Chemistry - Thermochemistry Question with Solution | TestHub
ChemistryThermochemistryEnthalpy of solution/dilution/hydrationMedium2 minQB
ChemistryMediumnumerical
The reversible reaction:
Na2SO4 · 10H2O → Na2SO4 + 10H2O; ΔH = +15.0 kcal
goes completely to the right at temperature above 34°C and remains completely on the left below this temperature. This system has been used in some solar houses for heating at night with the energy absorbed from the sun's radiation during the day. How many litres of fuel gas could be saved per night by the reversal of the dehydration of a fixed charge of 64.4 kg Na2SO4·10H2O? Assume that the fuel value of the gas is 7500 kcal/m3.
Answer:
400.00
Solution:
Moles of Na2SO4·10H2O = 64400/322 = 200 mol. Heat released on hydration at night = 200 × 15.0 = 3000 kcal. Fuel gas saved = 3000/7500 = 0.4 m3 = 400 l. Answer: 0400.
Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of solution/dilution/hydration
⏱ 2mℹ️ Source: QB
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