Kinetics of the reaction A (g)to 2" B"(g)+C(g) is followed by measuring the total pressure at different times. It is given that Initial pressure of A = 0.5 atm. Total pressure of A after 2 hours = 0.7 atm. Rate constant of the reaction =1xx10^(-3)s^(-1) What is the rate of reaction -(d[A])/(dt) when the total pressure is 0.7 atm ?

Kinetics of the reaction A (g)to 2" B"(g)+C(g) is followed by measurin

1.	Kinetics of the reaction A (g)to 2" B"(g)+C(g) is followed by measuring the total pressure at different times. It is given that Initial pressure of A = 0.5 atm. Total pressure of A after 2 hours = 0.7 atm. Rate constant of the reaction =1xx10^(-3)s^(-1) What is the rate of reaction -(d[A])/(dt) when the total pressure is 0.7 atm ?
Answer» `2.0xx10^(-4)" M s"^(-1)` `4.0xx10^(-4)" M s"^(-1)` `5.0xx10^(-4)" M s"^(-1)` `7.0xx10^(-4)" M s"^(-1)` Solution :`{:(,2A(g),to, 2B(g),+,C(s)),("Initial",,05" atm",,,),("After 2 hours",,05-p,,2p, p):}` Total PRESSURE after 2 hours `= (05 -p) + 2 p + p` `=05 + 2p` `therefore 05 + 2p = 07orp = 01` atm `therefore` Pressure of A after 2 hours `= 05 - 01 = 04` atm RATE CONSTANT in `s^(-1)` shows that it is a reaction of 1st order. `therefore` Rate after 2 hours `= k[A]= k P` `= (10^(-3)s^(-1))(04 " atm ") = 40 xx 10^(-4) " atm " s^(-1).`