John Denker Search this site: The following were written mainly to answer questions that came up on Phys-L, the Forum for Physics Educators.
From the table results we know that: The procedure was good and the mix of reactants was intimate, so we can say that the experiment were suitable. The first reaction CaCO was a very slow reaction.
Therefore, when reading the temperature we had to check it constantly and pick up the biggest value. The second one CaO was a very fast reaction, so when reading the temperature, we had to choose the first biggest value, because after that that point the temperature will decrease and the results will be anomalous.
This will lead to 0. Our results were within this value. Limitations in the experimental procedures: Because of the changing character of the temperature we might have got an anomalous result. So, because of the changing of the temperature values during the experiment we might get anomalous results.
Hence, we can say that the experiments were not very reliable, especially because of the temperature which is very hard to be measured accurately, but also because of the heat lost during the experiment. When mixing the reactants a considerable amount of heat was evolved as both of the reactions are exothermic.
To improve this, we should measure the heat evolved during the two experiments and maybe try to measure the temperature more accurately, so that the errors and anomalous results will be minimized or even canceled out.
The carbonates of calcium are not normally decomposed. This requires high temperatures and produces carbon dioxide and leaves a calcium oxide. Thermal decomposition takes place when carbonates of calcium are heated in special heat resistant test-tube and break down to give carbon dioxide and calcium oxide.
The experiment shows that the rate of reaction increases at higher temperatures. When a dilute acid as hydrochloric acid is added to powdered calcium carbonate, carbon dioxide is evolved.
Since the carbon dioxide escapes from the reaction environments, the whole reaction losses mass. A high temperature is needed to make the left-to-right reaction take place.
Reactants have less energy than products so heat is absorbed. The reaction does not start until energy is initially supplied.Chemistry Ia Enthalpy Change of Neutralisation Essay.
To calculate the enthalpy change of neutrallzatlon of the given pairs of acid and base - Chemistry Ia Enthalpy Change of Neutralisation Essay introduction.
Theory: When alkali neutralizes an acid, a salt and water are formed. By measuring this heat transfer in a constant pressurized environment, the enthalpy of the reaction can be used to Infer certain Information about a specific reactions reactants and products. The transfer of heat from outside sources In would be described as an endothermic reaction.
After learning about Aerobic and Anaerobic Respiration, revise the topic and test yourself to affirm your knowledge.
Since, ∆H = H final – H initial, the enthalpy change for a chemical reaction is given by the enthalpy of the products minus the enthalpy of the reactants: ∆H = H products – H reactants Typically, we can determine the magnitude of the heat flow produces.
The measurement of heat flow is calorimetry, and the device used to measure heat. In this lesson, you will learn about the different kinds of energy and how these types of energy can be transformed from one form to another.
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