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What else can I help you with?
Why does physisorption decrease with the increase of temperature?
Physisorption is weaker than chemisorption and is typically dependent on van der Waals forces. As temperature increases, the thermal energy disrupts these weak interactions between the adsorbate and the surface, leading to a decrease in physisorption.
Is ionisation enthalpy of potassium higher than that of sodium?
The ionisation enthalpy of potassium is lower than that of sodium.
How do you know if an enthalpy change diagram is endothermic or exothermic?
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.
Which chemical reaction does the enthalpy diagram above represent?
I'm unable to view images or diagrams, so I cannot directly identify the chemical reaction represented in the enthalpy diagram you mentioned. However, enthalpy diagrams typically illustrate exothermic or endothermic reactions by showing changes in enthalpy during the reaction process. If you describe the key features of the diagram, such as whether the products are at a lower or higher energy level than the reactants, I can help you identify the type of reaction it represents.
What is known about a reaction with the positive enthalpy?
A reaction with a positive enthalpy change, often referred to as an endothermic reaction, absorbs heat from its surroundings. This means that the products of the reaction have a higher energy content than the reactants. As a result, the temperature of the surroundings may decrease during the reaction. Examples include photosynthesis and the dissolution of certain salts in water.
Why does physisorption decrease with the increase of temperature?
Physisorption is weaker than chemisorption and is typically dependent on van der Waals forces. As temperature increases, the thermal energy disrupts these weak interactions between the adsorbate and the surface, leading to a decrease in physisorption.
Is ionisation enthalpy of potassium higher than that of sodium?
The ionisation enthalpy of potassium is lower than that of sodium.
How do you know if an enthalpy change diagram is endothermic or exothermic?
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.
What is the difference between the bond enthalpy of the reactants and the bond enthalpy of the products in a chemical reaction?
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.
Why is enthalpy change of atomization of bromine is higher than bond enthalpy?
The enthalpy change of atomization of bromine is higher than its bond enthalpy because it accounts for breaking the diatomic molecule into individual bromine atoms in the gas phase, which requires overcoming intermolecular forces. Bond enthalpy, on the other hand, only considers the energy needed to break the specific bond in a molecule, not breaking the entire molecule into individual atoms.
What is the definition of physisorption?
Physisorption is the reversible adsorption of molecules onto a surface due to weak van der Waals forces. It involves physical interactions rather than chemical bonds, and can occur in processes such as gas adsorption on solid surfaces.
In an exothermic reaction is the energy of the products higher or lower than that of the reactants?
In an exothermic reaction the energy of the products is less than that of the reactants.
How does molar enthalpy of fussion of ice compare with the molar enthalpy of fussion of other solids?
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.
How do you know if a reaction is entropy driven enthalpy driven or driven by both enthalpy and energy?
If the ∆H is positive and the ∆S is positive, then the reaction is entropy driven. If the ∆H is negative and the ∆S is negative, then the reaction is enthalpy driven. If ∆H is positive and ∆S is negative, then the reaction is driven by neither of these. If ∆H is negative and ∆S is positive, then the reaction is driven by both of these.
What is the sign of the enthalpy change for an endothermic 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..
Which enthalpy is higher 2 Cl or cl2?
The enthalpy of Cl2 (chlorine gas) is higher than 2 Cl (two atoms of chlorine). This is because forming Cl2 from two Cl atoms involves the breaking of an existing bond between the atoms, which requires energy input, whereas 2 Cl atoms do not require this bond formation energy.
How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?
Sodium has only one valence electron, and when that is donated to some other atom, the remaining ion has a noble gas configuration that is highly stable. Disrupting that by another ionization requires much energy. Magnesium has two valence electrons; therefore the second is almost as easy to donate as the first. The third ionization enthalpy of magnesium would be very high.
