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When 0.15 mol of CO taken in a 2.5 L fla...

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.

Text Solution

AI Generated Solution

To solve the given problem step by step, we will break it down into parts as requested. ### Given Data: - Moles of CO = 0.15 mol - Volume of flask = 2.5 L - Temperature = 750 K - Total pressure at equilibrium = 8.5 atm - Moles of methanol formed (CH₃OH) = 0.08 mol ...
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