A displacement reaction occurs when a more reactive substance takes a less reactive one out of its salt solution; a double displacement reaction occurs when two compounds exchange ions. In a displacement reaction, only a single displacement takes place, whereas, in a double displacement reaction, two displacement takes place between the molecules. e.g. Single displacement …
(a) Thermal decomposition reaction (Thermolysis ) Potassium chlorate decomposition: Potassium chlorate breaks down into potassium chloride and oxygen when heated strongly. The production of oxygen is produced through this reaction. 2KClO3 + Heat → 2KCl + 3O2 (b) Electrolytic decomposition reaction (Electrolysis) Sodium chloride decomposes into sodium and chlorine when electricity is applied to molten …
The decomposition reaction is defined as the splitting of bigger molecules into two or smaller molecules, whereas the combination reaction is considered to be the reaction of two or more molecules to generate a larger molecule. Essentially, this describes how the decomposition process is the combination reaction\’s polar opposite. Since the heat from the surrounding …
For survival, life requires energy. The food we eat provides us with this energy. Through the process of digestion, the food molecules are reduced to simpler molecules like glucose. When these materials combine with the oxygen already present in our body cells, carbon dioxide and water are produced, along with a certain amount of energy …
Why is respiration considered to be an exothermic reaction? Read More »
When energy from the surroundings is absorbed in heat from the surroundings, an endothermic reaction takes place (For example, Photosynthesis, melting of ice, evaporation). On the other side, an exothermic reaction involves the release of energy from the system into the surroundings (Examples: Explosions, concrete settings, nuclear fission and fusion).
(i) 2KBr + BaI2 → 2KI + BaBr2 (Double Displacement Reaction) (ii) ZnCO3 → ZnO + CO2 (Decomposition Reaction) (iii) H2 + Cl2 → 2HCl (Combination Reaction) (iv) Mg + 2HCl → MgCl2 + H2 (Displacement Reaction)
2Ca(OH)2 + 2CO2 → 2CaCO3 + 2H2O Zn + 2AgNO3 → Zn(NO3)2 + 2Ag 2Al + 3CuCl2 → 2AlCl3 + 3Cu BaCl2 + K2SO4 → BaSO4 + 2KCl
(a) 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O (b) 2NaOH + H2SO4 → Na2SO4 + 2H2O (c) NaCl + AgNO3 → AgCl + NaNO3 (d) BaCl2 + H2SO4 → BaSO4 + 2HCl
(a) Unbalanced: H2 + N2 → NH3 Balanced: 3H2 + N2 → 2NH3 (b) Unbalanced: H2S + O2 → H2O + SO2 Balanced: 2H2S + 3O2 → 2H2O + 2SO2 (c) Unbalanced: BaCl2 + Al2(SO4)3 → AlCl3 + BaSO4 Balanced: 3BaCl2 + Al2(SO4)3 → 2AlCl3 + 3BaSO4 (d) Unbalanced: K + H2O → KOH + …
When the number of distinct atoms on the reactant and product sides of an equation is equal, the equation is said to be balanced. Chemical equations must be balanced for the reaction to follow the Law of Conservation of Mass. Chemical equation balancing is a trial-and-error process with no defined approach.
