● tab Starting with the following equation, MgCl₂(aq) + Na3PO4(aq) → Mg3(PO4)2 (s) + NaCl(aq) calculate the moles of MgCl₂ that will be required to produce 635 grams of Mg3(PO4)2. esc aps lock 1 F1 Missing: 635 | Must include: 635 Q 9,841 X . 2 ☀ F2 W A S #3 80 F3 E 23 D $ 4 a F4 R stv % 5 F भ F5 T MacBook Air < 6 A G r: F6 Y & 7 80 H F7 MA U 8 DII F8 J + 1
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.
![### Calculating Moles of MgCl₂
**Problem Statement:**
Starting with the following equation,
MgCl₂(aq) + Na₃PO₄(aq) → Mg₃(PO₄)₂(s) + NaCl(aq)
Calculate the moles of MgCl₂ that will be required to produce 635 grams of Mg₃(PO₄)₂.
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In this problem, you need to use stoichiometry to determine the number of moles of magnesium chloride (MgCl₂) needed to produce a specific amount of magnesium phosphate (Mg₃(PO₄)₂). This involves the following steps:
1. **Balanced Chemical Equation:** Confirm the balanced chemical equation.
MgCl₂(aq) + Na₃PO₄(aq) → Mg₃(PO₄)₂(s) + NaCl(aq)
(Ensure the equation is balanced. If necessary, balance it by ensuring the same number of each type of atom on both sides of the equation.)
2. **Calculate Molar Masses:** Calculate the molar masses of the relevant reactants and products.
- Molar mass of MgCl₂:
\[ \text{Mg} = 24.31 \, \text{g/mol} \]
\[ \text{Cl} = 35.45 \, \text{g/mol} \]
\[ \text{MgCl}_2 = 24.31 + 2(35.45) = 95.21 \, \text{g/mol} \]
- Molar mass of Mg₃(PO₄)₂:
\[ \text{Mg} = 24.31 \, \text{g/mol} \]
\[ \text{P} = 30.97 \, \text{g/mol} \]
\[ \text{O} = 16.00 \, \text{g/mol} \]
\[ \text{Mg}_3(\text{PO}_4)_2 = 3(24.31) + 2(30.97 + 4(16.00)) = 262.86 \, \text{g/mol} \]
3. **Determine Moles of Mg₃(PO₄)₂:**
\[
\text{M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F57980898-f1ea-4baf-a646-fad54b56b73d%2F6251a5e5-c90a-4047-bc5f-9e48e9146df7%2Fai5i8dt_processed.jpeg&w=3840&q=75)
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