specific heat experiment calorimeter

The amount of heat absorbed or released (q) by the object depends on its mass (m), specific heat (C s), and the change in temperature (ΔT). Specific heat can be defined as the amount of heat required (q) to raise the temperature of one gram of the substance by one degree Celsius.

One technique we can use to measure the amount of heat involved in a chemical or physical process is known as calorimetry. Calorimetry is used to measure amounts of heat transferred to or from a substance. To do so, the heat is exchanged with a calibrated object (calorimeter).

One technique we can use to measure the amount of heat involved in a chemical or physical process is known as calorimetry. Calorimetry is used to measure amounts of heat transferred to or from a substance. To do so, the heat is exchanged with a calibrated object (calorimeter).

Experiments show that thermal energy required to raise the temperature depends on its mass, specific heat capacity and the desired rise in temperature. In this experiment, you will learn to determine specific heat capacity of water using a calorimeter.

You will find the specific heat of a metal by equating the heat lost by the metal (at high temperature) to the heat gained by the water reservoir at a lower temperature when they are mixed in the calorimeter.

• Measure, calculate, and correctly use the terms heat, temperature, specific heat, reaction enthalpy, endothermic reaction, and exothermic reaction. • Understand the relationship between heat and specific heat capacity.

Heat and Specific Heat: The amount of heat required to raise the temperature of a solid body depends on its change in temperature (ΔT), its mass (m), and an intrinsic characteristic of the material forming the body called specific heat (c). The heat is calculated from the equation Q =cmΔT (8-1)

In this experiment, you will determine the specific heat capacities of two different unknown metals by observing the transfer of heat from a heated piece of metal to a sample of water at room temperature.

The specific heat test described in this article required many modifications and repetitions to display conclusive results. The results obtained were relatively accurate even taking into consideration the modification of using a calorimeter made of Styrofoam cups.

In this experiment, the amount of heat that is lost by a sample of metal as it cools is equal to the amount of heat gained by the water in the calorimeter. This assumes that no heat is lost from the calorimeter to its surroundings (the room), and that the amount of heat that is absorbed by the calorimeter itself is so small we can ignore it.