The calorimeter exists as a fixed unit, thus its heat capacity is a fixed value. The amount of water in the calorimeter, however, can vary, and thus the heat capacity of the water can vary. When dealing with variable amounts of material, one often prefers to use an intensive measure of the heat capacity.
The Heat Capacity represents the change in temperature in the sample for a given amount of heat. The SI Unit of Heat Capacity is joule per kelvin (JK-1). Specific Heat Capacity represents the amount of heat needed to raise the temperature of a unit mass of a substance by 1°C. The SI units of Specific Heat Capacity are J kg−1K−1 and J/kg°C.
The temperature increase is measured and, along with the known heat capacity of the calorimeter, is used to calculate the energy produced by the reaction. Bomb calorimeters require calibration to determine the heat capacity of the calorimeter and ensure accurate results.
The thermal value of such a calorimeter is the heat capacity of the calorimetric system. The determination of the unknown calorific value or other reaction of the chemical thermodynamics Q is reduced to measure the temperature change Δ t of the calorimetric system caused by the process under study: Q = c Δt. Typically, the Q value refers to.
The heat capacity of the bomb calorimeter can be estimated by considering the calorimeter to be composed of 450 g water and 750 g stainless steel. Knowing the specific heat capacity of water to be 1 cal/g·K and estimating the specific heat capacity of steel to be 0.1 cal/g·K yields. 4. B. Measuring C v
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