hand, thereby slow the reaction (Ascroft). When the hand is submerged in cold water, the sensory receptor nerves in the skin recognize the fall in temperature and send signals to the hypothalamus. Then the hypothalamus sends signals that cause blood vessels to constrict in order to preserve heat.

In conclusion temperature change did affect one of the tubes in two very different ways whilst concentration also played a role in the change of the product and reactant. Le chatelier's principle states that through change in temperature, change in concentration and adding pressure you can create an equilibrium where there can be a forward reaction and a reverse reaction. By continuously adding and taking away heat and changing concentration we have created these reactions. When we took away the heat by putting it in the ice bath it would shift left while when we added heat to it would shift right. We saw this reaction take place as there was color change in tube 2 compared to tube 1.

Lastly the final product crystals were not washed with hot water because it would have melted the crystal thus cold water was used. The Hydrolysis reaction included an acidic environment and an acidic catalyst to make the reaction occur faster and initiate the reaction as well. The acidic environment is required in order to add the hydrogen and oxygen onto the carbonyl groups in the final product. Dicarboxylic acid is not very soluble in water/acetone which ultimately resulted in larger yield of product. 2.

We tried to minimize the effect of the heat loss by using chilled water instead of room temperature, although not much correction was done. Also, incomplete combustion (carbon monoxide and carbon are made instead of carbon dioxide) was a severe hindrance to the lab. The lack of lab resources and a changing environment were the main limitations to finding accurate values during the combustion

For an endothermic reaction, heat is absorbed in the reaction, and the value of ΔH is positive. For an exothermic reaction, the situation is just the opposite. Heat is released in the reaction, so heat is a product, and the value of ΔH is negative. If we picture heat as a reactant or a product, we can apply Le Chatelier's principle on raising or lowering concentrations. For instance, if we raise the temperature on an endothermic reaction, it is essentially like adding more reactant to the system, and therefore, by Le Chatelier's principle, the equilibrium will shift the right.

Purpose and Techniques: This experiment has the aim to determine a chemical formula of hydrated compound, which ingrains cupper, chloride and water molecules in its structure. In order to find this hydrated compound, it is necessary to use the law of multiple proportions. In other word, finding the appropriate variables values to this compound (CxCly*zH2O). Additionally, two major steps are required to proceed the experiment. The first consists to heat a sample to liberate the water hydration, and then compare two mass weights before and after heating so gets easier to find the water percentage (mass).

When the hot water was added it made it rise to the top of the container and spread. That showed us that the bottom layers would be hotter and the top layers would be colder. The asthenosphere is making convection currents. Since the convection currents are always moving it causes the asthenosphere to move and bend because it is ductile. When the asthenosphere moves which is under the tectonic plates it will cause an earthquake or more specifically the Alaskan Way

The purpose of this report is determine if sodium chloride is a viable option as a deicer on winter roads. To determine this, one must compare a multitude of factors. In this lab, the freezing point depression of water, enthalpy of dissolution, cost, and environmental impact will be discussed. A large factor in how effective a substance is as a deicer is it’s ability to decrease the freezing point of water. If the freezing point of water can be lowered, the outside temperature must be much colder to reach this new freezing point, resulting in less ice on the roads.

I think the difference in temperature can cause convection currents, because like the lava lamp the more hot something is the more dense it becomes then it rises to the top, the more cool something gets the less dense it becomes and it sinks to the bottom. So when plate tectonics go through a convergent boundary it slides under the crust it then has a current, which is caused from convection. Which then spreads. Then it heats up, and rises to the top. Once it 's at the top it cools down and becomes less dense then this process is repeated.

My main question is: At which temperature will children 's multivitamins dissolve the quickest when placed in water at different temperatures (0°C,50°C and 100°C)? My hypothesis for this question is that the children 's multivitamin will dissolve differently when placed under different water temperatures.I predict that the multivitamins will dissolve very fast when placed in the hot water ( in this experiment 100°C), and will dissolve very slowly when placed in the ice cold water (in this experiment, 0°C).My prediction is based on alot of things that are dissolvable.Dissolve more quicker in hot water than cold water as it has more concentration.