What is the order of the reaction for the following reaction and for each reagen

Question

What is the order of the reaction for the following reaction and for each reagent given?

2. Determine the rate of the chemical reaction shown directly below, given an NO

concentration of 12.0 x 10?3 M, an H2 concentration of 3.0 x 10?3 M, and a rate constant k of 2.5 x 102M?2s?1

The rate law for this reaction is rate = k [NO]2[H2] 2NO + 2H2 ? N2 + 2H2

3. Write the rate law for the general reaction given by aA + bB ? cC + dD

4. a) What is the purpose of using Iodine (and not some other halogen) in this reaction? b) Why is the concentration of iodine so much lower than the other reactants?

b) Why is the concentration of iodine so much lower than the other reactants?

exp a b c rate 1 0.002 0.15 0.132 0.0057 2 0.002 0.25 0.132 0.0158 3 0.003 0.15 0.132 0.0114 4 0.003 0.15 0.246 0.0114

Explanation / Answer

1)   rate = K [ a]^x [b]^y [c]^z

now consider exp 1 and 3 , b and c are constante

rate 1 / rate 3 = [a1/a2]^x

0.0057 / 0.0114 = [ 0.002/0.003]^x

(2/3)^x = 0.5

x= 1.5

so the order with respect to a is 1.5

now consider exp 1 and 2 , a and c are constant

rate 2 / rate 1 = ( b2/b1 )^y

0.0158/ 0.0057 = ( 0.25/0.15)^y

y = 2

so the order with respect to b is 2

now consider exp 3 and 4 , a and b are constant

rate 4 / rate 3 = ( c4/c3)^z

0.0114/0.0114 = ( 0.246 / 0.132)^z

z = 0

so the order with respect to c is 0

so the overall order = 1.5 + 2 + 0 = 3.5

2)   rate = k [ N0]2 [H2]

rate = 2.5 x 100 x [ 12 x 10-3]2 [ 3 x 10-3]

rate = 1.08 x 10-4

so the rate is 1.08 x 10-4

3) aA + bB ---> cC + dD

rate law is

rate = K [ A]^a [ B]^b

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