Explanation:
1. The three factors are;
- Increasing the surface area of the reactants
- Using a catalyst
- Increasing temperature
2. Raising the temperature of a reaction mixture is the same as increasing the kinetic energy of the reacting molecules.
3. This reaction is an exothermic reaction. In exothermic reaction, the temperature of the system (mixture) decreases while that of the surroundings increases.
4. Reactions that releases energy to the surroundings are exothermic reactions.
5. All the options is an example of exothermic process because heat is being removed from the system except;
B. Evaporation of water - This is because it must absorb heat from the surroundings making it endothermic.
Answer:
True
Explanation:
This is because the Earths ionisphere was distrubed which makes radio communications.
Answer: Compound . Chemical reactions can divide elements into simpler substances, but they cannot separate elements into simpler substances. Physical or chemical characteristics of substances can be categorised.
Compounds and elements can be created from pure substances. A chemical reaction is required to break down pure substances (elements and compounds) into their component atoms or elements. This is known as the chemical separation process. Physical separation of pure substances is impossible.
Explanation:
What makes something pure substance?
One element or a small number of related compounds make up pure substances. Mixtures are assemblages of many components. Mixtures of two or more substances (or elements) that cannot be visually distinguished from one another are referred to as homogeneous mixtures.
What sort of compound would that be?
A substance made up of two or more components is called a compound. Table salt, water, and carbon dioxide are a few examples of compounds
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Answer:
The statement is FALSE.
Explanation:
It is known as the ion effect common to the displacement of an ionic equilibrium when the concentration of one of the ions that are involved in said equilibrium changes, due to the presence in the dissolution of a salt that is dissolved in it.
Given the reaction of the dissociation reaction of a weak electrolyte:
AB (s) ⇔ A⁺(aq) + B⁻ (aq)
The equilibrium constant of the reaction is:
![K_{ps}=\frac{[A^+][B^-]}{[AB]}](https://tex.z-dn.net/?f=K_%7Bps%7D%3D%5Cfrac%7B%5BA%5E%2B%5D%5BB%5E-%5D%7D%7B%5BAB%5D%7D)
Given the reaction of the dissociation reaction of a stong electrolyte:
CB (s) ⇒ C⁺(aq) + B⁻ (aq)
If the electrolyte CB is added to the medium in which electrolyte AB is found, the medium will have a common ion B⁻:
AB (s) ⇔ A⁺(aq) + B⁻ (aq)
CB (s) ⇒ C⁺(aq) + B⁻ (aq)
By the Le Chatelier's principle, having more concentration of products, the balance will shift to the right.
Hence, the extent of ionization of a weak electrolyte is decreased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.
