3. The heat of reaction for Equation 1 is equal to the heat of formation of solid magnesium oxide. a. Look up the heat of formation of magnesium oxide in your textbook or a chemical reference source. b. Calculate the percent error in your experimental determination of the heat of reaction for Equation 1. Show Calculation
3. The heat of reaction for Equation 1 is equal to the heat of formation of solid magnesium oxide. a. Look up the heat of formation of magnesium oxide in your textbook or a chemical reference source. b. Calculate the percent error in your experimental determination of the heat of reaction for Equation 1. Show Calculation
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Answer question 3
Transcribed Image Text:3. The heat of reaction for Equation 1 is equal to the heat of formation of solid magnesium
oxide.
a. Look up the heat of formation of magnesium oxide in your textbook or a chemical
reference source.
b. Calculate the percent error in your experimental determination of the heat of reaction
for Equation 1. Show Calculation
Transcribed Image Text:• Hess's Law
• Calorimetry
Background
Magnesium reacts with oxygen in air to form magnesium oxide, according to Equation 1.
Mg(s) + 20,(g)
→ MgO(s) + heat
Equation 1
As mentioned above, a great deal of heat and light are produced-the temperature of the
flame can reach as high as 2400 °C. The amount of heat energy produced in this reaction
cannot be measured directly in the high school lab. It is possible, however, to determine the
amount 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 and
reactants-is equal to the am
depend on how the transformation occurs. This definition of enthalpy makes it possible to
determine the heats of reaction for reactions that cannot be measured directly. According to
Hess's Law, if the same overall reaction is achieved in a series of steps, rather than in one
step, the enthalpy change for the overall reaction is equal to the sum of the enthalpy
changes for each step in the reaction series. There are two basic rules for calculating the
enthalpy change for a reaction using Hess's Law.
unt of heat transferred at constant pressure and does not
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 to
the amount of reactant. Thus, if an equation is multiplied by a factor of two to increase
the number of moles of product produced, then the heat of reaction must also be multi-
plied by a factor of two.
Equations can be "subtracted" by reversing the reactants and products in the balanced
C
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