Answer:
a) First-order.
b) 0.013 min⁻¹
c) 53.3 min.
d) 0.0142M
Explanation:
Hello,
In this case, on the attached document, we can notice the corresponding plot for each possible order of reaction. Thus, we should remember that in zeroth-order we plot the concentration of the reactant (SO2Cl2 ) versus the time, in first-order the natural logarithm of the concentration of the reactant (SO2Cl2 ) versus the time and in second-order reactions the inverse of the concentration of the reactant (SO2Cl2 ) versus the time.
a) In such a way, we realize the best fit is exhibited by the first-order model which shows a straight line (R=1) which has a slope of -0.0013 and an intercept of -2.3025 (natural logarithm of 0.1 which corresponds to the initial concentration). Therefore, the reaction has a first-order kinetics.
b) Since the slope is -0.0013 (take two random values), the rate constant is 0.013 min⁻¹:
![m=\frac{ln(0.0768)-ln(0.0876)}{200min-100min} =-0.0013min^{-1}](https://tex.z-dn.net/?f=m%3D%5Cfrac%7Bln%280.0768%29-ln%280.0876%29%7D%7B200min-100min%7D%20%3D-0.0013min%5E%7B-1%7D)
c) Half life for first-order kinetics is computed by:
![t_{1/2}=\frac{ln(2)}{k}=\frac{ln(2)}{0.013min^{-1}} =53.3min](https://tex.z-dn.net/?f=t_%7B1%2F2%7D%3D%5Cfrac%7Bln%282%29%7D%7Bk%7D%3D%5Cfrac%7Bln%282%29%7D%7B0.013min%5E%7B-1%7D%7D%20%20%3D53.3min)
d) Here, we compute the concentration via the integrated rate law once 1500 minutes have passed:
![C=C_0exp(-kt)=0.1Mexp(-0.013min^{-1}*1500min)\\\\C=0.0142M](https://tex.z-dn.net/?f=C%3DC_0exp%28-kt%29%3D0.1Mexp%28-0.013min%5E%7B-1%7D%2A1500min%29%5C%5C%5C%5CC%3D0.0142M)
Best regards.
H
it’s is magnesium iodide
Answer:
1
False. if they all moved together at any time then it would be a million things withinthe human species all at once at a high rate