Consider the reaction A+2BC whose rate at 25 C was measured using three differen

Question

Consider the reaction A+2BC whose rate at 25 C was measured using three different sets of initial concentrations as listed in the following table: Trial [A] (M) [B] (M) Rate (M/s) 1 0.10 0.050 6.0×104 2 0.10 0.100 1.2×103 3 0.20 0.050 2.4×103 Part A What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B]. rate = k[A]2[B]

Part B Calculate the initial rate for the formation of C at 25 C, if [A]=0.50M and [B]=0.075M. Express your answer to two significant figures and include the appropriate units.

Explanation / Answer

now calculate the rate constant using first equation

rate = k[A]2[B]

take the first row from table it not necessary you can take any

6.0×104 = K[0.1]2[0.05]

K = 6.0×104 / 5*10^-4

K = 1.2 mol-2 lit2 sec-1

now use the same equation

substitute the given concentration and use the same K value find the rate constant

rate = k[A]2[B]

rate = 1.2 [0.5]2[0.075]

= 0.0225 M/S

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