Friday, September 27, 2019

Determine Specific heat capacity of water and metals Essay

Determine Specific heat capacity of water and metals - Essay Example During the experiment, precautionary measures were observed in order to prevent accidents by adhering to laboratory rules and regulations. While handling hot objects, direct contact was avoided and tongs were used to handle the metals. While transferring metals, splashing of hot water was prevented through gentle removal and dipping of the metal and thermometers in the beakers. To ensure that the metal cooled enough, running cold water on the metal surface and then dried. Measure the mass of the empty beaker record it, and then pour 500ml or 0.5 kg water into the beaker and measure the total mass. The mass of water is determened by subtracting the mass of the beaker from the total mass and recorded the mass (m). The table illustrates the data collected in the respective timeline during the experiment and recorded immediately. The data helps in drawing a chart that can be use to determine the value of R2 that is the line of best fit that is supposed to be 1. The chart is drawn from the data in Table 3 which will facilitate determining the closeness to the theoretical R2=1. From the chart the R2= 0.9913 which is very close to the optimum theoretical value. The equation of the trend line is y = 50.774x - 1266.6 that provides for a gradient of 50.774 and with a constant value of -1266.6. The specific heat capacity obtained for Water trial1 was (4076.25 J kg-1 â„Æ' -1) and trial2 (4080 J kg-1 â„Æ' -1). The specific heat capacity obtained for Aluminium was (890.37 J kg-1 â„Æ' -1) and that of Copper was (387.738 J kg-1 â„Æ' -1). Comparing these values with theoretical values, water, aluminium, copper are respectably (4185 J kg-1 â„Æ' -1), 897 (J kg-1 â„Æ' -1) and 385 (J kg-1 â„Æ' -1) (The Engineering Toolbox, n.d.), we can note a slight difference in the values. The values are not exactly the same as the theoretical values. The experimental error  is 2.25%. There are some explanations for this. Heat is lost to the surrounding during the transfer of

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