Answer question 3 2. Use Hess's Law to calculate the heat of reaction for Equation 1. Hint: See your answer inPreLab Question #2. Show Calculation3. The heat of reaction for Equation 1 is equal to the heat of formation of solid magnesiumoxide.a. Look up the heat of formation of magnesium oxide in your textbook or a chemicalreference source.b. Calculate the percent error in your experimental determination of the heat of reactionfor Equation 1. Show Calculation • Heat of reaction• Heat of formation• Hess's Law• CalorimetrygroundMagnesium reacts with oxygen in air to form magnesium oxide, according to Equation 1.Mg(s) + ½0,lg)- MgO(s) + heatEquation 1As mentioned above, a great deal of heat and light are produced-the temperature of theflame can reach as high as 2400 °C. The amount of heat energy produced in this reactioncannot be measured directly in the high school lab. It is possible, however, to determine theamount of heat produced by an indirect method, using Hess's Law.The heat or enthalpy change for a chemical reaction is called the heat of reaction (AH).The enthalpy change-defined as the difference in enthalpy between the products andreactants-is equal to the amount of heat transferred at constant pressure and does notdepend on how the transformation occurs. This definition of enthalpy makes it possible todetermine the heats of reaction for reactions that cannot be measured directly. According toHess's Law, if the same overall reaction is achieved in a series of steps, rather than in onestep, the enthalpy change for the overall reaction is equal to the sum of the enthalpychanges for each step in the reaction series. There are two basic rules for calculating theenthalpy change for a reaction using Hess's Law.Equations can be "multiplied" by multiplying each stoichiometric coefficient in the bal-anced chemical equation by the same factor. The heat of reaction (AH) is proportional tothe amount of reactant. Thus, if an equation is multiplied by a factor of two to increasethe number of moles of product produced, then the heat of reaction must also be multi-plied by a factor of two.

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Answer question 3 2. Use Hess's Law to calculate the heat of reaction for Equation 1. Hint: See your answer inPreLab Question #2. Show Calculation3. The heat of reaction for Equation 1 is equal to the heat of formation of solid magnesiumoxide.a. Look up the heat of formation of magnesium oxide in your textbook or a chemicalreference source.b. Calculate the percent error in your experimental determination of the heat of reactionfor Equation 1. Show Calculation • Heat of reaction• Heat of formation• Hess's Law• CalorimetrygroundMagnesium reacts with oxygen in air to form magnesium oxide, according to Equation 1.Mg(s) + ½0,lg)- MgO(s) + heatEquation 1As mentioned above, a great deal of heat and light are produced-the temperature of theflame can reach as high as 2400 °C. The amount of heat energy produced in this reactioncannot be measured directly in the high school lab. It is possible, however, to determine theamount of heat produced by an indirect method, using Hess's Law.The heat or enthalpy change for a chemical reaction is called the heat of reaction (AH).The enthalpy change-defined as the difference in enthalpy between the products andreactants-is equal to the amount of heat transferred at constant pressure and does notdepend on how the transformation occurs. This definition of enthalpy makes it possible todetermine the heats of reaction for reactions that cannot be measured directly. According toHess's Law, if the same overall reaction is achieved in a series of steps, rather than in onestep, the enthalpy change for the overall reaction is equal to the sum of the enthalpychanges for each step in the reaction series. There are two basic rules for calculating theenthalpy change for a reaction using Hess's Law.Equations can be &#34;multiplied&#34; by multiplying each stoichiometric coefficient in the bal-anced chemical equation by the same factor. The heat of reaction (AH) is proportional tothe amount of reactant. Thus, if an equation is multiplied by a factor of two to increasethe number of moles of product produced, then the heat of reaction must also be multi-plied by a factor of two.

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