1a. A proposed mechanism is: 1) 2 A + B → C (slow) 2) C → A...

1a. A proposed mechanism is:

1) 2 A + B → C (slow)

2) C → A + D (fast)

If this mechanism is correct, by what numerical factor should the rate of reaction increase if [A] is increased by a factor of (6.57x10^0)?

1b. A first-order reaction has a half-life of (5.30x10^1) minutes. How many minutes would it take for the only reactant to decrease to 12.5% of its initial concentration?

1c. A reaction has an activation energy of 125.0 kJ/mol. At 310. K, the rate constant is (6.09x10^-4) s^-1. What would be the value of the rate constant in s^-1 at 300. K?

1d. A reaction is known to follow first-order kinetics and has a rate constant of (6.260x10^-2) min^-1. If the initial concentration of the only reactant is (1.44x10^0) M, what will be the concentration after (5.150x10^1) minutes?

1e. A reaction is known to follow first-order kinetics. What is the half-life (in seconds) if it takes (7.110x10^2) seconds for the concentration of the only reactant to drop from (3.790x10^0) M to (3.83x10^-1) M?

Will rate. Due in 30 min, Please answer it all. Thank you.

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Expert Solution

queen_honey_blossom answered 1 year ago

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