Based on the following thermochemical equations<br><br><br><br><br>The value of ‘’ will be — Thermodynamics and Thermochemistry Chemistry Question
Question
Based on the following thermochemical equations<br>$\text{H}_2\text{O(g)} + \text{C(s)} \to \text{CO(g)} + \text{H}_2\text{(g)}; \Delta H = 131\text{ kJ}$<br>$\text{CO(g)} + 1/2 \text{O}_2\text{(g)} \to \text{CO}_2\text{(g)}; \Delta H = -282\text{ kJ}$<br>$\text{H}_2\text{(g)} + 1/2 \text{O}_2\text{(g)} \to \text{H}_2\text{O(g)}; \Delta H = -242\text{ kJ}$<br>$\text{C(s)} + \text{O}_2\text{(g)} \to \text{CO}_2\text{(g)}; \Delta H = X\text{ kJ}$<br>The value of ‘$X$’ will be
💡 Solution & Explanation
The final reaction is the sum of the first three reactions. By adding them together, intermediate species ($\text{H}_2\text{O(g)}$, $\text{CO(g)}$, $\text{H}_2\text{(g)}$) cancel out, resulting directly in the formation equation for $\text{CO}_2$. $X = 131 + (-282) + (-242) = 131 - 524 = -393\text{ kJ}$.