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The concentration of reactant undergoing decomposition was o.1 ,0.08 and 0.067mol/L after 1.0,2.0,and 3.0 hr respectively.the order of reaction.?
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The concentration of reactant undergoing decomposition was o.1 ,0.08 a...
Analyzing the Reaction Order
To determine the order of the reaction, we can use the concentration data provided at various time intervals. The concentrations of the reactant are:
- At 1.0 hr: 0.1 mol/L
- At 2.0 hr: 0.08 mol/L
- At 3.0 hr: 0.067 mol/L
Calculating the Change in Concentration
- From 1.0 hr to 2.0 hr:
- Change = 0.1 - 0.08 = 0.02 mol/L
- From 2.0 hr to 3.0 hr:
- Change = 0.08 - 0.067 = 0.013 mol/L
Determining the Rate of Change
- Average rate from 1.0 hr to 2.0 hr:
- Rate = Change in concentration / Change in time = 0.02 / 1 = 0.02 mol/L/hr
- Average rate from 2.0 hr to 3.0 hr:
- Rate = Change in concentration / Change in time = 0.013 / 1 = 0.013 mol/L/hr
Order of Reaction Calculation
To find the order of the reaction, we can compare the rates of change with respect to the concentration.
If we assume a first-order reaction:
- The rate of reaction is proportional to the concentration of the reactant.
- A decrease in concentration will yield a corresponding decrease in the rate.
Since the rate decrease is not constant and appears to diminish over time, it suggests the reaction is not first-order.
Conclusion
The observed data indicates that the reaction follows a second-order kinetics:
- The rate decreases more significantly as the reaction progresses, suggesting that the reaction order is higher than one.
In summary, the reaction is likely a second-order reaction based on the concentration changes over time.
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The concentration of reactant undergoing decomposition was o.1 ,0.08 and 0.067mol/L after 1.0,2.0,and 3.0 hr respectively.the order of reaction.?
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