The equilibrium constant for the reaction $$A2(g)+B2(g)$$⇌$$2AB(g)$$ at $$100$$°C is $$50$$. If a one liter flask containing one mole of $$A2$$ is connected to a $$2$$ litre flask containing two moles of $$B2and$$ allowed to react, the amount of AB formed at equilibrium at $$100$$°C is

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The equilibrium constant for the reaction $$A2(g)+B2(g)$$⇌$$2AB(g)$$ at $$100$$°C is $$50$$. If a one liter flask containing one mole of $$A2$$ is connected to a $$2$$ litre flask containing two moles of $$B2and$$ allowed to react, the amount of AB formed at equilibrium at $$100$$°C is

Infinity Learn · Accepted Answer

$$A2(g)+B2(g)$$⇌$$2AB(g)$$ Initial moles                       $$1$$          $$2$$             $$0$$                                          $$-x$$         $$-x$$        $$+2x$$ At equilibrium              $$1-x$$    $$2-x$$         $$2x$$ Equilibrium constants $$Kc=$$[AB]$$2A2B2$$                                      $$KC=2x321-x32-x3$$                                      $$50=(2x)2(1-x)(2-x)$$ $$50x2-150x+100=0$$                              $$x=0.934$$   Number of moles AB $$=$$ $$2x$$                                         $$=$$ $$1.868$$ moles

The equilibrium constant for the reaction A2(g)+B2(g)⇌2AB(g) at 100°C is 50. If a one liter flask containing one mole of A2 is connected to a 2 litre flask containing two moles of B2and allowed to react, the amount of AB formed at equilibrium at 100°C is

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