1) For the reaction A ↔ B, equilibrium data is shown below. What is the value of kA that would satisfy the equation: rate of conversion of A to B = kA x number of A molecules?
Time | Number of A Molecules | Number of B Molecules | # of A reacting in next second | # of B reacting in next second | # of A formed in next second | # of B formed in next Second |
0 | 40000 | 0 | 6000 | 0 | 0 | 6000 |
1 | 34000 | 6000 | 5100 | 2100 | 2100 | 5100 |
2 | 31000 | 9000 | 4650 | 3150 | 3150 | 4650 |
3 | 29500 | 10500 | 4425 | 3675 | 3675 | 4425 |
4 | 28750 | 11250 | 4313 | 3938 | 3938 | 4313 |
5 | 28375 | 11625 | 4256 | 4069 | 4069 | 4256 |
6 | 28188 | 11813 | 4228 | 4134 | 4134 | 4228 |
7 | 28094 | 11906 | 4214 | 4167 | 4167 | 4214 |
8 | 28047 | 11953 | 4207 | 4184 | 4184 | 4207 |
9 | 28023 | 11977 | 4204 | 4192 | 4192 | 4204 |
10 | 28012 | 11988 | 4202 | 4196 | 4196 | 4202 |
2) For the reaction A ↔ B, equilibrium data is shown below. What is the value of kB that would satisfy the equation: rate of conversion of B to A = kB x number of B molecules?
Time | Number of A Molecules | Number of B Molecules | # of A reacting in next second | # of B reacting in next second | # of A formed in next second | # of B formed in next Second |
0 | 40000 | 0 | 6000 | 0 | 0 | 6000 |
1 | 34000 | 6000 | 5100 | 2100 | 2100 | 5100 |
2 | 31000 | 9000 | 4650 | 3150 | 3150 | 4650 |
3 | 29500 | 10500 | 4425 | 3675 | 3675 | 4425 |
4 | 28750 | 11250 | 4313 | 3938 | 3938 | 4313 |
5 | 28375 | 11625 | 4256 | 4069 | 4069 | 4256 |
6 | 28188 | 11813 | 4228 | 4134 | 4134 | 4228 |
7 | 28094 | 11906 | 4214 | 4167 | 4167 | 4214 |
8 | 28047 | 11953 | 4207 | 4184 | 4184 | 4207 |
9 | 28023 | 11977 | 4204 | 4192 | 4192 | 4204 |
10 | 28012 | 11988 | 4202 | 4196 | 4196 | 4202 |
ANSWER - Part A:
The equation
rate of conversion of A to B = (kA) x (# molecules of A)
it resembles a straight-line equation (y = mx +b) where
Then, we need to plot the rate of conversion of A to B vs. the number of molecules of A:
From the plot we get
Then the value of kA is
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ANSWER - Part B:
It is similar to part A, but in this case the equation is
rate of conversion of B to A = (kB) x (# molecules of B)
where
Then, we need to plot the rate of conversion of B to A vs. the number of molecules of B:
From the plot we get
Then the value of kB is
1) For the reaction A ↔ B, equilibrium data is shown below. What is the value...