Answer:
Explanation:
The total energy or intrinsic energy of a system is called the enthalpy. In thermochemistry, we have two types of enthalpy changes which are:
- Exothermic changes
- Endothermic changes
For the freezing of water, the enthalpy change is an exothermic one. Exothermic changes are designated as negative. In this chemical change, heat is liberated to the surroundings and this leaves the environment at a much higher temperature. In freezing, the enviroment gains more heat as the material begins to cool to lower temperature.
Entropy is the degree of randomness or disorderliness of a system. When a phase change occurs from liquid to solid, freezing takes place. Such a change increases the orderliness of a system and entropy diminishes. Here, entropy is negative.
The free energy is a measure of the energy a system that does useful work. Free energy depends on enthalpy, entropy and temperature of a system. For phase changes such as freezing of water, the value of free energy change is 0.
For this process, an increases in temperature makes it non-spontaneous. Increasing temperature would alter the course of the reaction and makes it exothermic. For entropy, increasing temperature would increase entropy and therefore, the reaction would not be feasible.
Temperature would mostly affect the free energy. An increase in temperature would increase the value of entropy change and the reaction would not be spontaneous. With falling temperature value, the reaction becomes more spontaneous and favored.
- Answer:
Energy release is exothermic reaction whiles energy absorb is endothermic reaction
Explanation:
Exothermic reaction is when the reactant is above the product while endothermic the product is below the reactant in the diagrams we have some part as activation energy
Answer:
Option b
Explanation:
Henry law describes solubility of gases in liquids.
According to Henry's law, amount of gas dissolved in a liquid depends upon its partial pressure above the liquids.
Mathematically, Henry's law is represented as:
C = K × P
Where,
C = Solubility of gas or concentration of gas in liquids
K = Henry's constant
P = Partial pressure of the gas over the liquid
For, Henry's law to be valid, pressure should be not too high and temperature should not be too low. Henry's law is also valid in case of low dissolved gas concentrations.
So, among the given options, option b, temperature is correct.
Answer: Silicon dioxide
Explanation:
di is 2 and since oxygen is 2
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