Chemistry - Chemical Equilibrium Question with Solution | TestHub
ChemistryChemical EquilibriumProblems involving KpHard2 minQB
ChemistryHardsingle choice
HBr is oxidised by O2 as:
HBr(g) + 1/4O2(g) ⇌ 1/2Br2(g) + 1/2H2O(g)
At a pressure of 760 mm and with an initial mixture containing 10% HBr and 90% O2, the degree of decomposition of the HBr is 0.10. What is the equilibrium partial pressure of oxygen?
Options:
Answer:
A
Solution:
Take 100 mol mixture: HBr = 10, O2 = 90 HBr decomposed = 10 × 0.10 = 1.0 mol; O2 consumed = 1.0/4 = 0.25 mol
Equilibrium: O2 = 89.75 mol; total moles = 9.0 + 89.75 + 0.5 + 0.5 = 99.75 mol
PO2 = (89.75/99.75) × 760 = 683.8 mm
This is option (a).
Stream:JEESubject:ChemistryTopic:Chemical EquilibriumSubtopic:Problems involving Kp
⏱ 2mℹ️ Source: QB
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