Enthalpy of formation of magnesium oxide lab report. To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law Essay Example for Free 2019-01-12

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Heat of formation of magnesium oxide Essay Example

enthalpy of formation of magnesium oxide lab report

Compound A substance made up of two or more different types of atoms that have been joined bonded together. Write a step-by-step procedure for the investigation. Swiss-born-Russian scientist, Germain Henri Hess had come up with the idea of calculating the enthalpy of reaction of a certain reaction using an alternate set of stepwise reactions which would add together in such a way that it would give the same reaction. Clean the piece of magnesium ribbon with sandpaper, then coil it loosely around a pencil. From the figure, the value for the maximum temperature reached can be safely estimated to be 40. The controlled variable is that the Magnesium used is possibly from the same ribbon and after being cut into lengths was stored in the same way in plastic containers. Butane can now be represented in empirical formula as C2H5.

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Magnesium Oxide Chemistry Report Essay Example for Free

enthalpy of formation of magnesium oxide lab report

Be careful around the bunsen burner, even when switched off — they may still be hot! This means that heat was being produced immediately and the lid was not on the calorimeter to keep the heat from escaping. Analytical balances have an absolute uncertainty of ±0. Parallax error We must keep our eye level the same as that of the liquid that we are measuring. Answer: Assumptions: 1 Assume that the hydrochloride acid solution has the same destiny and specific heat capacity as water 2 The amount heat released by the reaction are totally absorbed by the calorimeter. While performing all the experiments, it was made sure that only one person was in-charge of the stopwatch.

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Hess

enthalpy of formation of magnesium oxide lab report

Disposed the reaction of solution. The crucible containing the magnesium with the lid on was weighed. Random errors in this experiment were also quite large with the error due to uncertainty in the stopwatch only one being negligible enough. This indicates that increase in temperature leads to an increase in the reaction rate. Figure 2: Zoomed in view of the y-axis and horizontal line intersection. A lid was placed on top and through the hole, a thermometer was placed through it.

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Heat of Reaction for the Formation of Magnesium Oxide Lab Answers

enthalpy of formation of magnesium oxide lab report

Disposed the reaction of solution. So as the magnesium was being carried from the measuring area to the workstation or while it was sitting on the counter top or being poured in, it could have reacted with the oxygen in the atmosphere and combusted. Only after investments in a better calorimeter and an analytical balance have been made, should one think to invest in a 15cm3 pipette. We can use these masses to work out the formula of magnesium oxide. A gas is beginning to form, only a little bit.

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To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law.

enthalpy of formation of magnesium oxide lab report

In the total of 4 trials, 92 thermometer readings have been taken. The weights do not match possibly because the scales used in the experiment were not accurate to the right number of decimal places. The empirical formula is largely useful in determining the ratio of elements within ionic compounds where the structure is of a non-directional nature of bonding where any ion at any time could be surrounded by 4, 6, or 8 oppositely charged ions. Using the calorimeter one can then determine the rise and fall in temperature of the reaction. Hypothesis Based on the law of definite proportions it is hypothesized that the percentage composition of magnesium oxide will be 60. This indicates that increase in temperature leads to an increase in the reaction rate. Moreover, such high temperatures cannot be measured using a common thermocouple K-type so they need much more sophisticated setup of Ir-Rh thermocouples in an inert atmosphere.

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Heat of Reaction for the Formation of Magnesium Oxide Lab Answers

enthalpy of formation of magnesium oxide lab report

This was due to the production of MgO which is white in color and since it is insoluble in water, it turns water milky. The thermometer has some problem, which made the data not so accurate. In other words, if a chemical change takes place by several different routes, the overall enthalpy change is the same. Atomic Number The amount of protons found in the nucleus. Be careful not to inhale the magnesium oxide powder.

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Essay about Heat of formation of magnesium oxide

enthalpy of formation of magnesium oxide lab report

Ruler Different rulers have different systematic and random errors. Retort stand, ring clamp, clay triangle 5. Because the substances were transferred so quickly and taking into account the number of seconds that it took to replace the thermometer to begin recording data again it is possible that energy was either lost in the transfer or energy was lost before the recording was actually able to begin. Thermometer Different thermometers have different ranges and systematic and random errors. Once again, the change that would have occurred would have been minimal as it is difficult for large amounts of magnesium to react with oxygen in such a short amount of time without the use of a catalyst. This means that the heat produced if all 0.


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Hess

enthalpy of formation of magnesium oxide lab report

Magnesium Ribbon Safety: Done 1. Intuitively, lower the value for ΔT, lower the heat released by the reaction. Excess of distilled water To be used to wash the calorimeter before using it for the next trial. This indicated that in this reaction, Hydrogen gas was not produced. Although this does not completely stop heat from escaping it certainly decreases the amount that can escape. Setting up the calorimeter — Two Styrofoam coffee cups were taken and one was placed inside the other with a rubber band in between the cups to create an air gap. This was done using a calorimeter, which was calibrated by adding a known amount of both hot and cold water.


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