$$0.4$$ mole of CO taken in a $$2$$ L flask is maintained along with a catalyst at $$812$$ K so that the reaction : $$CO(g)$$ $$+$$ $$2H2(g)$$ ⇌ $$CH3OH(g)$$ can takes place , $$H2$$ is introduced until total pressure of system is $$20$$ atm & $$0.2$$ moles of $$CH3OH$$ is formed at equilibrium then the correct statements among the following:

Question

$$0.4$$ mole of CO taken in a $$2$$ L flask is maintained along with a catalyst at $$812$$ K so that the reaction : $$CO(g)$$ $$+$$ $$2H2(g)$$ ⇌ $$CH3OH(g)$$ can takes place , $$H2$$ is introduced until total pressure of system  is $$20$$ atm & $$0.2$$ moles of $$CH3OH$$ is formed at equilibrium then the correct statements among the following:

Infinity Learn · Accepted Answer

T $$=$$ $$812$$ K ,P $$=$$ $$20$$ atm  , V $$=$$ $$2$$ Lit.$$CO(g)$$    $$+$$         $$2H2(g)$$   →   $$CH3OH(g)$$  $$0.4$$ – x                    $$a-$$ $$2x$$            x $$=$$ $$0.2$$ mol           PV $$=$$ nRT                                a $$=$$ $$0.6$$           Kc $$=$$ $$100$$         $$Kp=Kc$$  (RT)Δn,   In absence of catalyst $$CH3OH$$ formation is negligible. Then total no.of mole  $$=$$ nCO $$+$$ $$nH2$$ $$=$$ $$1$$

Detailed Solution

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