Prima kosten-baten analyse inderdaad. (Waarbij de "kosten" in dit geval dus "moeite" is: reparatiespullen mee, leren banden plakken, je zorgen maken over pech onderweg etc.)
Het voordeel van de actieradius is dat je toch nooit veel verder dan een kilometer of 30 a 40 van huis zult zijn. In ieder geval niet zolang je geen tweede accu bij je hebt.
Ik heb helaas een manager die mij als uitzendkracht rustig de toko uitwipt als ik te vaak te laat kom. Lekke band of geen lekke band.
CO2 patronen bij lek
Sorry, maar dit klopt niet. Lucht is ca 70% stikstof, 21% zuurstof, wat CO2 en edelgassen, ... CO2 is zeker niet kleiner. Ik heb dat trouwens altijd onzin gevonden, (auto)banden vullen met stikstof om die reden.
Scheldelaan-Stromer
-
Fastedde
- Veteraan
- Berichten: 341
- Lid geworden op: 16 jul 2017, 18:10
- Locatie: Friesland
- Merk SP: Stromer ST2s
- Km-stand: 7500
HAllo Buzze, ik was dit ook altijd met je eens, maar ben na 2x dit probleem te hebben ervaren (na lekrijden, band plakken en met CO2 vullen, de volgende dagen een zachte band) eea wezen googelen, onderstaand komt van een ander forum, dit klinkt mij aannemelijk, diffisie proces:
Maar ja, misschien is t een placebo effect? Who knows.
" I suppose I should say something insightful rather than simply reacting...
Okay. Let's start with the Ideal Gas Law which is:
PV=nRT
Where:
P = Pressure
V = Volume
n = number of moles
R = Universal gas constant
T = Temperature
We assume for now that this is a closed system which is not entirely true as we will see later. Thus we have:
Pcyl Vcyl / ncyl R Tcyl = Ptube Vtube / ntube R Ttube
Now n is a constant and is fixed (ncyl = ntube) as of course is R, thus our relationship becomes:
Pcyl Vcyl / Tcyl = Ptube Vtube / Ttube
Initially Pcyl > Ptube. As the gas from the cylinder flows into the tube, Ptube starts to go up and Pcyl starts to decrease. However, bear in mind that Vtube also increases. Because Vcyl is fixed, in order to preserve the relationship, Tcyl must decrease. This is why the cylinder gets cold.
The gas expands from a smaller volume in the cylinder to a larger volume in the tube. The ratio of this expansion combined with the initial pressure in the cylinder directly governs the final pressure inside the tube when everything has come to equilibrium. The molecules of the gas do not expand or shrink. The space between them does. All molecular sizes are governed by the composition of their atoms and their atomic bonds.
Now we come to why tyres filled with CO2 go flat faster than with air. CO2 molecules are more permeable and soluable in butyl rubber than other molecules in air. Thus when a tube is filled with air, the CO2 molecules will tend to permeate and leak through the rubber faster than the other components of other gases in the air. This leaves other gasses such as Nitrogen and Oxygen (amongst others) to linger around longer. When a tube is filled with just CO2, the rate of leakage is the same as that of the CO2 leaking out through the tube filled with air but since there's only CO2 to leak, the tube will go flat faster.
BTW, CO2 doesn't necessarily leak through rubber faster because of its size but because of how the molecules in rubber attract CO2 better than Oxygen or Nitrogen. As a result, the CO2 permeates the rubber which then swells and thus allows more molecules to escape.".
+ST2S and n-joying it to the max...
