Table of Contents
- 1 How long will it take for the concentration of so2cl2 to decrease to 25\% of its initial concentration?
- 2 Is the decomposition of hydrogen peroxide a first-order reaction?
- 3 What is the rate law for the decomposition of SO2Cl2?
- 4 What is the half-life for this reaction SO2Cl2?
- 5 How many half lives are required for the concentration of reactant to decrease to 25?
- 6 For what order reaction does the half-life get longer as the initial concentration increases?
How long will it take for the concentration of so2cl2 to decrease to 25\% of its initial concentration?
FREE Expert Solution. Thus, the time it takes for the concentration of SO2Cl2 to decrease to 25\% of its initial concentration is 9625 s.
Is the decomposition of hydrogen peroxide a first-order reaction?
Hydrogen peroxideThe decomposition of hydrogen peroxide to form oxygen and hydrogen is a first-order reaction.
What is the effect of reactant concentration on the half-life of a first-order reaction?
For a first-order reaction, the concentration of the reactant decreases by a constant with each half-life and is independent of [A].
What is the half-life for a first-order reaction?
The half-life of a first-order reaction is a constant that is related to the rate constant for the reaction: t1/2 = 0.693/k. Radioactive decay reactions are first-order reactions. The rate of decay, or activity, of a sample of a radioactive substance is the decrease in the number of radioactive nuclei per unit time.
What is the rate law for the decomposition of SO2Cl2?
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42×10-4 s-1.
What is the half-life for this reaction SO2Cl2?
Question: The first-order reaction, SO2Cl2 → SO2 + Cl2, has a half-life of 8.75 hours at 593 K.
Are decomposition reactions always first order?
In the atmosphere, photolysis reactions obey first-order kinetics. Also, unimolecular decomposition reactions at their high-pressure limit empirically follow first-order kinetics.
What is the equation for first order reaction?
The integrated rate law for the first-order reaction A → products is ln[A]_t = -kt + ln[A]_0. Because this equation has the form y = mx + b, a plot of the natural log of [A] as a function of time yields a straight line.
How many half lives are required for the concentration of reactant to decrease to 25?
Thus the half-life of a reaction is the time required for the reactant concentration to decrease from [A] 0 to [A] 0/2….Half-Lives.
| Number of Half-Lives | Percentage of Reactant Remaining | |
|---|---|---|
| 1 | 100\%2=50\% | 12(100\%)=50\% |
| 2 | 50\%2=25\% | 12(12)(100\%)=25\% |
| 3 | 25\%2=12.5\% | 12(12)(12)(100\%)=12.5\% |
| n | 100\%2n | (12)n(100\%)=(12)n\% |
For what order reaction does the half-life get longer as the initial concentration increases?
Zero-Order Reaction
Half-Life for a Zero-Order Reaction As initial concentration increases, the half-life for the reaction gets longer and longer.
What is the half-life for the first order decay of carbon 14?
5720 years
Carbon-14 is decaying constantly with a half-life of 5720 years.
What is second order of reaction?
A second order reaction is a reaction where x + y = 2. This can happen if one reactant is consumed at a rate proportional to the square of the reactant’s concentration (rate = k[A]2) or both reactants are consumed linearly over time (rate = k[A][B]).