The calorimeter was designed in 1780 by a chemist named Antoine Lavoisier with help from a mathematician by the name of Pierre Simon de Laplace. Now a widespread tool, we will be using the calorimeter, and our knowledge of equations to find the specific heat of zinc and aluminum. OBJECTIVE/GOAL In this experiment we will Measure the mass and temperature of water in a calorimeter Heat a metal sample of a known mass to a specific temperature Calculate the change in water temperature caused by adding the hot metal sample Calculate the specific heat of the metal using your mass and temperature data PROCEDURE 1. Prepare a data table as directed in the Analysis. Safety goggles and lab apron must be worn for the experiment.
Dr Khounsary explains an experiment using a fixed voltage and varying the temperature of the wire using a torch. The article further explains that the temperature coefficient of copper at 20 degrees C is .00393 and that a single degree of temperature change would increase the resistance of the wire by that amount. In the article regarding the Effect of Temperature on Conductivity (The Nuffield Foundation, 2006) the article describes how the conductivity of a wire decreases as it is heated. It provides an example schematic diagram for the test circuit and the use of Eureka wire instead of copper wire. A2a.
It is useful at predicting reactant and product quantities through a reaction. There is enthalpy, Hess’s Law and is related to thermodynamics. It is applied in the real world by adding ice to water, burning fuel for a vehicle, and when power plants pump water into their machinery to keep them cool and not overheat. 2.In an insulated container, you mix 200g of water at 80°C with 100g of water at 20°C. After mixing, the temperature of the water is 60°C.
Below is a table showing the elements that make up the wall. Elements | Thickness (m) | Thermal Conductivity (W/mk) | Resistance (m²k/w) | Rsi | - | - | 0.123 | Plaster | 0.012 | 0.16 | 0.075 | Block | 0.100 | 0.19 | 0.526 | Insulation | 0.150 | 0.035 | 4.286 | Brick | 0.100 | 0.84 | 0.119 | Rso | - | - | 0.055 | TOTAL | | | 5.184 | Resistance is calculated through (Thickness divided by Thermal Conductivity) Once we have the total resistance (rate of heat released) we can work out the U-value using the following formula: 1 U-value = Rt 1 = 5.184 = 0.19 w/m²k Now that I have calculated the U-value, I can calculate the amount of heat loss through the following: = Area x U-value x Temperature Difference = 150 x 0.19 x 14 = 399w Therefore as shown above the total amount of heat loss through 150m² of cavity wall is 399w. 2. Sound Calculation If the intensity of a sound is measured at 0.04w/m², calculate the resultant decibel level (dB)! I dB = 10 log ( I ) where I = 1 x 10¹² 0.04 dB = 10 log ( 1x10¹² ) dB = 10 log ( 4x10¹º ) dB = 106 3.
The term Cp is the specific heat of the material (at constant atmospheric pressure). Different materials have different specific heat values. The units of specific heat are : Joules/gram deg – C. In this lab we will find the specific heat value of Zinc and compare it to accepted values.This will do by heating a mass of Zinc up to the temperature of boiling water and placing the hot metal into a cup of cold water. The thermal energy that the zinc loses goes into heating up the water in the cup. By knowing the starting temperatures and the final temperature of the water and the zinc, the specific heat of Zinc may be easily obtained.
In our 2nd, we examined the effect of warmer temperature. Our research question was, ‘does catalase denature in stages or all at once as temperature increases?’ Our hypothesis was: if temperature increases, then the catalase will denature in stages as the temperature increase, the catalase will slowly stop working. We followed the procedures in the lab manual (choinski and karatit 2014) with the following expetions: For experiment 1, we used 1.5% hydrogen peroxide concentration and experimented this concentration at 4*c, 24*c (room temp. ), 44*c, 52*c and 60*c. For experiment 2, we used 3% hydrogen peroxide concentration and experiment this concentration at 21*c (room temp. ), 35*c, 45*c, 55*c, & 60*c. Figure 1: Effect of temperature on catalase activity.
Based on the Bayle’s Law, the pressure of the gas is inversely proportional to the volume with fixed temperature. Conclusion: Our experimental result shows the slope of our graph of Inverse Volume versus Pressure is 2330 + 15Kpa*ml. We used the slope divided by (R*T), then we are able to find value of n which is n=9.50*10^-4. Our graph is a linear line, which means the product of pressure and volume is a constant (value of slope). Thus we are able to find that the pressure of gas is inversely proportional to the volume with fixed temperature.
Design Lab-Chemistry HL Date; 27th February and 1st March 2013 Grade 11 Increasing the temperature to increase the rate of reaction between sulfuric acid and iron powder Experiment; To investigate the effect of temperature of reactants on the rate of reaction Focus Question; How does temperature (30, 35,40,45,50 degrees Celsius) affect the rate of reaction of H2SO4 (1.0M, Volume; 20ml) and Fe (2.5g) in 6 minutes? Fe (s) + H2SO4(l) FeSO4(l) + H2(g) Variables; Independent Variable- Temperature Dependent Variable- how much hydrogen gas is produced Controlled Variable-Sulfuric Acid (1.0M, Volume; 20ml), Iron powder (2.5g), and time (6 minutes) Materials; 3 100ml Flasks 1 cork 1 tube 1 100ml graduated cylinder 1 25ml graduated cylinder 1 clamp stand 1 spatula 1 apron A pair of gloves 1 dropper 1 tub of water 1 waterbath 1 balance scale Stopwatch 3 pieces of paper 2 thermometers 37.5 grams of Iron Powder (Fe) 300 ml of 1.0M H2SO4 Procedure; 1. Wear an apron, gloves and goggles for safety reasons 2. Obtain all materials which are 3 100ml flasks, 1 cork, 1 tube, 1 100ml graduated cylinder, 1 25ml graduated cylinder, 1 clamp stand, 1 spatula, 1 dropper, 1 tub of water, 1 waterbath, 1 balance scale, 1 stopwatch, 2 thermometer to your work place 3. Then obtain 37.5 grams of iron powder, and 300 ml of 1.0M H2SO4 to your work place 4.
The moles of KNO3 s/ Kg solvent were needed to calculate the correct molal concentration. Another goal or purpose of this experiment was to calculate the heat of solution of each of the different concentrations. The inverse temperature and a linear plot of the molal concentration were needed to calculate this. The linear equation needed to calculate this was In(s)= -( H/ 2R)(1/T)+(1/2) where R is a constant and T was the temperature. The linear regression model could also be use to approximate the heat of solution.
IB Internal Assessment Objective: Investigate the Effect of Temperature on the rate of Digestion of Gelatine by Trypsin OBJECTIVE OF THE INTERNAL ASSESSMENT Research Question How will temperature affect the rate of digestion of gelatine by a 2% trypsin solution? Variables * The Dependent Variable is the time taken (seconds) for gelatine to digest. * The Independent Variable is the temperature (°C) we use to heat up the water bath for the solution. * The Controlled Variables are the size of the silver-acetate film pieces (1.5 x 1.0 cm), the volume of the 2% trypsin solution (3cm³), and the thermometers used to measure the temperature of the water in the tinc cans as well as the temperature of the 2% trypsin solution in the test tubes (the same thermometer was used at all times). RAW DATA AND OBSERVATIONS Initial observations 1.