'Cooling Drinks\r'

'1) What is the special potential heat up of confederacy of irrigate?Specific latent heat of unification is the count of heat absorbed or released by a substance when ever-changing states. This could be boiling or passing. latent heat of fusion is the sum of brawn needed to track down a substance, tour latent heat of vaporisation is the sum of get-up-and-go needed to boil a substance. The particular latent heat of fusion of weewee supply supply is 334 j/g In the graph, you can see that as the temperature increases much than skill is needed to heat the piss. When the temperature hits the latent heat of fusion, the temperature stops rising as the vital force is being used to neuter the state of wet. This also happens when the latent heat of vaporisation2) What is the detail heat capacity of weewee?The specific heat capacity is the inwardness of heat that is needed to raise the temperature of a substance. The specific heat capacity water is 4181 j/kg. This i s higher than most metals. present be some other substances with their specific heat capacity; SubstanceC (J/g oC) occupation 1.01 Aluminium 0.902 Copper 0.385 Gold 0.129 fight 0.450 Mercury 0.140 Sodium Chloride 0.864 Ice 2.03 water 4.183) Why energy is needed to melt shabu and how this is apologizeed by the structures of ice and water The molecules of H20 be rent differently in water than in ice. In water they are floating around freely and in ice they are â€Å"stationary”, they l ane(prenominal) vibrate slowly. This is because they don’t wipe out enough energy to break their intermolecular bonds. So in order to melt ice you need to add energy to give the molecules kinetic energy to run into around, becoming less stationary. If enough energy is given to the molecules they break the intermolecular bonds and the ice melts to ice. 4) Why is ice more than effectual for cooling a inebriation than nipping water The cooling of a drink with a cube of ice is mo re effective than victimisation cold water because ice can absorbs a part more heat. This is because it has a higher specific latent heat of fusion.HypothesisThe greater the issue forth of ice that melts the bigger the temperature fall away of the water This is because when more ice melts more energy is taken from the waterApparatus5 identical beakers which are do of the same materials Thermometers with a suitable crease; -10oC to 100oC Measuring with volume above 200cm3 Top-pan residuum reading with up to 35g Ice (crushed), not straight form the freezer qualified insulating material Means of removing water e.g. newsprint towels Stopwatch to mea certain time in minutes and secondsMethod1) Pour 200cm3 of water into 4 same sized beakers of the same materials. This is so the materials does not affect the in temperature 2) I’m going to heartbeat the temperature of the water. I’m going to make sure the temperature is the same to make it a fairish test. I’m going to ensue the water to become room temperature for some 5 minutes 3) I’m going to add 15g of ice to Beaker 1, 25g to Beaker 2, 25g to Beaker 3 and the fourth Beaker totallyow for aim no ice.The fourth beaker will set the benchmarks. The list of ice is the independent variable. I will measure the ices freshet by using the top-pan balance. I used these certain amount of mass so I have a big range of data and will make a part comparison. 4) I will then measure the temperature of the beakers every minute for three minutes. 5) thusly I will regorge all my results into a table and then into a line graph so I can make easy comparisons Hazards, the risks and how to sign on the risksResults Table1. Describe both patterns or arcs in your results. Comment on any unexpected results. After analysing my result I have found some trends in the data. I also saw some anomalies that came up in the experiment. The most obvious trend is in the line graph and the temperature d rop. The more mass of ice I put into the beaker to cool the drink, the faster the temperature dropped. For example, in beaker one 2. Compare results of your own investigation ( subtract 2) with the data from other groups within your class and any data collected in resolve 1. Comment on any similarities and differences.Suggest and explain assertable reasons for any differences. 3. Evaluate your results, the method acting you used and how well you managed the risks. 4. Do your results from Part 2 support the hypothesis suggested by Charlie’s friend? Explain your answer. 5. It is possible to use the equations below to predict the temperature drop of the water when a chosen amount of ice is added to it. Will the actual temperature drop, measured in your experiment, be equal to the predicted take to be? Use relevant scientific explanations in your answer. Use the results of your experiment, appropriate calculations and your research (Part 1) to bequeath evidence to support your answer. 1 cm3 of water has a mass of 1 gEnergy = mass à specific heat capacity à temperature shift Energy = mass à specific latent heat\r\n'