If the following reaction:
NO(g) + 1/2O2(g) NO2(g)
has the following enthalpy change:
H° = -56 kJ/mol
What is the enthalpy of the decomposition reaction of 2 moles of NO2?
A. 112 kJ
B. 56 kJ
C. -56 kJ
D. -112 kJ
i think the answer is d
I just answered your earlier post.
To find the enthalpy change of the decomposition reaction of 2 moles of NO2, we need to consider the balanced equation for the reaction.
The given reaction is:
2NO(g) + O2(g) → 2NO2(g)
The enthalpy change for this reaction is -56 kJ/mol, which means that 56 kJ of energy is released per mole of NO2 formed.
In the decomposition reaction, we are given that we have 2 moles of NO2. Since the coefficient in front of NO2 is 2 in the balanced equation, we can multiply the enthalpy change by 2 to find the total enthalpy change for 2 moles of NO2.
-56 kJ/mol × 2 = -112 kJ
Therefore, the enthalpy change of the decomposition reaction of 2 moles of NO2 is -112 kJ.
So, the correct answer is option D, -112 kJ.