Specific Heat Of An Unknown Object

The aim of the experiment was to find out how changing the mass effects the rise of the temperature of water.

In this experiment, the results of the tested materials gave off heat and the change in the temperature was positive because when one substance was added to another the temperature increased. A calorimetric constant is required because the calorimeter that was made is different for every lab group.

In order to measure the heats of reactions, add the reactants into the calorimeter and measure the difference between the initial and final temperature. The temperature difference helps us calculate the heat released or absorbed by the reaction. The equation for calorimetry is q=mc(ΔT). ΔT is the temperature change, m is the mass, c is the specific heat capacity of the solution, and q is the heat transfer. Given that the experiment is operated under constant pressure in the lab, the temperature change is due to the enthalpy of the reaction, therefore the heat of the reaction can be calculated.

You have the mass of water from calculation #9, the specific heat of water is 4.184 J/g(oC), and the temperature change of water

13. Calculate the change in temperature for the water caused by the addition of the aluminum by subtracting the initial temperature of the water from the

1. Consider eight two-cubic centimeter (2 cm3) sugar cubes stacked so that they form a single 2 x 2 x 2 cube. How does the surface area of the single, large cube compare to the total surface area of the individual eight cubes? Report your answer as a ratio. Be sure to show all calculations leading to an answer.

Is it possible to find the specific heat of unknown metals using calorimetry? This experiment was designed to determine the specific heat capacity of two unknown metal sample. By comparing the data with the accepted heat capacities of various metals, the composition of the unknown samples was identified. Two unknown metals were put in boiling water for two minutes to ensure thermal equilibrium. The metal was then transferred into a calorimeter where the temperature was measured. The steps above were repeated for the second unknown metal as well. The cp , specific heat, of the metal was then calculated. Based off of the calculations, the obscure metal number one is zinc. This is on the account that the specific heat of the unknown metal was

This lab’s problem asked how the heat capacity of a lead sinker can be determined (Bridges 192). The hypothesis stated for the first experiment that if the lead sinker is heated in boiling water, placed in a calorimeter, and tracked consistently for the temperature, then the heat capacity of the lead sinker can be calculated because with the mass of the lead sinker, the original volume and mass of the water, and before and after temperature checks of the water, the data collected can be used with available formulas for heat capacity to find the heat capacity of the lead. This statement was not supported by the data for the first experiment because the margins of error were too great to affirm the hypothesis. Likewise, though there wasn’t a

In an article called “Heat Transfer by conduction” by Mike Brown, it states “Thermal energy in the vibrating particles or molecules is passed on to nearby particles in a process called conduction”. This explains to us the process of conduction in which it relates to our design because when we insert the thermometer into the warm water, our goal is to keep the water warm with our cup so that once the thermometer makes DIRECT contact with the warm water, it will heat up the thermometer and give us an exact temperature.

We did our experiment using popcorn and bread. First we measured the mass of the pieces of bread and popcorn and we weighed their mass. We added 10cm of water into a test tube, measured the temperature. We heat the water with the help of the fire that caught on the food substance and we measured the temperature at the end when the food had completely burnt out. To find the energy released we used the formula, energy released = mass of water (g)*temperature rise *4.2/ mass of food sample (g)

Showing that in order for the accepted value to be achieved even less heat needs to be lost to the spatial surroundings. Nevertheless the graphs showed that the newly constructed calorimeter efficiently achieve more than half of the accepted value by using 715 kJ/mol to burn through the alcohol but

Hypothesis: If the temperature of the chip rises, the temperature of the water above it will absorb some of the energy released by the endothermic reaction of the burning potato chip. Raw Data/ Results/ Observations: An increase in the mass of the potato chip resulted in an increase in temperature change, with the height of the water above the flame produced by the burning chip remaining constant. Although there was ½ gram more water in the second experiment, the

The following materials will be gathered, a Coke Can Calorimeter, graduated cylinder, thermometer, ring stand, balance, a long thin stick, paper clip, matches, a marshmallow, a CHEEZ-IT, a Chex-Mix, and Cheetos. A Coke Can Calorimeter with a stick through the tab will be placed on the ring stand. An unwound paper clip will be placed directly underneath the calorimeter on the base of the ring stand. Water and a thermometer will be placed inside the calorimeter. The sample will be placed on the paper clip, so that the sample will almost be touching the bottom of the calorimeter. A match will be lit, and then will be used to catch the bottom of the sample on fire. A close eye will be kept on the thermometer to see when the temperature reaches

In part A of the experiment we added 100 degree Celsius water to room temperature and tracked the temperature of the mixture to see how much it changed. Using this information we were able to calculate how much energy was given off by the how water and how much energy was absorbed by the cold water. The difference of the absolute values of these two values divided by the difference in temperature gave us the calorimeter constant. The calorimeter constant is an important value because it allow us to calculate how much energy is absorbed by the calorimeter in other reactions. Our calorimeter constant makes sense because it is a smaller value and with the colorimeter being Styrofoam, and insulator, the amount of heat absorbed by the calorimeter

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: