The relationship between the mass $m$ and the molecular weight $MM$ is the following: $n=m/(MM)=>m=nxxMM$, where, $n$ is the number of mole of the substance in question.
The only two substances that are of interest to you are $"A"$ and $"B"$, so you can write the chemical equation as $color(red)(2)"A" + ... -> color(blue)(3)"B" +...
Your strategy here will be to use a sample of this compound to help you determine its empirical formula use the equation, the gas' , and the known STP...
As always with these problems, it is useful to assume $100*g$ of unknown compound....and thus find an empirical formula... $"Moles of carbon"=(12.8*g)/(12.011*g*mol^-1)=1.066*mol.$ $"Moles of hydrogen"=(2.1*g)/(1.00794*g*mol^-1)=2.084*mol.$ $"Moles of bromine"=(85.1*g)/(79.90*g*mol^-1)=1.066*mol.$ And we...
First, you want to find the ratio between the empirical formula and molecular formula; that is, how much has the molecular formula been simplified to reach the empirical formula. We...
$1*m^3-=1000*L$, and this is a very large volume. If you ever shift $4-5*m^3$ of concrete this is a good few hours hard work. Now gases have the property that they...
The solubility of a substance is a measure of how much can dissolve in a certain at a given temperature, and is usually expressed in units of grams of solute...
The distinction between a molecular and non-molecular structure is one of the most important criteria with which to assess . But here, if we have an elemental molecule, we have...
The rate of diffusion ($U_(rms)$) is given by: $U_(rms)=sqrt((3RT)/(MM))$ Where MM is the molar mass of the gas. Thus, when $MM$ increases, the diffusion rate will decrease.
We're asked to calculate the formula weight of a pure substance, knowing that $4.81xx10^-3$ $"mol"$ has a mass of $0.963$ $"g"$. To calculate the formula weight (relative , atomic weight,...
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