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Consider an initial rate experiment for 2A(g) + B(g) --> products: Determine the order of the reaction with respect to A and B and determine a value for k. Experiment initial rate (M/min) [A}O (M) [B]O (M) 1 0.50 0.100 0.100 4.50 0.300 0.100 3 1.00 0.100 0.200 4 4.00 0.200 0.200

Consider an initial rate experiment for 2A(g) + B(g) --> products: Determine the order of the reaction with respect to A and B and determine a value for k. Experiment initial rate (M/min) [A}O (M) [B]O (M) 1 0.50 0.100 0.100 4.50 0.300 0.100 3 1.00 0.100 0.200 4 4.00 0.200 0.200

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Consider an initial rate experiment for 2A(g) + B(g) --> products:

 Determine the order of the reaction with respect to A and B and determine a value for k.

### Initial Rate Experiment for the Reaction 2A(g) + B(g) → Products This experiment aims to determine the order of the reaction with respect to reactants A and B, as well as calculate the rate constant \( k \). #### Experimental Data: | Experiment | Initial Rate (M/min) | \([A]_0\) (M) | \([B]_0\) (M) | |------------|----------------------|----------------|---------------| | 1 | 0.50 | 0.100 | 0.100 | | 2 | 4.50 | 0.300 | 0.100 | | 3 | 1.00 | 0.100 | 0.200 | | 4 | 4.00 | 0.200 | 0.200 | ### Analysis: 1. **Order with respect to A:** - Compare Experiments 1 and 2: Doubling \([A]_0\) from 0.100 M to 0.300 M while keeping \([B]_0\) constant increases the rate from 0.50 M/min to 4.50 M/min. 2. **Order with respect to B:** - Compare Experiments 1 and 3: Doubling \([B]_0\) from 0.100 M to 0.200 M while keeping \([A]_0\) constant increases the rate from 0.50 M/min to 1.00 M/min. By analyzing these changes in initial rates, the respective orders of the reaction with respect to A and B can be determined, followed by calculation of the rate constant \( k \) using the rate law expression.
Transcribed Image Text:### Initial Rate Experiment for the Reaction 2A(g) + B(g) → Products This experiment aims to determine the order of the reaction with respect to reactants A and B, as well as calculate the rate constant \( k \). #### Experimental Data: | Experiment | Initial Rate (M/min) | \([A]_0\) (M) | \([B]_0\) (M) | |------------|----------------------|----------------|---------------| | 1 | 0.50 | 0.100 | 0.100 | | 2 | 4.50 | 0.300 | 0.100 | | 3 | 1.00 | 0.100 | 0.200 | | 4 | 4.00 | 0.200 | 0.200 | ### Analysis: 1. **Order with respect to A:** - Compare Experiments 1 and 2: Doubling \([A]_0\) from 0.100 M to 0.300 M while keeping \([B]_0\) constant increases the rate from 0.50 M/min to 4.50 M/min. 2. **Order with respect to B:** - Compare Experiments 1 and 3: Doubling \([B]_0\) from 0.100 M to 0.200 M while keeping \([A]_0\) constant increases the rate from 0.50 M/min to 1.00 M/min. By analyzing these changes in initial rates, the respective orders of the reaction with respect to A and B can be determined, followed by calculation of the rate constant \( k \) using the rate law expression.
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