Which equation represents the atomization of iodine
Answers
no correct option is present
the correct equation will be:
(s) ------> 2I(g)
- atomization is defined as breaking the substance into its atoms.
- for example, consider chlorine it is a diatomic molecule and hence it consists of two atoms. now if we separate or break the bond between these two atoms then these two atoms will be separated, this process is atomization:
key points to remember
- the substance is broken down into its respective atoms
- atoms should be obtained in the gaseous form only
- it is defined as one mole of the substance
analyzing different options:
- first option
the product is in solid state and hence incorrect
- second option
the product is in the liquid state and hence incorrect
- third option
although the product is in a gaseous state but the standard state of iodine is solid but the reactant is liquid and hence incorrect
- fourth option
although the product is in a gaseous state but the standard state of iodine is solid but the reactant is gas and hence incorrect.
so the correct equation will be:
(s)------> 2I(g)
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Answer:
Enthalpy of atomization, ΔaH0, is the change in enthalpy when one mole of bonds is completely broken to obtain atoms in the gas phase. For example: atomization of methane molecule.
CH4 (g) → C (g) + 4H (g) ΔaH0= 1665.0 kJ mol-1
For diatomic molecules, the enthalpy of atomization is equal to the enthalpy of bond dissociation. For example: the atomization of dihydrogen molecule.
H2 (g) → 2H (g); ΔaH0= 435.0 kJ mol-1
Enthalpy of solution:
Enthalpy of the solution, ΔsolH0 is the enthalpy change when one mole of a substance is completely dissolved in a solvent. For example: enthalpy of dissolution of ionic compound in water.
Enthalpy change during phase transition:
When a substance undergoes a phase transition, that is the phase of a substance changes from one form to another, some energy is released or absorbed. For example, when the ice melts to water, energy is required for melting. Common enthalpy change during phase transition includes:
Standard Enthalpy of vaporization:
The standard enthalpy of vaporization, ΔvapH0 is the amount of heat required to vaporize one mole of a liquid at constant temperature and under standard pressure (1bar).
Standard enthalpy of sublimation:
Standard enthalpy of sublimation, ΔsubH0 is the change in enthalpy when one mole of a solid substance sublimes at a constant temperature and under standard pressure (1bar).
If pressure is kept constant, the change in enthalpy is proportional to the change in a system’s internal energy. Therefore, the atomization enthalpy equals the sum of the fusion and vaporisation enthalpies.
Which element has the lowest enthalpy of atomisation in the series Sc (Z = 21) to Zn (Z = 30)?
Sc (Z = 21) to Zn (Z = 30) belong to the fourth period of the periodic table. The degree of metallic bonding an element undergoes influences the atomization enthalpy. The more extensive an element’s metallic bonding is, the more its atomization enthalpy would be. The presence of some unpaired electrons in all transition metals with the exception of Zn, explains why their metallic bonds are stronger. Zn has the lowest enthalpy of atomization because it lacks these unpaired electrons, which weakens the inter-atomic electrical connection.
Explanation:
Enthalpy of atomization, ΔaH0, is the change in enthalpy when one mole of bonds is completely broken to obtain atoms in the gas phase. For example: atomization of methane molecule.
CH4 (g) → C (g) + 4H (g) ΔaH0= 1665.0 kJ mol-1
For diatomic molecules, the enthalpy of atomization is equal to the enthalpy of bond dissociation. For example: the atomization of dihydrogen molecule.
H2 (g) → 2H (g); ΔaH0= 435.0 kJ mol-1
Enthalpy of solution:
Enthalpy of the solution, ΔsolH0 is the enthalpy change when one mole of a substance is completely dissolved in a solvent. For example: enthalpy of dissolution of ionic compound in water.
Enthalpy change during phase transition:
When a substance undergoes a phase transition, that is the phase of a substance changes from one form to another, some energy is released or absorbed. For example, when the ice melts to water, energy is required for melting. Common enthalpy change during phase transition includes:
Standard Enthalpy of vaporization:
The standard enthalpy of vaporization, ΔvapH0 is the amount of heat required to vaporize one mole of a liquid at constant temperature and under standard pressure (1bar).
Standard enthalpy of sublimation:
Standard enthalpy of sublimation, ΔsubH0 is the change in enthalpy when one mole of a solid substance sublimes at a constant temperature and under standard pressure (1bar).
If pressure is kept constant, the change in enthalpy is proportional to the change in a system’s internal energy. Therefore, the atomization enthalpy equals the sum of the fusion and vaporisation enthalpies.
Which element has the lowest enthalpy of atomisation in the series Sc (Z = 21) to Zn (Z = 30)?
Sc (Z = 21) to Zn (Z = 30) belong to the fourth period of the periodic table. The degree of metallic bonding an element undergoes influences the atomization enthalpy. The more extensive an element’s metallic bonding is, the more its atomization enthalpy would be. The presence of some unpaired electrons in all transition metals with the exception of Zn, explains why their metallic bonds are stronger. Zn has the lowest enthalpy of atomization because it lacks these unpaired electrons, which weakens the inter-atomic electrical connection.
The energy needed to detach one electron from each mole of free gaseous atoms of that element is the first ionisation energy of an atom. There are still positive (ie endothermic) atomization enthalpies and ionisation enthalpies. Atomization enthalpy (atH) is the transition in enthalpy when one mole of gaseous atoms is formed from an atomic matter. In the other hand, the energy needed to split one mole of bond to give separate atoms in the gaseous state is bond enthalpy / bond energy / bond dissociation enthalpy.
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