|Class 12 Chemistry Chemical Kinetics||First order reaction|
First order reaction
If the rate of reaction depends on the concentration of single reactant participating in chemical reaction raised to the first power then it is called a first order reaction.
A --> B
At time t = 0 concentration of A (reactant) is a and B (product) is 0. At time t = t the concentration of A (reactant) is (a-x) and that of B (product) is x.
-dx/dt ∝ (a-x) = dx/dt = k1(a-x)
∫ 0x dx/(a-x) = k1∫ 0t dt
dx/dt = k0(a-x)0
dx/dt = k0
∫0 x dx = k0∫ 0t dt
ln (a/a-x) = k1t => t = 1/ k1 ln (a/a-x) = 2.303/ k1 log (a/a-x)
k1 = 2.303 log (a/a-x)
PROBLEM. A first order reaction has a rate constant 1.15 10-3s-1. How long will 5 g of this reactant take to reduce to 3 g?
SOLUTION. From the question, we can write down the following information:
Initial amount = 5 g
Final concentration = 3 g
Rate constant = 1.15 10 - 3s - 1
We know that for a 1st order reaction,
t = (2.303/k)log[R0]/[R]
(2.303/1.15X10-3) X 0.2219 = 444.38 s = 444 s