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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 ...


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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 ...


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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 ...


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