20. Aluminum metal reacts with oxygen gas to form aluminum oxide, according to this equation: 4 Al(s) + 3 0,(g) → 2 Al,0,(s) How many grams of aluminum oxide will result from the reaction of 384 grams of oxygen gas? a. 12.0 grams Al,03 b. 8.00 grams Al,03 c. 816 grams Al,03 d. 1224 grams Al.Q.
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.
![**Chemical Reactions: Understanding the Formation of Aluminum Oxide**
**Problem Statement:**
When aluminum metal reacts with oxygen gas, aluminum oxide is formed according to the following chemical equation:
\[ 4 \text{Al}(s) + 3 \text{O}_2(g) \rightarrow 2 \text{Al}_2\text{O}_3(s) \]
**Question:**
How many grams of aluminum oxide will result from the reaction of 384 grams of oxygen gas?
**Options:**
a. 12.0 grams \(\text{Al}_2\text{O}_3\)
b. 8.00 grams \(\text{Al}_2\text{O}_3\)
c. 816 grams \(\text{Al}_2\text{O}_3\)
d. 1224 grams \(\text{Al}_2\text{O}_3\)
In this question, we need to determine the mass of aluminum oxide produced when 384 grams of oxygen gas reacts fully. The stoichiometric coefficients in the balanced chemical equation are used to find the molar relationship between reactants and products. This involves calculations based on the molar masses of aluminum, oxygen, and aluminum oxide.
Understanding chemical equations and stoichiometry is essential to solve such problems, as it allows for the quantitative analysis of reactants and products in a chemical reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7345e8e6-7416-43d6-9fee-55115ecf20af%2F2ebac559-fbc6-4535-9233-f683137cd455%2Fisq9w1aj_processed.jpeg&w=3840&q=75)
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