Lab 4 – Energy Sources and Alternative Energy Experiment 1: The Effects of Coal Mining |Table 1: pH of Water Samples | |Water Sample |Initial pH |Final pH (after 48 hours) | |Pyrite |6 |6 | |Activated Carbon |6 |7 | |Water |6 |6 | POST LAB QUESTIONS 1. Develop hypotheses predicting the effect of pyrite and coal (activated carbon) on the acidity of water? a. Pyrite hypothesis = The pyrite will probably dissolve a bit and increase the ph of the water b. Coal (activated carbon) hypothesis = The activated carbon will probably increase the ph of the water as it dissolves and releases chemicals into the water 2. Based on the results of your experiment, would you reject or accept each hypothesis that you produced in question 1?
Purpose What happens to the speed of a reaction between Calcium Carbonate (CaCO3 1M & 3M) and Hydrochloric acid (HCl) as the temperature is changed and the surface area of the reactant. HCl(aq) + CaCO3(s) → CaCl2(aq) + CO2(g) + H2O(l) is the reaction. Hypothesis Factors affecting the rate of Chemical reactions are varied. The “Rate of Reaction” means how fast is the reaction. In the collision theory reactions can happen when the reactant particles collide successfully but most collisions are not successful.
Lab 4 – Energy Sources and Alternative Energy Experiment 1: The Effects of Coal Mining |Water Sample |Initial pH |Final pH (24-48 hours) | |Pyrite |7 |4 | |Activated Carbon |7 |8 | |Water |7 |7 | POST LAB QUESTIONS Develop hypotheses predicting the effect of pyrite and coal on the acidity of water? Pyrite hypothesis = If the pyrite is left in a warm climate in water for 48 hrs, then it will have a higher pH then the initial Coal hypothesis = If the Coal is left in a warm climate in water for 48 hrs, then it will have a lower pH then the initial Based on the results of your experiment, would you reject or accept each hypothesis that you produced in question 1? Explain how you determined this. Pyrite hypothesis accept/reject = Reject. According to the pH balance strips, my pyrite recorded a significantly lower pH of 4.
The term Cp is the specific heat of the material (at constant atmospheric pressure). Different materials have different specific heat values. The units of specific heat are : Joules/gram deg – C. In this lab we will find the specific heat value of Zinc and compare it to accepted values.This will do by heating a mass of Zinc up to the temperature of boiling water and placing the hot metal into a cup of cold water. The thermal energy that the zinc loses goes into heating up the water in the cup. By knowing the starting temperatures and the final temperature of the water and the zinc, the specific heat of Zinc may be easily obtained.
Some scientist’s had this view in the past, which has now been refuted and replaced by more current thinking about how elements are arranged. I agree with Evie that the mass of magnesium goes up and my view is formed from the evidence presented by the results of the experiment carries out, the particle and brick models and findings of various scientists in this field. The mass of magnesium increases when it is burnt. The Magnesium reacts with the oxygen in the air to form the compound - magnesium oxide. The powder that remains will have lost some mass as smoke, but this resultant mass is still more than the mass of the metal that was burnt.
I thought distillation would remove the salt. The benzoic acid I wasn’t really sure about. B. If each step isn’t done correctly before moving on to the next step the percent for error rises. C. The sand recovery percentage being higher than the original sand percentage could take place if all the iron was not removed from the mixture.
Date : 18/02/2013 Micro-scale Determination of the Activation Energy of the Hydrogen Peroxide-Iodide Reaction Abstract: The purpose of this experiment was to determine the rate at which hydrogen peroxide decomposes to water and oxygen with the use of an iodide catalyst. Using the logarithmic form of the Arrhenius equation: ln k’ = -Ea/RT + ln A . the activation energy was determined to be 52.3 kJ/mol. It was also found that increasing the temperature also increased the rate, as there was more energy available to increase the speed of the reaction. Introduction: The purpose of this experiment was to determine the Activation Energy of the Hydrogen Peroxide-Iodide reaction.
The yield decreased with increasing temperature, due to increased enzyme deactivation at higher temperatures, while the initial reaction rate increased with increasing temperatures. Keywords: Enzymes; saccharification; steam-pretreatment; willow; hydrolysis; temperature Introduction The costs of raw material and enzymes are the two major cost components in the bioconversion of lignocellulosic material to ethanol. =In a previous study,2 the cost of enzymes were found to constitute about 80% of the total hydrolysis cost. It is thus necessary to optimize the enzymatic hydrolysis to obtain high yields at low enzyme consumption. In two previous studies, 3,4 steam pretreatment was shown to be a very
We are looking to find wether the reaction is exothermic or endothermic. Experiment 2: the aim for this experiment is to record the pH level of a sodium hydroxide and hydrochloric acid reaction. Then record it into the graph, it should resemble the standard neutralization curve, as shown under the introduction. Materials: what you will need for both experiments: Experiment 1: ➢ 20g baking soda ➢ 20g citric acid ➢ 2 cm strip of magnesium ➢ 50 ml of 5M HCl acid ➢ 50 ml measuring cylinder ➢
Abstract: The original purpose of this experiment was to combine Calcium Oxide and Water to attempt to replicate the self-heating can and record the temperatures achieved, however on commencement of the experiment it was discovered that there was an error with either the chemicals or the set-up procedure as no heat was generated. Instead, the experiment was slightly altered with new chemicals. The purpose of the new experiment was to experimentally determine the Specific Heat Capacity of Sodium hydroxide and also to determine which ratio of Sodium Hydroxide to Water will produce the most heat. It was hypothesised that the ideal concentration would be 7.5g of NaOH to 112.5g of H2O and that this reaction would reach between 50-60oC. The experiment was carried out by placing 112.5g of water into a large beaker and then adding the different amounts of NaOH and recording the heat given off.