Home
Class 11
CHEMISTRY
4.4 grams of CO(2) are introduced into a...

4.4 grams of `CO_(2)` are introduced into a 0.82 L flask containing excess solid carbon at `627^(circ)C`, so that the equilibrium:
The density of equilibrium gaseous mixture corresponds to an average molecular weight of 36.
`K_(p)=P_(CO)^(2)/P_(CO_2)and K_(C)([CO]^(2))/([CO_(2)])`
`[R=0.082"Lt-atm/mol-K",C=12,0=16]`
Total number of moles of equilibrium gaseous mixture is :

A

`(1)/(30)`

B

`(2)/(15)`

C

`(1)/(15)`

D

`(1)/(10)`

Text Solution

Verified by Experts

The correct Answer is:
D
Promotional Banner

Similar Questions

Explore conceptually related problems

4.4 grams of CO_(2) are introduced into a 0.82 L flask containing excess solid carbon at 627^(circ)C , so that the equilibrium: The density of equilibrium gaseous mixture corresponds to an average molecular weight of 36. K_(p)=P_(CO)^(2)/P_(CO_2)and K_(C)([CO]^(2))/([CO_(2)]) [R=0.082"Lt-atm/mol-K",C=12,0=16] K_(p) of the reaction C(s) +CO_(2)(g)hArr2CO(g) is :

4.4 grams of CO_(2) are introduced into a 0.82 L flask containing excess solid carbon at 627^(circ)C , so that the equilibrium: The density of equilibrium gaseous mixture corresponds to an average molecular weight of 36. K_(p)=P_(CO)^(2)/P_(CO_2)and K_(C)([CO]^(2))/([CO_(2)]) [R=0.082"Lt-atm/mol-K",C=12,0=16] If in the problem,where actually 1.2g of solid carbon is present initially, how many total moles of CO_(2) would have to be inroduced initiallly so that at equilibrium only a trace of carbon remained?

If partial pressure of N_2 in gaseous mixture containing equal mass of CO and N_2 is 0.5 atm then the total pressure of gaseous mixture is

At 540 K, 0.10 mol of PCl_(5) is heated in a 8L flask. The pressure of equilibrium mixture is found to be 1.0 atm . Calculate K_(p) and K_(c ) for the reaction.

A mixture of 4 moles H_(2)O and 1 mole CO is allowed to react to come to an equilibrium. The equilibrium pressure is 2.0 atm. Calculate partial pressure (in atm) of CO(g) at equilibrium. H_(2)O (g) + CO(g) harr CO_(2) (g) + H_(2) (g); K_(C) =0.5 Use sqrt(41) = 6.4

Consider the following heterogeneous equilibrium, CaCO_(3)(s)CaO(s)+CO_(2)(g) . At 800^(@)C , the pressure of CO_(2) is 0.236 atm. The value of K_(c) for the abvoe given equilibrium reaction at this temperature is