For reaction `Ato` products, initially 8M of A is take. In 20 minutes the concentration of Ais reduced to 4M. In next 10 minutes the concentration of A is reduced to 2M. Report the order of the reaction.

Explanation

To determine the order of the reaction A → products, we can analyze the concentration changes over time. Here’s a step-by-step solution:

### Step 1: Identify Initial and Final Concentrations
Initially, the concentration of A is 8 M. After 20 minutes, the concentration of A is reduced to 4 M. In the next 10 minutes, the concentration further reduces to 2 M.

- Initial concentration (A₀) = 8 M
- Concentration after 20 minutes (A₁) = 4 M
- Concentration after an additional 10 minutes (A₂) = 2 M

### Step 2: Calculate the Change in Concentration
- The change in concentration from A₀ to A₁ over 20 minutes:
\[ \Delta A_1 = A_0 - A_1 = 8 \, \text{M} - 4 \, \text{M} = 4 \, \text{M} \]

- The change in concentration from A₁ to A₂ over the next 10 minutes:
\[ \Delta A_2 = A_1 - A_2 = 4 \, \text{M} - 2 \, \text{M} = 2 \, \text{M} \]

### Step 3: Determine the Rate of Reaction
The rate of reaction can be expressed as the change in concentration over time.

- For the first interval (20 minutes):
\[ \text{Rate}_1 = \frac{\Delta A_1}{\Delta t_1} = \frac{4 \, \text{M}}{20 \, \text{min}} = 0.2 \, \text{M/min} \]

- For the second interval (10 minutes):
\[ \text{Rate}_2 = \frac{\Delta A_2}{\Delta t_2} = \frac{2 \, \text{M}}{10 \, \text{min}} = 0.2 \, \text{M/min} \]

### Step 4: Analyze the Rates
Since the rates of change of concentration are constant over the two intervals, we can conclude that the reaction does not depend on the concentration of A. This is indicative of a zero-order reaction.

### Step 5: Conclusion
From the analysis, we find that the reaction is of zero order.

### Final Answer
The order of the reaction is **0**.

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