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### Training Questions

1. **First-order reaction:**
- The reaction is 40% complete after 50 minutes. Calculate the rate constant \( K \) per second.
- In how many minutes will the reaction be 80% complete?

2. **First-order reaction:**
- After 50 seconds, 32.5% of the reactive material remains. Calculate the rate constant \( K \).
- How much time does it take until only 25% of the reactive material remains?

3. **First-order reaction:**
- The half-life is 30 minutes. Calculate the rate constant \( K \) per second.
- What is the remaining amount of reactive material after 70 minutes?

4. **Industrial counterpart degradation:**
- It degrades according to the law of first-order reactions.
- If the half-life is 50 minutes, what is the time needed for 80% decomposition?

5. **Second-order reaction:**
- The reaction is 20% complete in 40 minutes. Given an initial concentration of the reactant of 0.1 mol/L, calculate the rate constant \( K \).
- Calculate the time required for the disappearance of half of the initial concentration.
- Given an initial concentration of the reactant of 0.01 mol/L, calculate the time required for 20% completion.

6. **Reaction kinetics:**
- Equal amounts of material A and B are added to a liter of solvent. After 500 seconds, half of A has reacted. Calculate the amount of substance A that reacts after 800 seconds given the following scenarios:
- Zero-order reaction of substance A.
- First-order reaction of substance A, independent of B.
- Second-order reaction of A and B, if the concentrations of A and B are equal.

Answer :

Final answer:

In the subject of chemistry, the rate of first-order and second-order reactions can be calculated using specific formulas. The half-life of a first-order reaction is independent of initial reactant concentration, while for a second-order reaction, it is directly proportional. Rate constants and remaining concentrations can also be calculated using their respective formulas.

Explanation:

These series of questions pertain to the concepts of first-order reactions and second-order reactions in the subject of chemistry. Reaction order is integral to understanding the kinetics of a chemical reaction, which tells us how the rate of a reaction changes with change in concentration. To answer these questions, we need to apply the appropriate formula for first order and second order reactions, depending on the question.

For a first order reaction, the half-life is independent of the initial concentration of the reactant, and the rate constant (K) can be calculated using the formula K=0.693/half-life. To find the remaining concentration after a certain period, we can use the formula [A] = [A]0 * e^(-kt), where [A] is the remaining concentration, [A]0 is the initial concentration, k is the rate constant and t is the time.

For a second order reaction, the half life is dependent on the initial concentration and can be calculated by the formula t1/2 = 1 / (k[A]0), where [A]0 is the initial concentration and k is the rate constant. To find the rate constant k, we need the initial concentration of the reactant and the time required for a certain percentage of reaction to complete. The integrated rate equation for second order reactions, 1/[A] = kt + 1/[A]0, can also be used to solve some of these problems.

Learn more about Chemical Kinetics here:

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