Química·Andalucía·2011·Variante 611Ejercicio6Opción B2 puntosPara la reacción: CHX4(g)+2 OX2(g)→COX2(g)+2 HX2O(l)\ce{CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)}CHX4(g)+2OX2(g)COX2(g)+2HX2O(l)DatosΔHf0[CHX4(g)]=−74,8 kJ/mol\Delta H_f^0[\ce{CH4(g)}] = -74{,}8\,\text{kJ/mol}ΔHf0[CHX4(g)]=−74,8kJ/molΔHf0[COX2(g)]=−393,5 kJ/mol\Delta H_f^0[\ce{CO2(g)}] = -393{,}5\,\text{kJ/mol}ΔHf0[COX2(g)]=−393,5kJ/molΔHf0[HX2O(l)]=−285,5 kJ/mol\Delta H_f^0[\ce{H2O(l)}] = -285{,}5\,\text{kJ/mol}ΔHf0[HX2O(l)]=−285,5kJ/molS0[CHX4(g)]=186,3 J⋅mol−1⋅K−1S^0[\ce{CH4(g)}] = 186{,}3\,\text{J} \cdot \text{mol}^{-1} \cdot \text{K}^{-1}S0[CHX4(g)]=186,3J⋅mol−1⋅K−1S0[OX2(g)]=205,1 J⋅mol−1⋅K−1S^0[\ce{O2(g)}] = 205{,}1\,\text{J} \cdot \text{mol}^{-1} \cdot \text{K}^{-1}S0[OX2(g)]=205,1J⋅mol−1⋅K−1S0[COX2(g)]=213,7 J⋅mol−1⋅K−1S^0[\ce{CO2(g)}] = 213{,}7\,\text{J} \cdot \text{mol}^{-1} \cdot \text{K}^{-1}S0[COX2(g)]=213,7J⋅mol−1⋅K−1S0[HX2O(l)]=69,9 J⋅mol−1⋅K−1S^0[\ce{H2O(l)}] = 69{,}9\,\text{J} \cdot \text{mol}^{-1} \cdot \text{K}^{-1}S0[HX2O(l)]=69,9J⋅mol−1⋅K−1aCalcule la variación de entalpía y de la entropía de la reacción en condiciones estándar a 25 ∘C25\,^{\circ}\text{C}25∘C.bIndique razonadamente si el proceso es espontáneo a 100 ∘C100\,^{\circ}\text{C}100∘C.
