For a reaction a + b → products, the following data were collected. experiment number initial concentration of a (m) initial concentration of b (m) observed initial rate (m/s) 1 3.40 4.16 1.82 ✕ 10−4 2 4.59 4.16 3.32 ✕ 10−4 3 3.40 5.46 1.82 ✕ 10−4 calculate the rate constant for this reaction.

Rate constant k = 1.57*10⁻⁵ s⁻¹

Explanation:

Given reaction:

Expt    [A] M        [B] M         Rate [M/s]

1          3.40         4.16           1.82*10^-4

2         4.59         4.16           3.32*10^-4

3.        3.40          5.46          1.82*10^-4

where k = rate constant

x and y are the orders wrt to A and B

To find x:

Divide rate of expt 2 by expt 1

To find y:

Divide rate of expt 3 by expt 1

Therefore: x = 2, y = 0

To find k

Use rate for expt 1:

girl imma just put my comment here because i need a couple point okurrttt

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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