`2X(g) rarr 3Y(g)+2Z(g)`
`{:("Time (in min)",0,100,200,):}`
`|{:("Partial pressure of X (mm Hg)",800,400,200,),("Assuming ideal gas condition, calculate",,,,):}|`
(a) Order of reaction
(b) Rate constant
( c) Time taken for `75%` completion of reaction
(d) Total pressure when `p_(x) = 700 mm`

A first order reaction is 20% complete in 10 min . Calculate (a) the specific rate constant of the reaction and (b) the time taken for the reaction to reach 75% completion.

A first order reaction is 20% complete in 10 min . Calculate (a) the specific rate constant of the reaction and (b) the time taken for the reaction to reach 75% completion.

In the following gaseous phase first order reaction A(g) rarr 2B(g)+C(g) initial pressure was found to be 400 mm of Hg and it changed to 1000 mm of Hg after 20min. Then a) half life for A is 10 min b) rate constant is 0.0693 "min"^(-1) c) partial pressure of C at 30 min is 350 mm of Hg d) total pressure after 30 min is 1100 mm of Hg

2A(g)rarr2B(g)+3C(g) is a first order reaction . When the reaction started , the pressure of the system was P_(0) , and it was found to be P_(t) after time t . The rate constant of the reaction can be expressed by the equation -

For the first order reaction A(g) rarr 2B(g) + C(g) , the initial pressure is P_(A) = 90 m Hg , the pressure after 10 minutes is found to be 180 mm Hg . The rate constant of the reaction is

A gaseous compound XY_2 dissociates as: XY_2(g) hArr XY(g) + Y(g) If the initial pressure is 500 mm of Hg and the total pressure at equilibrium is 700 mm of Hg, calculate K_p for the reaction.

XY_(2) dissociates XY_(2)(g) hArr XY(g)+Y(g) . When the initial pressure of XY_(2) is 600 mm Hg, the total equilibrium pressure is 800 mm Hg. Calculate K for the reaction Assuming that the volume of the system remains unchanged.