The Effect Of Heat And Calorimeter On The Heat Capacity

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.

14. Calculate the change in the metal’s temperature by subtracting the initial temperature of the iron from the final

2. How did concentration and/or volume differences affect the heat change (q) for each trial?

To improve the experiment, the methodology could be improved by having an efficient calorimeter to retain as much heat as possible, rather than just a tin can. Additionally, more trials for each of the experiments could be conducted to ensure correct and precise data is collected to determine more accurate conclusions.

There are four basic components for thermal energy (heat): 1. All matter is made up of tiny particles called atoms. These can only be seen with special microscopes. 2. The atoms are always moving – they all have kinetic energy. 3. The particles have space between them. Different states of matter have different amounts of space. 4. Adding heat (energy) to matter makes the particles move more quickly. Since faster moving things have more kinetic energy, adding heat increases the energy of the particle. 5. Cooling it down decreases the amount of kinetic energy and slows the movement down.

The amount of heat gained can be found by multiplying the (mass)(specific heat of water)(change in temperature). This follows the rule of Conservation Of Energy, that states energy can be neither created nor destroyed. Using this we are able to see that the amount of energy absorbed by the water is also equal to the amount released by the food in the

However, the calculated value of specific heat, i.e. 12.91 j/g0C, was relatively larger than expected due to some possible sources of errors. One of the possible sources of error in the experiment was possible loss of heat through the hole where the thermometer was initially inserted. In addition, heat loss may have occurred when the metal was transferred from the heated beaker to the calorimeter. To reduce these errors, the experiment should be conducted in a more controlled

To provide more information, the heat capacity formula is specific heat capacity times mass => C = m * c Heat can be transferred between different objects and one way to calculate it is: q = m*c*ΔT or C*ΔT. We use this formula to answer some questions about the metal that we have worked with in the lab. In the lab we used an isolated system, which is called calorimeter that measures the difference of temperature during a chemical reaction (Retrieved from lecture notes).

Q_c (1) where Q_h is the heat lost by the hot fluid and Q_c

When the fuels are burnt, energy is given off. I will be calculating the energy given off using the formula above. The specific heat capacity is the energy

Heat is a form of energy that is transferred between two substances at different temperatures. The flow of the energy is from the object of higher temperature to the object of lower temperature. The heat is measured in units of energy, usually calories or joules. Temperature on the other hand, is how cold or hot an object is. The temperature is the average kinetic energy per molecule of a substance. This is measured in degrees on the Celsius or Fahrenheit or in Kelvins.

Changes in heat capacity affect people in everyday life, from everyday activities like the amount of time it takes to cook to the construction of a bridge. Heat capacities are usually measured and tabulated in a different form of conditions for a multiple number of examples. Knowing the stage or property of the heat, (solid, liquid or vapor) of the substance during pressure, temperature and common desire composition is an important tool to remember before figuring up its heat. Heat capacity could be determined by the capacity of the temperature of an object multiplied by the mass as well as the chemical composition, temperature, and pressure of a substance (Science.com)

He later established the general theory of specific heats by observing the amount of heat required to raise the temperature of different substances by the same temperature interval.

Here, u signifies the temperature of the entire body and ∝ signifies the thermal diffusivity. Furthermore, the differential heat equation above must respect the following boundary conditions: