The reaction below is the last step in the commercial production of sulfuric acid. How much heat is transferred if 200 kg of sulfuric acid are produced? SO3(g) + H2O(l) H2SO4(aq) ΔH = -227 kJ
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Step 1
Then, we convert the mass of sulfuric acid produced into moles. 200 kg is equal to 200,000 g. So, the number of moles of sulfuric acid produced is 200,000 g / 98 g/mol = approximately 2041 mol. The heat transferred is the product of the number of moles and the Show more…
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SO3(g) + H2O(l) → H2SO4(aq) is the final step in the synthesis of sulfuric acid in industry. The ΔH for this reaction is -227 kJ. Explain whether it is necessary to heat up or cool down the reaction mixture.
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The reaction $$\mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q)$$ is the last step in the commercial production of sulfuric acid. The enthalpy change for this reaction is $-227 \mathrm{kJ}$ In the design of a sulfuric acid plant, is it necessary to provide for heating or cooling of the reaction mixture? Explain your answer.
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