# Heat of formation of magnesium oxide. Magnesium oxide 2022-10-27

Heat of formation of magnesium oxide Rating: 6,5/10 1422 reviews

Heat of formation, also known as enthalpy of formation, is the measure of the amount of heat energy required to form a compound from its element(s) under standard conditions. The heat of formation of a compound can be either positive or negative, depending on whether the compound absorbs or releases heat during its formation.

The heat of formation of magnesium oxide (MgO) is a positive value, indicating that the compound absorbs heat when it is formed. MgO is an ionic compound formed from the elements magnesium and oxygen, and it is commonly used as a refractory material due to its high melting point and good thermal stability.

To calculate the heat of formation of MgO, we can use the following equation:

ΔHf[MgO] = ΣΔHf[products] - ΣΔHf[reactants]

In this equation, ΔHf represents the heat of formation, and the terms on the right side represent the sum of the heat of formation values for the products and reactants, respectively.

The heat of formation of an element in its standard state is defined as zero, so we can substitute the heat of formation values for the reactants and products from a reliable reference. Using data from the NIST Chemistry WebBook, the heat of formation of MgO can be calculated as follows:

ΔHf[MgO] = ΔHf[O2(g)] + ΔHf[Mg(s)] - ΔHf[Mg(s)] - ΔHf[O2(g)]

ΔHf[MgO] = -602.8 kJ/mol

This value represents the heat of formation of MgO under standard conditions (25°C and 1 atm). It tells us that the formation of one mole of MgO from its elements requires the absorption of 602.8 kJ of heat energy.

In conclusion, the heat of formation of MgO is a positive value that reflects the heat energy required to form the compound from its elements under standard conditions. This value is important in understanding the thermodynamics of chemical reactions involving MgO and can be used to predict the direction and extent of such reactions.

## Heat Of Formation Of Magnesium Oxide Report Example 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. Third, the change of temperature is the property that needs to be measured. Using the calorimeter one can then determine the rise and fall in temperature of the reaction. Consequently, the heat value, or Q, would have been lower which also would have lead to a lower enthalpy value, like the one that was found. Retrieved 26 September 2011. 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. However to determine the proper equation for ΔHT, the stoichiometric equations must first be balanced: Therefore the heat formation of MgO was determined to be -618.

Next

## Magnesium Oxide Report Guidelines Using molar masses of both magnesium and oxygen, an expected percent composition, by mass, was found and compared to our experimental results. For the experiment to be preformed accurately the magnesium would have had to react with only oxygen and no magnesium should have been lost in the process of it being heated, however this was not the case. We then recorded the mass m of room temperature water and ice water each in a respective cup and then poured the ice water into the room temperature water and recorded the temperature change. One possible source of error could be not reading the measurement on the thermometer accurately. In other words, if a chemical change takes place by several different routes, the overall enthalpy change is the same, regardless of the route by which the chemical change occurs provided the initial and final condition are the same. When a chemical reaction occurs in an open container most of the energy gained or lost is in the form of heat.

Next

## Heat Formation for Magnesium complianceportal.american.edu I would expect that any error that might have occurred happened during the transference from one cup to another. As you continue, Magnesium Oxide Heat Lab 4. To determine the accuracy of the calculation we can determine the % error: As far as accuracy goes a percent error of 2. Since both reactions are in dilute water solutions of HCl it was necessary to know the heat capacity of water, but because some heat would be transferred to the calorimeter whose heat capacity was unknown, we had to record a correction factor x based upon the specific heat of water using the The Enthalpy of Formation of Magnesium Carbonate Magnesium Carbonate, MgCO3, is a white solid that occurs naturally as a mineral, as has a variety uses. Therefore, the average temperature high for the Mg and HCl solution in trial 2 was 44.

Next

## [Solved] Finding the enthalpy of formation of magnesium The change in enthalpy of this reaction is quite difficult to measure directly by experiment. In the future the procedure should emphasize the importance of measuring and pouring the magnesium after the HCl has been measured and poured into the calorimeter, this would prevent other reactions from occurring. In this experiment, a coffee cup calorimeter was used. Experimental report A coffee cup calorimeter was assembled. IEEE Transactions on Magnetics.

Next

## Heat of Formation of Magnesium Oxide (2).docx To prevent even the slightest anomalies, in the future any holes on the calorimeter can be covered by tape or another item that could block the passage. However, this would explain the small error in this experiment as the discrepancies were not that high. Using the calorimeter one can then determine the rise and fall in temperature of the reaction. Magnesium burns so bright because the reaction releases a lot of heat. Results Times Temp Mg oC Temp MgO oC 0 22 20 30 23 21 60 24 21 90 23 21 120 22.

Next

## Heat Formation of Magnesium Oxide Data All mass readings are given in units of grams g , and all temperature readings are given in degrees Celsius °C. Heat flows between the system and surroundings until the two are at the same temperature, when a chemical reaction occurs in which the system absorbs heat, the process is endothermic it feels cold. Almost no work is done i. Once again, the loss of heat would have resulted in a lower enthalpy value. When a chemical reaction occurs in which the system produces heat it is exothermic it feels hot … Determining Best Calorimeter Experiment Background: Calorimetry is the science of measuring the heat of chemical reactions or physical changes. In particular, 2O 3 ca.

Next

## Heat of Reaction for the Formation of Magnesium Oxide Lab Answers A gas is beginning to form, only a little bit. Magnesium Oxide Heat Lab — Best Lab Report 2022 Posted on April 21, 2022 This article provides a sample lab procedure and report on Permalink: Magnesium Oxide Heat Lab Report Objective To determine the heat formation of MgO Magnesium Oxide using Introduction Chemical reactions require heat energy to complete, called an endothermic reaction, or produce heat energy, and thus called an exothermic reaction. A calorimeter is a device used to determine the specific heat of chemical reaction or a physical change. To determine the accuracy of the calculation we can determine the % error: As far as accuracy goes a percent error of 2. The crucible was then weighed and the mass recorded. Second, we mixed the solutions a number of times using different ratios of reactants. From this lab it can be concluded that the law of definite proportion stating that the elements in a pure compound combine in definite proportion to each other is factual.

Next

## Heat of formation of magnesium oxide This error would only be specific to the magnesium as the magnesium oxide has already reacted with oxygen and no further reaction would occur. Methods As per lab manual we used a calibrated calorimeter using a rounded end thermometer so as to not puncture a hole in the calorimeter to determine the heats of reaction for Magnesium Mg with Hydrochloric Acid HCl and Hydrochloric Acid with Magnesium Oxide MgO. We then recorded the mass m of room temperature water and ice water each in a respective cup and then poured the ice water into the room temperature water and recorded the temperature change. Conclusion In this lab we were able to determine the heat of formation of MgO using a simply constructed calorimeter, which was found to be -618. HCl was poured into the coffee cup with the Mg. Therefore, the average temperature high for the MgO and HCl solution in trial 2 was 29. Both of these conditions would have lead to a lower final temperature value.

Next