For the reaction x2 + y + z -> xy + xz it is found that doubling the concentration of x2 doubles the reaction rate. triplingthe concentration on triples the rate, and doubling the concentration of 2 has no effect, (a) what is the rate law for thisreaction? (b) why is it that the change in the concentration of 2 has no effect on the rate? (c) suggest a mechanism for thereaction that is consistent with the rate law.

(a) R=k[X2][Y] (b) reaction is zero order wrt Z (c) X2 + Y --- XY +  X (slow step)

X + Z --- XZ    (fast step)

Explanation:

(a) Suppose the reaction rate R with respect to a component X2 with concentration [X2] is generally expressed as follows:

R = k [X2]^n                     (1)

Where k is the rate constant and n is the order of reaction with respect to X2.

When the reaction rate is found to double by doubling the concentration of X2, the following equation could be developed:

2R = k *(2[X2])^n           (2)

Dividing equation (2) by (1) yields

2R/R= k *(2[X2])^n / k *[X2]^n  

2=2^n , n = 1

Thus, the reaction is first order with respect to X2.

In the same manner,  

Tripling the concentration of Y triples the rate,  

R = k [Y]^m                     (3)

Where k is the rate constant and m is the order of reaction with respect to Y.

When the reaction rate is found to triple by tripling the concentration of Y, the following equation could be developed:

2R = k *(3[Y])^m           (4)

Dividing equation (4) by (3) yields

3R/R= k *(3[Y])^m / k *[Y]^m  

3=3^m  , m = 1

Thus, the reaction is first order with respect to Y.

Therefore,the rate law for this reaction is R = k [X2] [Y]

(b)

Provided that doubling the concentration of Z has no effect, we perform similar analysis as above with p representing order of reaction wrt Z:  

R = k [Z]^p                     (5)

R = k (2*[Z]^p                     (6)

R/R= k *(2[Z])^p / k *[Z]^p  

1=2^p  , p = 0

Thus, the reaction is zero order wrt Z. This explains why the change in concentration has no effect on the rate.

(c) A suggested mechanism for the reaction that is consistent with the rate law will therefore be

X2 + Y  XY +  X (slow step)

X + Z XZ    (fast step)

The rate law is determined by the slow step, and this is very consistent with the experimentally observed data.

Besides, addition of the two step yields the overall reaction, and both steps are reasonable.

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g

3 1/4 %

explanation: