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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 isA. 0.0620 atm.B. 0.0310 atm.C. 0.0582 atm.D. 0.2610 atm. |
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Answer» Correct Answer - C `"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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