For the decomposition reaction
`NH_2COONH_4(s) hArr 2NH_3(g) +CO_2(g)`
the `K_p =2.9 xx 10^(-5) "atm"^3`. The total pressure of gases at equilibrium when 1 mole of `NH_2COONH_4` (s) was taken to start with would be

For the decomposition reaction: NH_(2)COONH_(4(s))hArr2NH_(3(g))+CO_(2(g)) . (K_(p)=2.9xx10^(-5)atm^(2)) The total pressure of gases at equilibrium when 1 "mole" of NH_(2)COONH_(4(s)) was taken to start with would be:

For the decomposition reaction NH_(2)COONH_(4)(s) hArr2NH_(3)(g)+CO_(2)(g) , the K_(p)=3.2xx10^(-5)atm^(3) . The total pressure of gases at equilibrium when 1.0 mol of NH_(2)COONH_(4)(s) was taken to start with will be:

For the decomposition reaction NH_(2)COONH_(4)(s) hArr2NH_(3)(g)+CO_(2)(g) , the K_(p)=3.2xx10^(-5)atm^(3) . The total pressure of gases at equilibrium when 1.0 mol of NH_(2)COONH_(4)(s) was taken to start with will be:

For the reaction NH_(2)COONH_(4)(g)hArr 2NH_(3)(g)+CO_(2)(g) the equilibrium constant K_(p)=2.92xx10^(-5)atm^(3) . The total pressure of the gaseous products when 1 mole of reactant is heated, will be

For the reaction NH_(2)COONH_(4)(g)hArr 2NH_(3)(g)+CO_(2)(g) the equilibrium constant K_(p)=2.92xx10^(-5)atm^(3) . The total pressure of the gaseous products when 1 mole of reactant is heated, will be

Unit of K_p for NH_4COONH_(2(s)) harr 2NH_(3(g))+ CO_(2(g)) is

For the following reaction : NH_(2) COO NH_(4) (s) hArr 2 NH_(3) (g) + CO_(2) (g) If the total pressure of the system at equilibrium is 3 atm , then the value of K_(p) will be -

Peqfor NH_(4)COONH_(2(s)) harr 2NH_(3(g))+ CO_(2(g)) at certain temperature is 0.9 atm. Then, partial pressure of Ammonia at equilibrium (in atm)

Solid ammonium carbamate dissociated according to the given reaction NH_2COONH_4(s) hArr 2NH_3(g) +CO(g) Total pressure of the gases in equilibrium is 5 atm. Hence K_p .