CuSO (aq) + ZnCrO (aq) 2K (s) + Cl₂(g) → 2K C1 (s) - NaCl(aq) + AgNO3(aq) reaction KOH(aq) + HClO4(aq) → KClO4(aq) + H,O(1) - ZnSO4 (aq) + Cu Cro(s) NaNO3(aq) + AgCl (s) type of reaction (check all that apply) combination O precipitatio O single replacement O combustion double replacement acid-base 00010 decomposition combination O single replacement double replacement decomposition O combination O single replacement double replacement decomposition O combination O precipitatio O combustion acid-base O precipitatio O combustion O acid-base O precipitatio single replacement O combustion double replacement O acid-base decomposition
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 Reaction Types
#### Reaction Table
This table categorizes various chemical reactions by their type. Each reaction is defined with chemical formulas for both reactants and products.
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**Reaction 1:**
\[ \text{CuSO}_4\,(aq) + \text{ZnCrO}_4\,(aq) \rightarrow \text{ZnSO}_4\,(aq) + \text{CuCrO}_4\,(s) \]
- **Type of Reaction:**
- Combination
- Single Replacement
- **Double Replacement**
- Decomposition
- **Precipitation**
- Combustion
- Acid-Base
**Reaction 2:**
\[ 2\text{K}\,(s) + \text{Cl}_2\,(g) \rightarrow 2\text{KCl}\,(s) \]
- **Type of Reaction:**
- **Combination**
- Single Replacement
- Double Replacement
- Decomposition
- Precipitation
- Combustion
- Acid-Base
**Reaction 3:**
\[ \text{KOH}\,(aq) + \text{HClO}_4\,(aq) \rightarrow \text{KClO}_4\,(aq) + \text{H}_2\text{O}\,(l) \]
- **Type of Reaction:**
- Combination
- Single Replacement
- Double Replacement
- Decomposition
- Precipitation
- Combustion
- **Acid-Base**
**Reaction 4:**
\[ \text{NaCl}\,(aq) + \text{AgNO}_3\,(aq) \rightarrow \text{NaNO}_3\,(aq) + \text{AgCl}\,(s) \]
- **Type of Reaction:**
- Combination
- Single Replacement
- **Double Replacement**
- Decomposition
- **Precipitation**
- Combustion
- Acid-Base
---
**Key:**
- **Combination:** Two or more substances combine to form one product.
- **Single Replacement:** One element replaces another in a compound.
- **Double Replacement:** Exchange of ions between two compounds.
- **Decomposition:** One substance breaks down into two or more substances.
- **Precipitation:** Formation of](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9e783f66-b34a-45d9-ad0a-1bd44c44ca06%2Feb766c74-ee32-47d0-866e-918457d43019%2Fn25w1bd_processed.jpeg&w=3840&q=75)
a) Precipitation reaction:
In precipitation reaction an insoluble salt is formed by the reaction between 2 aqueous solution containing soluble salts.
b) Double displacement reaction
In double displacement reaction the cation and anion of the two compound switch places. In this reaction 2 Compound (reactants) exchange of ions to form 2 new compounds (products).
c) Single displacement reaction:
Single displacement reaction occurs when one of the element displaces the another element from its compound.
d) Redox reaction:
In redox reactions oxidation and reduction occurs simultaneously.
e) Neutralization reaction:
Neutralization reaction also known as acid base reaction. As in this reaction acid and base neutralizes to produce salt and water.
f) Decomposition reaction:
Decomposition reaction occurs when large or complex compound break down into simpler compounds or elements.
g) Combustion reaction:
Combustion reaction is a reaction in which the hydrocarbons react with oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O).
h) Combination reaction :
Combination reaction is a reaction in which 2 or more reactant combine to form a single product.
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