Converting Second Order to First Order: A Systematic Approach

In summary, the given second order equation can be changed into a system of first order equations by defining new variables and the resulting system is a representation of a central force field with a force inversely proportional to the 3rd power of distance. There may be two more equations that go with this one, and changing them into first order equations is straightforward.
  • #1
Dustinsfl
2,281
5
Can this second order be changed into a system of first order:
$$
x''(t) = -\frac{\mu}{(\sqrt{x^2+y^2+z^2})^3}x
$$
 
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  • #2
Let $x_{1}=x$ and $x_{2}=x'$. Then you have the first-order system
\begin{align*}
x_{1}'&=x_{2}\\
x_{2}'&=-\frac{\mu}{ \left(x_{1}^{2}+y^{2}+z^{2} \right)^{3/2}}.
\end{align*}
What are $y$ and $z$ doing? Are they independent functions of time?
 
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  • #3
Physically, this looks like a central force field with a force that varies inversely with the 3rd power of distance.

Can it be that you actually have: $r''(t)=- {\mu \over r^3}$?

If that is the case you can do the following:

$\ddot r=- {\mu \over r^3}$

Multiply left and right with $2 \dot r$.
$2\ddot r \dot r = -2 {\mu \over r^3} \dot r$

$\dot r^2 = {\mu \over r^2} + C$
 
  • #4
My guess - there are two more equations that go with this one!
 
  • #5
Jester said:
My guess - there are two more equations that go with this one!

There but if it was straight forward in changing the first equation, I would have done the other two. Will 2 other coupled equations alter how they are re-written as first order equations?

$$
y''(t) = -\frac{\mu}{(\sqrt{x^2+y^2+z^2})^3}y
$$
$$
z''(t) = -\frac{\mu}{(\sqrt{x^2+y^2+z^2})^3}z
$$
 
  • #6
Ackbach said:
Let $x_{1}=x$ and $x_{2}=x'$. Then you have the first-order system
\begin{align*}
x_{1}'&=x_{2}\\
x_{2}'&=-\frac{\mu}{ \left(x_{1}^{2}+y^{2}+z^{2} \right)^{3/2}}.
\end{align*}
What are $y$ and $z$ doing? Are they independent functions of time?

I had a typo by the way
$$
x''(t) = -\frac{\mu}{(\sqrt{x^2+y^2+z^2})^2}x
$$
 
  • #7
Assuming
$$x''(t)=-\frac{\mu}{(x^{2}+y^{2}+z^{2})^{3/2}}\,x,$$
then you can let $x_{1}$ and $x_{2}$ be defined as above, and let $y_{1}=y$ and $y_{2}=y'$, as well as $z_{1}=z$ and $z_{2}=z'$. Then you get the following system:
\begin{align*}
x_{1}'&=x_{2}\\
y_{1}'&=y_{2}\\
z_{1}'&=z_{2}\\
x_{2}'&=-\frac{\mu}{(x_{1}^{2}+y_{1}^{2}+z_{1}^{2})^{3/2}}\,x_{1}\\
y_{2}'&=-\frac{\mu}{(x_{1}^{2}+y_{1}^{2}+z_{1}^{2})^{3/2}}\,y_{1}\\
z_{2}'&=-\frac{\mu}{(x_{1}^{2}+y_{1}^{2}+z_{1}^{2})^{3/2}}\,z_{1}.
\end{align*}
 

FAQ: Converting Second Order to First Order: A Systematic Approach

What is the difference between 2nd order and 1st order reactions?

2nd order reactions involve two reactant molecules coming together to form the product, while 1st order reactions involve only one reactant molecule breaking down into products.

How do you determine if a reaction is 2nd order or 1st order?

The order of a reaction can be determined by analyzing the rate law equation. If the rate is directly proportional to the concentration of two reactants, the reaction is 2nd order. If the rate is directly proportional to the concentration of only one reactant, the reaction is 1st order.

Can a reaction have a fractional order?

Yes, it is possible for a reaction to have a fractional order. This occurs when the rate of the reaction is not directly proportional to the concentration of the reactants. It is commonly seen in complex reaction mechanisms where the rate is influenced by multiple factors.

How do 2nd order reactions differ from 0 order reactions?

In 0 order reactions, the rate of the reaction is not affected by the concentration of the reactants. This means that the reaction will proceed at a constant rate regardless of the amount of reactants present. In 2nd order reactions, the rate is directly proportional to the concentration of the reactants, meaning that the reaction rate will increase as the concentration of the reactants increases.

Can a 2nd order reaction become a 1st order reaction?

Yes, it is possible for a 2nd order reaction to become a 1st order reaction. This can occur when one of the reactants is present in a much higher concentration compared to the other reactant. In this case, the reaction rate will become dependent on the concentration of the reactant in lower abundance, making it a 1st order reaction.

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