CHEMWORK Balance the following chemical equations using the smallest whole number coefficients. Note: You must enter all coefficients, even if the value of the coefficient is 1. For example: 2 H₂(g) + 1 O₂(g) → 2 H₂O(l) 2 2 2 2 2 NaOH(aq) + H₂SO4(aq) + CoBr3(aq) + Al(s) + MnO₂ (s) + 13 1 1 3 3 BaCl₂(aq) → NaOH(aq) → Pb(NO3)2(aq) → H₂SO4 (aq) → CO(g) → 1 8 2 2 1 Ba(OH)₂ (s) + H₂O(l) + Al2(SO4)3(aq) + Co(NO3)3(aq) + Mn₂O3(aq) + 3 1 1 10 NaCl(aq) Na₂SO4(aq) 3 H₂(g) CO₂(g) PbBr₂(s)
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.
![**CHEMWORK**
**Balance the following chemical equations using the smallest whole number coefficients.**
**Note:** You must enter all coefficients, even if the value of the coefficient is 1.
**For example:**
\[ 2 \, H_2(g) + 1 \, O_2(g) \rightarrow 2 \, H_2O(l) \]
1. \[ 2 \, \text{NaOH}(aq) + 1 \, \text{BaCl}_2(aq) \rightarrow 2 \, \text{Ba(OH)}_2(s) + 1 \, \text{NaCl}(aq) \]
2. \[ 2 \, \text{H}_2\text{SO}_4(aq) + 3 \, \text{NaOH}(aq) \rightarrow 2 \, \text{H}_2\text{O}(l) + 3 \, \text{Na}_2\text{SO}_4(aq) \]
3. \[ 2 \, \text{CoBr}_3(aq) + 3 \, \text{Pb(NO}_3)_2(aq) \rightarrow 1 \, \text{Co(NO}_3)_3(aq) + 3 \, \text{PbBr}_2(s) \]
4. \[ 2 \, \text{Al}(s) + 13 \, \text{H}_2\text{SO}_4(aq) \rightarrow 8 \, \text{Al}_2(\text{SO}_4)_3(aq) + 10 \, \text{H}_2(g) \]
5. \[ 2 \, \text{MnO}_2(s) + 1 \, \text{CO}(g) \rightarrow 1 \, \text{Mn}_2\text{O}_3(s) + 1 \, \text{CO}_2(g) \]
**Explanation of the diagrams:**
There are no graphical diagrams in the provided image, only text-based chemical equations to be balanced. Each equation is presented with the smallest whole number coefficients necessary to balance the number of atoms of each element on both sides of the equation. The image highlights the importance of using coefficients to ensure the law of conservation of mass is upheld in chemical reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9a2edb2f-7c78-40b5-b7fe-b2ef3d716529%2F283ce618-13fb-41cb-903c-78218830020e%2F4yo7lkd_processed.png&w=3840&q=75)
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