Enthelpy change & lattice energy - check please

In summary, the conversation is about writing reactions that represent the enthalpy change as the lattice energy for different compounds. The first example given is the reaction for silver fluoride, with the physical states of solid silver fluoride and gaseous silver and fluoride ions. The person then asks for help with another reaction, specifically for iron (III) chloride. The expert asks for clarification on the physical state of silver fluoride, and then gives a hint to break down the molecule into individual atoms and assign the correct charges to them.
  • #1
jewilki1
21
0
Write the reaction where the enthalpy change is the lattice energy for silver floride. Make sure you include the physical states.

Ag F (ag) yields Ag Positive(g) + F negative(g)

Could you please check this
Thanks
Could you help with this one: write the equation for the reaction where the enthalpy change represents the lattice energy of iron (III) chloride (FeCl3) Do not forget to include the physical states. Could you get me started?
Thanks
 
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  • #2
jewilki1 said:
Write the reaction where the enthalpy change is the lattice energy for silver floride. Make sure you include the physical states.
Ag F (ag) yields Ag Positive(g) + F negative(g)
Could you please check this
Thanks
This is almost correct, but what is "(ag)" ?
Could you help with this one: write the equation for the reaction where the enthalpy change represents the lattice energy of iron (III) chloride (FeCl3) Do not forget to include the physical states. Could you get me started?
Thanks
This is just like the other problem. First break up the molecule into individual atoms (FeCl3 breaks up into an Fe atom and 3 Cl atoms). Next you put the correct charges on these atoms to convert them to the appropriate ions. So Fe should be Fe(3+), and each Cl would be... ?
 
  • #3


Sure, I would be happy to help with this question. The equation for the reaction where the enthalpy change represents the lattice energy of iron (III) chloride (FeCl3) would be:

FeCl3(s) → Fe3+(g) + 3Cl-(g)

This reaction represents the process of breaking apart the solid FeCl3 into its gaseous ions, Fe3+ and Cl-. The enthalpy change for this reaction would be equal to the lattice energy of FeCl3, which is the energy required to completely separate the ions in the solid crystal lattice. The physical states for this reaction are solid (s) for FeCl3 and gaseous (g) for Fe3+ and Cl-.

I hope this helps and please let me know if you have any further questions.
 

1. What is enthalpy change?

Enthalpy change, also known as heat of reaction, is the amount of energy absorbed or released during a chemical reaction. It is represented by the symbol ΔH and is measured in units of joules (J) or kilojoules (kJ).

2. How is enthalpy change related to lattice energy?

Lattice energy is the energy released when gaseous ions form a solid crystal lattice. This energy is directly related to enthalpy change because it is a measure of the strength of the attractive forces between ions in a crystal lattice. As enthalpy change increases, so does lattice energy.

3. How is enthalpy change calculated?

Enthalpy change can be calculated using the equation ΔH = H(products) - H(reactants), where H represents the enthalpy (or heat content) of the system. The enthalpy values for the reactants and products can be found in a standard enthalpy table.

4. What factors affect lattice energy?

The strength of the attractive forces between ions in a crystal lattice, and therefore the lattice energy, is affected by several factors. These include the size of the ions, the charge of the ions, and the distance between the ions. Generally, smaller ions and higher charges lead to stronger attractive forces and higher lattice energies.

5. How can enthalpy change and lattice energy be used in chemical reactions?

Enthalpy change and lattice energy are important in understanding the thermodynamics of chemical reactions. They can be used to predict whether a reaction will release or absorb heat, and to calculate the amount of heat released or absorbed. These values also provide insight into the stability of chemical compounds and the strength of their bonds.

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