New answers tagged combustion
2
The oxidation of hydrocarbons ($\ce{RH}$) such as this one proceed via a chain mechanism. The initiation step is
$$\ce{RH + O2 -> HO2^. + R^.}$$
and the propagation
$$\ce{ R^.+O2 -> RO2^. \\ RO2^. +RH -> ROOH +R^. }$$
But it does not stop there as the hydroperoxide decomposes $\ce{ ROOH -> RO^. + OH^.}$ and there are other reactions ...
0
In order to determine the rate law, you need to be able to measure either the rate at which the reactants are consumed or the products are formed.
A very common error is to base the rate law on the balanced chemical equation. In fact, many high school level teachers will teach kinetics this way. Unfortunately this is a serious error.
It is possible for ...
3
Do not use flour, it may explode!
Use the pot lid to smother the fire.
Use a fire blanket - read the instructions, watch a you tube demo. People who think they know what they're doing often spread it or end up burned.
Salt, will put out small fires, such as a pan fire, you won't have enough salt to smother a pot or absorb the heat.
Good for putting out ...
1
If you look at the overall reaction, there is actually no gas produced, but there is a consumption of gas:
$\ce{CH3(CH2)_n-OH + \frac{3}{2} (n + 1)O2 -> (n + 1)CO2 +(n + 2)H2O}$
So 1.5 mol of oxygen are consumed, while only 1 mol of carbon dioxide is formed, so the volume will be less if the temperature is maintained.
To perform this experiment, you ...
Top 50 recent answers are included
