Adiabatic flame temperature of hydrogen peroxide calculation

I will first demonstrate my cursory method for evaluating the adiabatic flame temperature of H2O2 at atmospheric pressure. 


$$\ce{H2O2 -> H2O + 0.5O2}$$


At $\pu{1200 K}$, 


\begin{align}
h\_\ce{H2O}^\pu{1200 K} - h\_\ce{H2O}^\pu{298 K} &= \pu{34.506 kJ/mol}\\
h\_\ce{O2}^\pu{1200 K} - h\_\ce{O2}^\pu{298 K} &= \pu{29.761 kJ/mol}\\
\Delta\_f H^\pu{298 K} &= \pu{-241.826 kJ/mol}
\end{align}
Sources: $\ce{H2O}$: <https://janaf.nist.gov/tables/H-064.html>; $\ce{O2}$: <https://janaf.nist.gov/tables/O-029.html>


At this temperature,


$$\text{Energy released} = 241.826 - 34.506 - 0.5 \times 29.761 = \pu{192.44 kJ/mol}$$


For Adiabatic flame temperature, the energy released should be equal to zero which is not so in this case (I am aware that the process is iterative). However, multiple sources indicate the flame temperature to be around $\pu{1000 K}$. A screenshot from RPA (a rocket propulsion software) is one such source. 


[![enter image description here](https://i.stack.imgur.com/WVdZO.png)](https://i.stack.imgur.com/WVdZO.png)
The software obviously takes into account other products but, even as a first estimate my calculation shouldn't have been so off from the software calculation. I would appreciate any help in pointing out the mistake in my calculation. 


