The gasification of coal is a method of producing methane by the following reaction.
C(s)+2H2(g)------> CH4(g) △H=?
Find △H(kJ/mol)
Answer (1)
[tex]\begin{gathered}\begin{gathered}{\underline{\huge \mathbb{A} {\large \mathrm {NSWER : }}}} \\\end{gathered}\end{gathered}[/tex] To find the change in enthalpy ([tex]\Delta H[/tex]) for the gasification of coal reaction: [tex]C(s) + 2H_2(g) \rightarrow CH_4(g)[/tex] we need to consider the standard enthalpy of formation ([tex]\Delta H_f^\circ[/tex]) values for each of the substances involved in the reaction. The enthalpy change for the reaction can be calculated using the following formula: [tex]\Delta H = \sum \Delta H_f^\circ (\text{products}) - \sum \Delta H_f^\circ (\text{reactants})[/tex] Look Up Standard Enthalpy of Formation Values For Methane ([tex]CH_4(g)[/tex]): [tex]\Delta H_f^\circ = -74.8 \text{ kJ/mol}[/tex] For Carbon ([tex]C(s)[/tex]): [tex]\Delta H_f^\circ = 0 \text{ kJ/mol}[/tex] (standard state) For Hydrogen ([tex]H_2(g)[/tex]): [tex]\Delta H_f^\circ = 0 \text{ kJ/mol}[/tex] (standard state) Calculate [tex]\Delta H[/tex] Now, applying the values into the equation: [tex]\Delta H = [\Delta H_f^\circ (CH_4)] - [\Delta H_f^\circ (C) + 2 \cdot \Delta H_f^\circ (H_2)][/tex] Substituting the values: [tex]\Delta H = [-74.8 \text{ kJ/mol}] - [0 + 2 \cdot 0][/tex] [tex]\Delta H = -74.8 \text{ kJ/mol}[/tex] Conclusion The change in enthalpy ([tex]\Delta H[/tex]) for the gasification of coal reaction is: [tex]\Delta H = -74.8 \text{ kJ/mol}[/tex] This indicates that the reaction is exothermic, releasing energy.
