For the gaseous phase reaction $$2A+B$$⇌$$2C+D$$ , initially there are $$2$$ mole each of A & B. If $$0.4$$ mol of D is present at equilibrium at a given T & P, incorrect relationship is

Question

For the gaseous phase reaction $$2A+B$$⇌$$2C+D$$     , initially there are $$2$$ mole each of A & B. If $$0.4$$ mol of D is  present at equilibrium at a given T  & P, incorrect relationship is

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$$2A$$    $$+$$     B   ⇌   $$2C$$   $$+$$  D $$2$$                 $$2$$              $$0$$        $$0$$      Initial (2-2x)    (2-x)        $$2x$$       x      EquilibriumBut D at Equilibrium $$=$$ $$0.4So$$ x $$=$$ $$0.4A=2-2(0.4)=1.2$$ $$B=2-x=2-0.4=1.6$$ $$C=2(0.4)=0.8$$ $$D=0.4$$ PB>PA>PC>PC $$PC=2PD$$ $$PA=3PB4$$

For the gaseous phase reaction $2 A + B ⇌ 2 C + D$ , initially there are 2 mole each of A & B. If 0.4 mol of D is present at equilibrium at a given T & P, incorrect relationship is

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For the gaseous phase reaction 2A+B⇌2C+D , initially there are 2 mole each of A & B. If 0.4 mol of D is present at equilibrium at a given T & P, incorrect relationship is

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For the gaseous phase reaction $2 A + B ⇌ 2 C + D$ , initially there are 2 mole each of A & B. If 0.4 mol of D is present at equilibrium at a given T & P, incorrect relationship is