Chemistry - Chemical Equilibrium Question with Solution | TestHub
ChemistryChemical EquilibriumProblems involving KpHard2 minQB
ChemistryHardsingle choice
Δf G° for the formation of HI(g) from its gaseous elements is -4.606 kcal/mol at 500 K. When the partial pressure of HI is 20 atm and of I2(g) is 4×10-4 atm, what must be the partial pressure of hydrogen at this temperature to reduce the magnitude of Δ G for the reaction to zero?
Options:
Answer:
D
Solution:
The reaction is 1/2H2(g) + 1/2I2(g) → HI(g) Take R = 2 cal/mol/K so that RT = 1000 cal/mol
Δ G° = -4606 cal/mol = -4.606 RT = -RTln 100
Δ G = Δ G° + RTln Q = 0 gives Q = 100
Q = PHI/(√(PH2)√(PI2)) = 20/(√(PH2)×0.02) = 100
√(PH2) = 20/(0.02×100) = 10
PH2 = 100 atm
This is option (d).
Stream:JEESubject:ChemistryTopic:Chemical EquilibriumSubtopic:Problems involving Kp
⏱ 2mℹ️ Source: QB
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