Answer:
The reaction will be spontaneous
Explanation:
To determine if the reaction will be spontaneous or not at this temperature, we need to calculate the Gibbs's energy using the following formula: 
 
 
<u>If the Gibbs's energy is negative, the reaction will be spontaneous, but if it's positive it will not.</u>
Calculating the  :
 : 
 
 
Now, other factor we need to determine is the sign of the S variation. When talking about gases, the more moles you have in your system the more enthropic it is. 
In this reaction you go from 7 moles to 8 moles of gas, so you can say that you are going from one enthropy to another higher than the first one. This results in: ![\Delta S>0[/tex}Back to this expression: [tex]\Delta G= -1267 - 473 K* \Delta S](https://tex.z-dn.net/?f=%5CDelta%20S%3E0%5B%2Ftex%7D%3C%2Fp%3E%3Cp%3EBack%20to%20this%20expression%3A%20%3C%2Fp%3E%3Cp%3E%5Btex%5D%5CDelta%20G%3D%20-1267%20-%20473%20K%2A%20%5CDelta%20S%20) 
 
If the variation of S is positive, the Gibbs's energy will be negative always and the reaction will be spontaneous.