Use standard enthalpies of formation to determine AHm for the reaction: Cr2O3(s) + 3CO(9)→2Cr(s) +3CO2(g). -2651.7 kJ 290.7 kJ -856.7 kJ 69.7 kJ

26. Calculate the enthalpy change for the reaction below. NO(g) + O(g) →→→ NO₂(g) Given following data: NO(g) + O₂(g) →→ NO₂(g) + O₂(g) 03(g) → 1.50₂(g) 0₂(g) →20(g) AH-198.9 kJ AH = -142.3 kJ ΔΗ = 495.0 kJ

Given the overall reaction from the previous problem: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) Using Le Chatelier’s principle, predict which direction the reaction will shift to reestablish equilibrium for each of the following changes: Calculate the enthalpy of reaction for this reaction using the standard thermodynamics values for the reactants and products. Is the reaction endothermic or exothermic? Now, use Le Chatelier’s principle again to determine the direction the equilibrium will shift if heat is added to the reaction.  If 35 kPa of CO is mixed with 35 kPa of hydrogen in a 1.5 L container at 25°C, what is the theoretical yield of methane?

Given that enthalpy of formation of the several compounds: C(s)+O2(g)>CO2(g);AH=-393.5kJ S(s)+O2(g)→SO2(g);AH=-296.8kJ C(s)+2S(s)→CS2(1);AH=+87.9 kJ Determine the enthalpy of combustion reaction of carbon disulfide!