δh₂ = -200 kj\nδh₃ = -300 kj\ne + f\nδh₁ = 800 kj\nδhᵣₓₙ\na + 2d\nwhat is the overall enthalpy change δhᵣₓₙ…

δh₂ = -200 kj\nδh₃ = -300 kj\ne + f\nδh₁ = 800 kj\nδhᵣₓₙ\na + 2d\nwhat is the overall enthalpy change δhᵣₓₙ for the system?\nmark this and return\nsave and ex

δh₂ = -200 kj\nδh₃ = -300 kj\ne + f\nδh₁ = 800 kj\nδhᵣₓₙ\na + 2d\nwhat is the overall enthalpy change δhᵣₓₙ for the system?\nmark this and return\nsave and ex

Answer

Explanation:

Step1: Analyze Enthalpy Paths

The enthalpy change for the reaction ( A + 2D \rightarrow E + F ) can be found by considering the sum of the enthalpy changes of the individual steps. The total enthalpy change is the sum of ( \Delta H_1 ), ( \Delta H_2 ), and ( \Delta H_3 ), but we need to consider the direction of each step. The green arrow ( ( \Delta H_1 = 800 , \text{kJ} )) is an upward (endothermic) step, the blue arrow ( ( \Delta H_2 = -200 , \text{kJ} )) is a downward (exothermic) step, and the purple arrow ( ( \Delta H_3 = -300 , \text{kJ} )) is also a downward (exothermic) step. The red arrow is the reaction enthalpy we need to find.

Step2: Apply Hess's Law

Hess's Law states that the total enthalpy change of a reaction is the sum of the enthalpy changes of its individual steps. So, we can write the equation for the total enthalpy change as: [ \Delta H_{\text{rxn}}=\Delta H_1+\Delta H_2+\Delta H_3 ] Substitute the given values: ( \Delta H_1 = 800 , \text{kJ} ), ( \Delta H_2=- 200 , \text{kJ} ), ( \Delta H_3 = - 300 , \text{kJ} ) [ \Delta H_{\text{rxn}}=800+( - 200)+( - 300) ] [ \Delta H_{\text{rxn}}=800 - 200 - 300 ] [ \Delta H_{\text{rxn}}=300 , \text{kJ} ]

Answer:

The overall enthalpy change ( \Delta H_{\text{rxn}} ) for the system is ( \boldsymbol{300 , \text{kJ}} )