2 ### Ammonia Decomposition ReactionAmmonia decomposes to form nitrogen and hydrogen, as shown in the following chemical equation:\[ 2\text{NH}_3(g) \rightarrow \text{N}_2(g) + 3\text{H}_2(g) \]A chemist finds that at a certain temperature, the equilibrium mixture of ammonia, nitrogen, and hydrogen has the following composition:| **Compound** | **Concentration at Equilibrium** ||--------------|-------------------------------------|| \(\text{NH}_3\) | 1.6 M || \(\text{N}_2\) | 0.34 M || \(\text{H}_2\) | 0.53 M |Calculate the value of the equilibrium constant \( K_c \) for this reaction. Round your answer to 2 significant digits.\[ K_c = \]This problem requires determining the equilibrium constant (\( K_c \)), using the formula:\[ K_c = \frac{[\text{N}_2][\text{H}_2]^3}{[\text{NH}_3]^2} \]The concentrations at equilibrium are provided, which can be plugged into the formula to calculate \( K_c \).

Given, 2 NH3(g) ➝ N2(g) + 3H2(g) Compound concentration at equilibrium NH3 1.6 M N2 0.34 M…

Ammonia decomposes to form nitrogen and hydrogen, like this: 2 NH3(g) → N₂(g) + 3H₂(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, nitrogen, and hydrogen has the following composition: compound concentration at equilibrium NH3 1.6M N₂ 0.34 M H₂ 0.53 M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = x10 X 3 ?