Question

In the first order decomposition of A : A  2B + 3C Concentration of A decrease from initial concentration 0.8M to 0.2M in 13.86 min. then calculate rate of appearance of B (in M/s) after 13.86 m​

Answer 1

Given info : in the first order decomposition of A : A ⇒2B + 3C. concentration of A decrease from 0.8M to 0.2 M in 13.86 min.

To find : the rate of appearance of B after 13.86 min is ...

solution : reaction is A ⇒2B + 3C

∴ - d[A]/dt = +1/2 d[B]/dt = +1/3 d[C]/dt

means, rate of disappearance of A = 1/2 × rate of appearance of B ....(1)

a/c to question, concentration of A decreases from 0.8M to 0.2 M in 13.86 min.

so, rate of disappearance of A = - (0.2 - 0.8)/13.86 M/min = 0.6/13.86 M/min

now rate of appearance of B = 2 × rate of disappearance of A [ from eq (1). ]

= 2 × 0.6/13.86 = 1.2/13.86 = 0.0866 M/min = 0.0866/60 M/sec = 0.00144 M/s

Therefore the rate of appearance of B is 0.00144 M/s

also read similar questions : for the reaction A + 2B equilibrium to C + D at a certain temperaturewhere concentration of c equal to concentration of ...

https://brainly.in/question/13132373

Equal volumes of 0.1 M AgMO3 and 0.2M NaCl are mixed. The concentration of NO³- ions in the mixture will be??

https://brainly.in/question/3504462