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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 |
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Answer» 0.0620 atm. `{:("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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