Given the data calculated in parts a, b, c, and d, determine the initial rate for a reaction that starts with 0.85 m of reagent a and 0.70 m of reagents b and c? express your answer to two significant figures and include the appropriate units. indicate the multiplication of units explicitly either with a multiplication dot or a dash. trial [a] (m) [b] (m) [c] (m) rate1 0.2 0.2 0.2 6.1x10^-52 0.2 0.2 0.6 1.8x10^-43 0.4 0.2 0.2 2.4x10^-44 0.4 0.4 0.2 2.4x10^-4

Answer : The initial rate for a reaction will be

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

The chemical equation will be:

Rate law expression for the reaction:

where,

a = order with respect to A

b = order with respect to B

c = order with respect to C

Expression for rate law for first observation:

....(1)

Expression for rate law for second observation:

....(2)

Expression for rate law for third observation:

....(3)

Expression for rate law for fourth observation:

....(4)

Dividing 1 from 2, we get:

Dividing 1 from 3, we get:

Dividing 3 from 4, we get:

Thus, the rate law becomes:

Now, calculating the value of 'k' by using any expression.

Putting values in equation 1, we get:

Now we have to calculate the initial rate for a reaction that starts with 0.85 M of reagent A and 0.70 M of reagents B and C.

Therefore, the initial rate for a reaction will be

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explanation: