The equation for nitrogen reacting with hydrogen is given below. $\text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g}) \qquad \Delta H_r^\circ = -92.2\,\text{kJ mol}^{-1}$ Which statement is correct?
- A$\Delta H_r^\circ$ is measured at $298\,^\circ\text{C}.$
- B$\Delta H_r^\circ$ is measured at $101\,\text{kPa}.$
- C$\Delta H_r^\circ$ represents the standard enthalpy change for the formation of ammonia gas.
- D$\Delta H_r^\circ$ represents the enthalpy change when $1.0\,\text{mol}$ of $\text{N}_2(\text{g})$ reacts with $1.0\,\text{mol}$ of $\text{H}_2(\text{g}).$