Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial chemical, and world production exceeds 2.0 x 10^11 kg per year. The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces 4.3 kg of solid sulfur and 10.0 atm of oxygen gas at 500. °C into an evacuated 40.0L tank. The engineer believes Kp=0.87 for the reaction at this temperature. Calculate the mass of solid sulfur she expects to be consumed when the reaction reaches equilibrium. Round your answer to 2 significant digits.

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A:

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A:

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Q: Find the molar enthalpy of the reactants and the products

A:

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