Ihave to take this quiz and i only have two questions left i do not want to fail! 1. for the following reaction, it is found that doubling the amount of a causes the reaction rate to double while doubling the amount of b causes the reaction rate to quadruple. what is the best rate law equation for this reaction? a + b -> 2c rate = k[a]2[b] rate = k[a][b] rate = k[a][b]2 rate = k[a]1/2[b] fill in the blank 2. determine the rate law, including the values of the orders and rate law constant, for the following reaction using the experimental data provided. x + y --> products trial [x] [y] rate 1 0.20 m 0.15 m 2.4 × 10-2 m/min 2 0.20 m 0.30 m 4.8 × 10-2 m/min 3 0.40 m 0.30 m 19.2 × 10-2 m/min

1.

2.

x= 2 , y= 1 Total order= 2+1= 3

rate constant (k)=

Explanation:-

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

k= rate constant

x = order with respect to A

y = order with respect to A

On doubling the concentration of A, rate doubles thus order w.r.t A is 1.

On doubling the concentration of B, rate quadruples thus order w.r.t B is 2.

Thus

(2)  

    (1)

   (2)

Dividing 2 by 1

   (2)

   (3)

Dividing 3 by 2

rate law:

Total order = 2+1 = 3

using 1:

answer: - 3.) the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

solution: - as per the rules, oxidation number of oxygen in its compounds is -2. the sum of oxidation numbers of all the elements of a molecule or compound is zero.

also, the oxidation number in elemental form is zero.

in no, the oxidation number of o is -2 so the oxidation number of n is +2 so that the sum is zero.

similarly, the oxidation number of c in co is +2 and o is -2.

on product side the oxidation number of n is 0 as it is in the elemental form() .

oxidation number of c in carbon dioxide is +4 as there are two oxygen in it and we know that each oxygen is -2.

so, oxidation number of n is changing from +2 to 0 and the oxidation number of c is changing from +2 to +4.

since nitrogen is reduced and hence no is acting as an oxidizing agent. carbon is oxidized and so co is acting as a reducing agent.

so, the right choice is number 3.)the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

you did not give any options thus this is the best answer i can give to you with this little information you have given

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