1.

The value of K_(p) for the reaction NH_(2)COONH_(4)(s) hArr2NH_(3)(g)+CO_(2)(g)" is "2.9xx10^(-5)"atm"^(3). The total pressure of gases at equilibrium when NH_(2)COONH_(4)(s) is taken to start the reaction at the initial concentration of 1.0 mole is

Answer»

0.0620 atm.
0.0310 atm.
0.0582 atm.
0.2610 atm.

Solution :`"The reaction is",NH_(2)COONH_(4)(s)hArr2NH_(3)(g)+CO_(2)(g)`
`{:("Initial conc.",1.0"mole",,0,,0),("EQM. conc.",0,,2,,1):}`
Let P be the equilibrium pressure then the PARTIAL pressure of ammonia `=(2)/(3)P` and the of carbon dioxide is `(1)/(3)P`.
Or`""K_(p)=[(2P)/(3)]^(2)[(P)/(3)]=(4P^(3))/(27)`
Or `""2.9xx10^(-5)=(4P^(3))/(27)" or "4P^(3)=27xx2.9xx10^(-5)`
Or `""P=root(3)((27xx2.9xx10^(-5))/(4))`
Or `""P=0.0582" atm. "`


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