Home
Class 11
CHEMISTRY
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.

Text Solution

AI Generated Solution

To solve the problem, we will break it down into two parts: ### Part A: Calculate \( K_p \) and \( K_c \) 1. **Write the balanced chemical equation:** \[ \text{CO}(g) + \text{H}_2(g) \rightleftharpoons \text{CH}_3\text{OH}(g) \] ...
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY|Exercise Concept Applicationexercise 7.1|53 Videos

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY|Exercise Ex 7.2|40 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY|Exercise Archives Subjective|15 Videos

  • CLASSIFICATION AND NOMENCLATURE OF ORGANIC COMPOUNDS

    CENGAGE CHEMISTRY|Exercise Analytical and Descriptive Type|3 Videos

Similar Questions

Explore conceptually related problems

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.

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) .

For the reaction CO(g)+2H_(2)(g)hArrCH_(3)OH(g) Hydrogen gas is introduced into a five-litre 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 constants K_(p) and K_(c ) .

For the reaction at 127^@ C N_2(g) + 3H_2(g) hArr 2NH_3(g) the partial pressures of N_2 and H_2 are 0.80 and 0.40 atm respectively at equilibrium. The total pressure of the system is 2.80 atm. Calculate K_p and K_c for the reaction.

For the reaction C(s) +CO_(2)(g) rarr 2CO(g), k_(p)=63 atm at 100 K. If at equilibrium p_(CO)=10p_(CO_(2)) then the total pressure of the gases at equilibrium is

For the equilibrium system : CO(g)+2H_2(g)hArr CH_3OH(l) what is K_c ?