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timo86m
 2 years ago
for nin
And using calc to derive this formula
timo86m
 2 years ago
for nin And using calc to derive this formula

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timo86m
 2 years ago
Best ResponseYou've already chosen the best response.1Yes i remember integrating with time.

timo86m
 2 years ago
Best ResponseYou've already chosen the best response.1The central science book is not that advanced then since it just gives you formulas but doesn't explain how to reach that conclusion

timo86m
 2 years ago
Best ResponseYou've already chosen the best response.1calc 2 in this case. There is also some advanced wave function kinda stuff.

timo86m
 2 years ago
Best ResponseYou've already chosen the best response.1in the electronic structure of matter chapter luckily it dont go too far. It just gives you equations you will use.

abb0t
 2 years ago
Best ResponseYou've already chosen the best response.0Is this for thermodynamics? D:

abb0t
 2 years ago
Best ResponseYou've already chosen the best response.0For a reaction of the form: A > product a first order rate law takes the form: \[r = k_{1^{st}}[A]^1\] writing it in differentials, you get: \[\frac{ d[A] }{ dt } = k_{1^{st}}[A]\] The minus sign as A is a reactant and so its concentration decreases with time (whici is the slope of a graph of [A] against time will be negativ when you graph it) The variables [A] and t can be separated to give: \[\frac{ 1 }{ [A] }d[A] = k_{1^{st}}dt\] which CAN be integrated easily! \[\int\limits \frac{ 1 }{ [A] }d[A] = \int\limits k_{1^{st}}dt\] this gives: \[\ln[A] = k_{1^{st}}t + C\] The constant can be removed by supposing that at t = 0 since \[[A] = [A]_0\] which is the initial concentration of A giving us: \[\ln[A] = k_{1^{st}}t + \ln[A]_0\] to simplify it a bit more to a form that might be more familiar to you is: \[[A] = [A]_0 e^{(k_{1^{st}}t)} \]

nincompoop
 2 years ago
Best ResponseYou've already chosen the best response.1@abb0t I think what you did is the same to what I attached
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