Answered

Suppose a gaseous reaction is given as:

[tex]\[ 2 AB(g) \rightarrow A_2(g) + B_2(g) \][/tex]

What is the enthalpy change if the reaction releases [tex]\( 206 \, \text{kJ} \cdot \text{mol}^{-1} \)[/tex]?



Answer :

GinnyAnswer
To solve the given problem, we need to determine the enthalpy change ([tex]\(\Delta H\)[/tex]) for the reaction. The reaction provided is:

[tex]\[2 AB (g) \rightarrow A_2 (g) + B_2 (g)\][/tex]

The enthalpy change is specified as [tex]\(206 \, \text{kJ/mol}\)[/tex]. This means that the amount of energy absorbed or released during the reaction corresponds to this value.

In the context of the problem, the enthalpy change is given directly, so we do not need to perform any additional calculations. Therefore, the enthalpy change for the reaction is:

[tex]\[\Delta H = 206 \, \text{kJ/mol}\][/tex]

This indicates that the reaction involves an enthalpy change of 206 kilojoules per mole.