For the reaction A + B + C D The following data were obtained at constant temper
ID: 926892 • Letter: F
Question
For the reaction
A + B + C D
The following data were obtained at constant temperature:
What is the order with respect to each reactant? (Enter the order for A as Answer 1, that for B as Answer 2, and that for C as Answer 3. You must get all 3 correct.)
What is the value of the rate constant for the reaction at this temperature?
Trial Initial [A] (mol/L) Initial [B] (mol/L) Initial [C] (mol/L) Initial Rate (mol/L . s) 1 0.0865 0.0780 0.0156 0.086 2 0.1730 0.0780 0.0156 0.172 3 0.1730 0.1560 0.0156 0.688 4 0.0865 0.0780 0.0312 0.086Explanation / Answer
Answer –Given, reaction – A + B + C -------> D
So rate law is
Rate = k [A]x [B]y [C]z
In this rate law there are x,y and z are the order with respect to A, B and C
So,
Rate1 = k [A]1x [B]1y [C]1z
Rate2 = k [A]2x [B]2y [C]2z
Rate3 = k [A]3x [B]3y [C]3z
Rate4 = k [A]4x [B]4y [C]4z
Now we need to calculate order with respect to A means x, so we need to take ration Rate 2 by Rate 1
Rate2/ Rate1 = k [A]2x [B]2y [C]2z / k [A]1x [B]1y [C]1z
0.172 / 0.086 = (0.1730)x /(0.0865)x * (0.0780)y /(0.0780)y *(0.0156)z /(0.0156)z
2 = (2)x
So, x = 1
Now we need to calculate z
Rate3/ Rat2 = k [A]3x [B]3y [C]3z / k [A]2x [B]2y [C]2z
0.688 / 0.172 = (0.1730)x /(0.1730)x * (0.1560)y /(0.0780)y *(0.0156)z /(0.0156)z
4 = (2)y
So, y = 2
Now we need z calculate
Rate4/ Rate1 = k [A]4x [B]4y [C]4z / k [A]1x [B]1y [C]1z
0.086 / 0.086 = (0.0865) / (0.086) * (0.0780)2 /(0.0780)2 *(0.0312)z /(0.0156)z
1 = (2)z
So, z = 0
So the order with respect to A. B and C are 1, 2 and 0 respectively.
So rate of reaction depends on A and B.
Overall order of reaction = 1+2 = 3
So, rate law
Rate = k [A] [B]2
Now we need to put the values and calculate k
0.0156 Ms-1 = k (0.0865)*(0.0780)2
k = 0.0156 /0.000526
k = 29.6 M-2 s-1
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