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Question: The heat of combustion of yellow phosphorus is \( - 9.91KJ\) and heat of combustion of red phosphoru...

The heat of combustion of yellow phosphorus is −9.91KJ - 9.91KJ and heat of combustion of red phosphorus is −8.78KJ - 8.78KJ . Which of the following represents the heat of transition of yellow phosphorus to red phosphorus?
A. −18.69KJ - 18.69KJ
B. +1.13KJ + 1.13KJ
C. +18.69KJ + 18.69KJ
D. −1.13KJ - 1.13KJ

Explanation

Solution

We know that enthalpy of a system is the sum of internal energy and product of pressure and volume of that system. Hess’ law used in thermodynamics states that the change of enthalpy in a chemical reaction is a state function and is therefore independent of the path taken between initial and final states. If the enthalpy change for each equation is known, the resultant enthalpy is equal to the sum of enthalpies of each individual reaction.

Formula Used:
We will use the formula,
ΔnetH=∑ΔHr{\Delta _{net}}H = \sum {\Delta {H_r}}
ΔnetH={\Delta _{net}}H = Net enthalpy of the reaction
∑ΔrH=\sum {} {\Delta _r}H = Sum of enthalpies of the reactions.

Complete answer:
Phosphorus is a group 1515 element and is represented by the symbol PP . It is a p−p - block element and exists in many allotropic forms. Each allotropic form has a different chemical arrangement and different chemical properties. The two most common allotropic forms of phosphorus are white phosphorus and red phosphorus. Red phosphorus is formed by exposing white phosphorus to sunlight. Yellow phosphorus is formed from a small amount of red phosphorus and is highly toxic.
The heat of combustion is the amount of heat released when 11 mole of a compound is completely burnt. Since it is an exothermic reaction ΔH\Delta H is negative. According to the given question
The heat of combustion of yellow phosphorus is −9.91KJ - 9.91KJ
P4(y)+5O2→2P2O5{P_4}\left( y \right) + 5{O_2} \to 2{P_2}{O_5}
The heat of combustion of red phosphorus is −8.78KJ - 8.78KJ
P4(r)+5O2→2P2O5{P_4}\left( r \right) + 5{O_2} \to 2{P_2}{O_5}
Subtracting both the equations and applying Hess law, we get
P4(y)→P4(r){P_4}(y) \to {P_4}(r)
⇒−9.91−(−8.78)KJ=−1.13KJ\Rightarrow - 9.91 - ( - 8.78) KJ = - 1.13KJ

**Thus heat of transition of yellow phosphorus to red phosphorus is −1.13KJ - 1.13KJ . Therefore, the correct option is D.

Note:**
It is important to note that the transition takes place from yellow to red phosphorus. The enthalpy change should be calculated accordingly. Hess’ law is a very useful equation used to calculate the change in enthalpy from a large range of data. Born-Haber cycle is an application of Hess’ law. It is used to calculate the lattice energy of ionic compounds.