because u need to dissconnect the inter-molecular bonds aswell.(it's natural state is liquid)
not only the covalent ones.
Endothermic reaction: In an endothermic reaction, the products are higher in energy than the reactants. Therefore, the change in enthalpy is positive, and heat is absorbed from the surroundings by the reaction therefore enthalpy change show positive sign in a endothermic reaction..
The relationship between enthalpy (H) and entropy (S) is described by the Gibbs free energy equation, ΔG = ΔH - TΔS, where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy. For a reaction to be spontaneous at higher temperatures but not at lower temperatures, the entropy term (TΔS) must dominate over the enthalpy term (ΔH) in the Gibbs free energy equation. This suggests that the increase in entropy with temperature plays a more significant role in driving the reaction towards spontaneity than the enthalpy change.
The difference between the bond enthalpy of the reactants and the bond enthalpy of the products in a chemical reaction represents the energy change that occurs during the reaction. If the bond enthalpy of the products is lower than that of the reactants, it indicates that energy is released during the reaction, making it exothermic. Conversely, if the bond enthalpy of the products is higher than that of the reactants, it indicates that energy is absorbed during the reaction, making it endothermic.
The enthalpy of an ideal gas increases with temperature. As the temperature rises, the kinetic energy of the gas molecules also increases, leading to higher enthalpy.
The molar enthalpy of fusion of ice is relatively high compared to the molar enthalpy of fusion of many other solids. This is because ice requires a significant amount of energy to change from a solid to a liquid state due to its strong hydrogen bonds. However, there are some solids, such as metals, that have higher molar enthalpies of fusion than ice.
If you plot the reaction coordinate (what I think you mean by "enthalpy change diagram"), the reaction will be exothermic if the products are lower on the graph than the reactants. If they are higher than it is endothermic. For instance, if you go to the linked Wikipedia page (link to the left of this answer), the graph shown is of an exothermic reaction.
Endothermic reaction: In an endothermic reaction, the products are higher in energy than the reactants. Therefore, the change in enthalpy is positive, and heat is absorbed from the surroundings by the reaction therefore enthalpy change show positive sign in a endothermic reaction..
The ionisation enthalpy of potassium is lower than that of sodium.
The relationship between enthalpy (H) and entropy (S) is described by the Gibbs free energy equation, ΔG = ΔH - TΔS, where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy. For a reaction to be spontaneous at higher temperatures but not at lower temperatures, the entropy term (TΔS) must dominate over the enthalpy term (ΔH) in the Gibbs free energy equation. This suggests that the increase in entropy with temperature plays a more significant role in driving the reaction towards spontaneity than the enthalpy change.
Bromine has a higher electron affinity than iodine. This is because bromine has a smaller atomic size, resulting in a stronger attraction for electrons compared to iodine.
The relationship between air enthalpy and the efficiency of a heating and cooling system is that the enthalpy of the air affects the amount of energy needed to heat or cool it. Higher enthalpy levels require more energy to change the temperature of the air, which can impact the efficiency of the system. In general, a heating and cooling system will be more efficient when working with air at lower enthalpy levels.
The difference between the bond enthalpy of the reactants and the bond enthalpy of the products in a chemical reaction represents the energy change that occurs during the reaction. If the bond enthalpy of the products is lower than that of the reactants, it indicates that energy is released during the reaction, making it exothermic. Conversely, if the bond enthalpy of the products is higher than that of the reactants, it indicates that energy is absorbed during the reaction, making it endothermic.
The enthalpy of an ideal gas increases with temperature. As the temperature rises, the kinetic energy of the gas molecules also increases, leading to higher enthalpy.
Bromine has a larger radius (not raduis) than chlorine.
Bromine has because the ionization energy increases as you move across and decreases as you move down.
The molar enthalpy of fusion of ice is relatively high compared to the molar enthalpy of fusion of many other solids. This is because ice requires a significant amount of energy to change from a solid to a liquid state due to its strong hydrogen bonds. However, there are some solids, such as metals, that have higher molar enthalpies of fusion than ice.
The combustion of methanol to form products of H2O and CO2 do not have as much of an energy change compared to methane and a result methanol releases less energy compared to methane. The more negative an enthalpy change is, the more heat it is going to release.