Specific heat

program of your choice or print this page. Instructions: This is a two-part lab. Be sure to follow all steps given in the lab and complete all sections of the lab report before submitting to your instructor. Procedure: Part I: Determining the Specific Heat of a Known Metal 1. Place a plastic measuring trough on top of the digital balance, and press the "tare/on" button so that the mass of the trough will be "ignored." The digital balance should read "0.000 g" after this step. 2. Measure out

performed on the 24th of September 2015 1. Design Research question: What is the specific heat capacity of 100g brass mass, as measured by the method of mixtures using water in a polystyrene cup? Hypothesis: If I insert a 100g brass mass into a 100 degrees boiling water for two minutes and transfer it to cold water then the cold water’s temperature will increase because the 100g brass mass gained heat from the boiling water. Data: Use the results in your data table to calculate the average

Molar Heat of Combustion Aim: To find the molar heat of combustion for four different alkanols: 1. Methanol 2. Ethanol 3. 1-Propanol 4. 1-Butanol - And to compare the experimental value with the theoretical. Background: The Molar Heat of Combustion of a substance is the heat liberated when 1 mole of the substance undergoes complete combustion with oxygen at standard atmospheric pressure, with the final products being carbon dioxide gas and liquid water. (Ref. “Conquering Chemistry, Roland

located at the bottom of the kettle (Chris Woodford 2014). By plugging in the kettle into an electrical outlet an electric current is able to flow into the heating element. As the element has a certain resistance it converts the electrical energy into heat, heating the cold water surrounding the element. The higher the temperature, the faster the atom is (Chris Woodford 2014). Therefore, the faster atoms from the element collide with the slower atoms of

respiration. If breathing is difficult, give oxygen. Get medical attention if symptoms appear. 1.23 4 – Methyl – 2 – Pentanol Chemical Properties Odour: N/A Colour: N/A Molecular Weight: 102.18 g/mol pH: 7 Neutral Boiling Point: 131.8°C Specific Gravity: 0.81 g/ml (water =1) Solubility:

CALORIMETRY Gloria Adepiti Jordan Winter Amanda Candace CHM 2046L 07/07/2015 Introduction The process at which heat and energy is transferred from one area to another at a constant pressure is known as enthalpy, a key factor to this experiment. The experiment calorimetry is used to measure the changes in thermodynamic quantities using a device known as a calorimeter. But this experiment was done using two different types of calorimeter a Styrofoam (also known as a coffee cup) and a

geothermal, waste heat, low-pressure steam, and it contributes significant energy conservation. Ecofriendly working fluid leads to reduce the global warming and ozone layer depletion. The following reason is also growing the research interest of the system. It is suitable for small to very large capacity. Operating cost is too less when compared with other commercial technology, and it is required very less electrical energy to operate the pump. Less maintenance cost because of heat exchangers and there

energy.   Planning We will be using 6 different fuels to heat up 100ml of water, and find out the changes of the temperature. We will measure the temperatures of the water before and after the experiment. We will burn heat the water for exactly 2 minutes, and check the changes in temperature. The change in temperature will allow us to work out the energy given off the fuel by using this formula:   Mass of water x 4.2 (water’s specific heat capacity) x temperature change = energy transferred from

1. Figure 1 shows the heating phases that occurred during the experiment. There is an exponential decrease in temperature as the depth of the water increases. Water has a high specific heat capacity which means that it can resist changes in temperature. This is coupled with the fact that solar radiation progressively loses its penetrative ability as the depth of the water increases. The light attenuation in lakes describes the decrease in actual light that can penetrate a water column as well as

recorded; the change in temperature (∆T) was calculated by subtracting the initial temperature from the final temperature. The reaction was performed twice for every calorimeter. The heat capacity (Ccal) of each calorimeter was calculated using the formula, C_cal=(-〖∆H〗_rxn^o n_LR)/∆T [1] where ∆Horxn is the total heat