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0.25 mol of CO taken in a 1.5 L flask is...

`0.25` mol of `CO` taken in a `1.5 L` flask is maintained at `500 K` along with a catalyst so that the following reaction can take place:
`CO(g)+H_(2)(g)hArrCH_(3)OH(g)` .
Hydrogen is introduced until the total pressure of the system is `8.2 atm`, at equilibrium, and `0.1 mol` of methanol is formed. Calculate
a. `K_(p)` and `K_(c )`
b. The final pressure if the same amount of `CO` and `H_(2)` as before are used but no catalyst so that the reaction does take place.

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0.25 mol of CO taken in a 1.5 L flask is maintained at 500 K along with a catalyst so that the following reaction can take place: CO(g)+H_(2)(g)hArrCH_(3)OH(g) . Hydrogen is introduced until the total pressure of system is 8.2 atm , at equilibrium, and 0.1 mol of methanol is formed. Calculate a. K_(p) and K_(c ) b. The final pressure if the same amount of CO and H_(2) as before are used but no catalyst so that the reaction does take place.

When 0.15 mol of CO taken in a 2.5 L flask is maintained at 750 K along with a catalyst, the following reaction takes place CO(g)+2H_(2)(g) hArr CH_(3)OH(g) Hydrogen is introduced until the total pressure of the system is 8.5 atm at equilibrium and 0.08 mol of methanol is formed. Calculate a. K_(p) and K_(c) b. The final pressure, if the same amount of CO and H_(2) as before are used, but with no catalyst so that the reaction does not take place.

When 0.15 mol of CO taken in a 2.5 L flask is maintained at 750 K along with a catalyst, the following reaction takes place CO(g)+2H_(2)(g) hArr CH_(3)OH(g) Hydrogen is introduced unit the total pressure of the system is 8.5 atm at equilibrium and 0.08 mol of methanol is formed. Calculate a. K_(p) and K_(c) b. The final pressure, if the same amount of CO and H_(2) as before are used, but with no catalyst so that the reaction does not take place.

Find the relation betweenn K_(p)&K_(c) for the given reactions: CO(g)+2H_(2)(g)hArrCH_(3)OH(l) .

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For the reaction CO(g)+2H_(2)(g) hArr CH_(3)OH(g) hydrogen gas is introduced into a 5-L flask at 327^(@)C containing 0.2 mol of CO(g) and a catalyst, untill the pressure is 4.92 atm. At this point, 0.1 mol of CH_(3)OH(g) is formed. Calculate the equilibrium constant K_(p) and K_(c) .