Advertisements
Advertisements
प्रश्न
How will you represent first order reactions graphically.
Advertisements
उत्तर
i. The differential rate law for the first-order reaction A → P is 
The equation is of the form y = mx + c. A plot of rate versus [A]t is a straight line passing through the origin. The slope of straight line = k.
 |
| Variation of rate with [A] |
ii. The integrated rate law is
k = `2.303/t log_10 ["A"]_0/["A"]_"t"`
On rearrangement, the equation becomes
`(kt)/2.303 = log_10 ["A"]_0 - log_10 ["A"]_"t"`
Hence,
The equation is of the straight line. A graph of `log_10[A]_t` versus t yields a straight line with slope `-"k"/2.303` and y-axis intercepts as log10[A]0.
 |
| Variation of `log_10 [A]_t` with time |
iii. Rearranging the integrated rate law equation, we get
The equation has a straight-line form y = mx. Hence, the graph of `log_10 ([A]_0)/([A]_t)` versus t is a straight line passing through the origin.
 |
| Variation of `log_10 ([A]_0)/([A]_t)` with time |
APPEARS IN
संबंधित प्रश्न
Answer the following in one or two sentences.
How do the half-lives of the first order and zero-order reactions change with the initial concentration of reactants?
Answer the following in brief.
Obtain the relationship between the rate constant and half-life of a first-order reaction.
Answer the following in brief.
Derive the integrated rate law for the first-order reaction.
Answer the following in brief.
What are the units of the rate constant?
Time required for 100% completion of a zero order reaction is _______.
Write a mathematical expression for integrated rate law for zero-order reaction.
For the reaction 2NOBr → 2NO2 + Br2, the rate law is rate = k[NOBr]2. If the rate of a reaction is 6.5 × 10–6 mol L–1 s–1, when the concentration of NOBr is 2 × 10–3 mol L–1. What would be the rate constant of the reaction?
The rate constant of the first order reaction is 1.386 min–1. Calculate the time required for 80% reactant to decompose?
Derive an expression for the relation between half-life and rate constant for first-order reaction.
For a first-order reaction, the rate constant is 6.909 min−1 the time taken for 75% conversion in minutes is
Describe the graphical representation of first order reaction.
A first order reaction has a rate constant 0.00813 min-1. How long will it take for 60% completion?
The rate of the reaction \[\ce{A + B -> C}\] is 3.6 × 10−2 mol dm−3 s−1 when [A] = 0.3 mol dm−3 and [B] = 0.2 mol dm−3. Calculate k if reaction is first order in A and zero order in B.
The rate constant of a reaction has same units as the rate of reaction. The reaction is of ____________.
If [A] is the concentration of A at any time t and [A]0 is the concentration at t = 0, then for the 1st order reaction, the rate equation can be written as ____________.
The activation energy of a reaction is zero. Its rate constant at 280 K is 1.6 × 10-6 s-1, the rate constant at 300 K is ______.
Half-life period of a first order reaction, \[\ce{A -> product}\] is 3.0 hours. What is the value of rate constant?
The slope of a graph, log [A]t versus 't' for a first order reaction is −2.5 × 10−3 s−1. The rate constant for the reaction is ____________.
The half-life of a first order reaction is 6.0 hour. How long will it take for the concentration of reactant to decrease from 0.4 M to 0.12 M?
Which among the following is an example of zero order reaction?
Which among the following is an example of pseudo first order reaction?
A first order reaction takes 40 minutes for 30% decomposition. What is the half-life of reaction?
The time required to decompose SO2Cl2 to half of it's initial amount is 60 minutes. Calculate rate constant for this first order reaction.
Rate constant for zero order reaction is 2 × 10-2 mol L-1 s-1. If the concentration of the reactant after 25 sec. is 0.5 M, what is the initial concentration of reactant?
Which one of the following reactions is a true first-order reaction?
The rate constant for a first order reaction is 7.0 × 10-4 s-1. If initial concentration of reactant is 0.080 M, what is the half-life of reaction?
The half-life period for the first order reaction is 1.7 hrs. How long will it take for 20% of the reactant to disappear?
