how do i solve this thermochemical equation? and what r the steps to it

1. Find the heat of reaction for the following equation.
N2(g) + 2 O2(g) -> N2O4(g)

given the following steps
2NO2(g) -> N2(g)+ 2O2(g) delta H=-84.8 kj
N2O4(g)-> 2NO2(g) delta H= 72.8 kj
if you can solve this that would be really great thank you. and there might be more

To solve the given thermochemical equation and find the heat of reaction, follow these steps:

Step 1: Write down the given equations and their corresponding enthalpy changes:
a. 2NO2(g) -> N2(g) + 2O2(g) ΔH = -84.8 kJ
b. N2O4(g) -> 2NO2(g) ΔH = 72.8 kJ

Step 2: Rearrange equation "a" by switching the reactants and products to match the target equation. Keep track of the sign of the enthalpy change:
a. N2(g) + 2O2(g) -> 2NO2(g) ΔH = +84.8 kJ

Step 3: Add equation "b" to equation "a" by canceling out the common species (2NO2(g) and 2NO2(g)) to obtain the target equation:
N2(g) + 2O2(g) -> N2O4(g)

Add the enthalpy changes together:
ΔH = +84.8 kJ + 72.8 kJ = +157.6 kJ

Therefore, the heat of reaction for the given thermochemical equation is +157.6 kJ.

Note: It is important to pay attention to the stoichiometric coefficients and adjust them as needed to balance the equation. The signs of the enthalpy changes (ΔH) indicate whether a reaction is endothermic (+) or exothermic (-).