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for the first order reaction A(g) ------: 2B(g) +C(g) the initial pressure is Pa= 90 mm hg and pressure after 10 min. is 180 mm of hg. find the rate constant.ans is 1.15*10^-3
for the first order reaction
A(g) ------: 2B(g) +C(g)
the initial pressure is Pa= 90 mm hg and pressure after 10 min. is 180 mm of hg. find the rate constant.ans is 1.15*10^-3
A => 2B + C p 0 0 (initial) (at t=0) P-Po 2Po Po (final) (at t =10) initial total pressure = P = 90mm final total pressure = 180mm from eq adding all presures we get total pressure = P + 2Po P + 2Po = 180 90 + 2Po = 180 Po = 45 for A , initially pressure = P= 90 final pressure = P-Po = 90-45 = 45 rate constant (k) = 2.303 log(Pi/Pf) / t = 2.303 log90/45 / t =(2.303)log2/10 k = 0.069 min-1 this value of rate constant is in min-1 , 1min = 60sec so K = 0.069/60 sec-1 = 1.15*10-3 sec-1 approve if u like my ans
A => 2B + C
p 0 0 (initial) (at t=0)
P-Po 2Po Po (final) (at t =10)
initial total pressure = P = 90mm
final total pressure = 180mm
from eq adding all presures we get total pressure = P + 2Po
P + 2Po = 180
90 + 2Po = 180
Po = 45
for A , initially pressure = P= 90
final pressure = P-Po = 90-45 = 45
rate constant (k) = 2.303 log(Pi/Pf) / t
= 2.303 log90/45 / t
=(2.303)log2/10
k = 0.069 min-1
this value of rate constant is in min-1 , 1min = 60sec so
K = 0.069/60 sec-1 = 1.15*10-3 sec-1
approve if u like my ans
Dear student.,
Write the rate of reation in terms of pressure
r=(2.303log P/Po)/time
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