Given the rate equation... RATE = ([ Na 2 S 2 O 3 ]/time) = k [I - ] a [BrO 3 -

Question

Given the rate equation...
RATE = ([ Na2S2O3]/time) = k [I-]a [BrO3-]b [HCl]c
1A) You mix together in the proper manner the following:

The time to turn blue is... 56 sec

1B) You also mix together in the proper manner the following:

The time to turn blue is... 15 sec
Calculate:
The Experimental value of exponent b..._______________ (a)

2) If the exponents a, b, and c have the values:
a = 0;  b = 2;  c = 1
CALCULATE:
Rate constant k for data in 1B...______________ (b)

3) You mix together in the proper manner the following VOLUMES:

Using the rate constant and rate equation from problem 2),

CALCULATE the time to turn blue...__________________ sec (c)

4) A plot of log Rate vs 1/T gives a best straight line which goes through....
   1/T = 0.00300, log rate = -4.58
and 1/T = 0.00371, log rate = -6.00.
CALCULATE:
The Slope of the line..._____________ (d)

The Activation Energy (Ea) (Kj/mol)...________________(e)

Explanation / Answer

1)when you doubled the concentration of HCl the reaction went essentially 4X's faster

instead of taking 100 seconds, it took only 27 seconds

that's an effect of by the square

Rate = [2 X's as much HCl]^2

Rate = 4 X's faster

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