Question
What is the equilibrium constant for the reaction of nitrogen gas and hydrogen gas to form ammonia?
Answers
GPT-4o mini
The equilibrium constant (K) for the reaction of nitrogen gas (N₂) and hydrogen gas (H₂) to form ammonia (NH₃) can be expressed with the following balanced chemical equation:
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \]
The equilibrium constant expression (K) for this reaction is given by:
\[
K = \frac{[\text{NH}_3]^2}{[\text{N}_2][\text{H}_2]^3}
\]
Where:
- \([\text{NH}_3]\) is the concentration of ammonia,
- \([\text{N}_2]\) is the concentration of nitrogen gas,
- \([\text{H}_2]\) is the concentration of hydrogen gas.
The specific value of the equilibrium constant (K) depends on the temperature of the system since equilibrium constants are temperature-dependent. For the Haber process, which synthesizes ammonia, the value of K at 450 °C is typically around 6.0 × 10⁻², but this can vary with changes in temperature and pressure. If you need a specific value for a particular temperature, please provide that temperature or check relevant sources for those conditions.
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \]
The equilibrium constant expression (K) for this reaction is given by:
\[
K = \frac{[\text{NH}_3]^2}{[\text{N}_2][\text{H}_2]^3}
\]
Where:
- \([\text{NH}_3]\) is the concentration of ammonia,
- \([\text{N}_2]\) is the concentration of nitrogen gas,
- \([\text{H}_2]\) is the concentration of hydrogen gas.
The specific value of the equilibrium constant (K) depends on the temperature of the system since equilibrium constants are temperature-dependent. For the Haber process, which synthesizes ammonia, the value of K at 450 °C is typically around 6.0 × 10⁻², but this can vary with changes in temperature and pressure. If you need a specific value for a particular temperature, please provide that temperature or check relevant sources for those conditions.