$"Sodium chloride, potassium chloride, rubidium chloride,"$ $"caesium chloride,"$ all have a formula of $MCl$, where $M$ is the alkali metal. All the alkali metals have similar electronic configurations; thus they...
1 Answers 1 viewsThe formula for is $"% by mass" = "mass of a component"/"total mass" × 100 %$ You have $"9.03 g Mg"$ and $"3.48 g N"$, so $"total mass =...
1 Answers 1 viewsAs is typical with these questions, we assume $100*g$ of unknown compound, and work out the MOLAR quantities of each element present: $" moles of C":$ $(15.8*g)/(12.011*g*mol^-1)=1.32*mol$ $" moles of...
1 Answers 1 viewsAnd, of course for a binary compound, $%H=(100-82)%=??%$
1 Answers 1 viewsSince your compound will only contain sulfur and oxygen, you can conclude that the difference between the mass of sulfur and the mass of the final compound will represent the...
1 Answers 1 viewsYour goal when dealing with is to determine the smallest whole number ratio that exists between the that make up the compound. In order to do that, you first need...
1 Answers 1 viewsThe of tin in the compound will be equal to the ratio between the mass of tin and the mass of the compound, multiplied by $100$. $color(blue)("% Sn"...
1 Answers 1 viewsAnd then we work out the molar composition. Thus $"Moles of carbon"$ $=$ $(92.3*g)/(12.011*g*mol^-1)=7.68*mol$. And $"Moles of hydrogen"$ $=$ $(7.7*g)/(1.00794*g*mol^-1)=7.64*mol$. Clearly, there is $1:1$ molar equivalence with respect to $C:H$....
1 Answers 1 viewsWe thus predict that hydrogen sulfide would have a formula of $H_2S$, an analogue of the popular $H_2O$ molecule.
1 Answers 1 viewsThe idea here is that you need to use the equation to determine how many moles of oxygen gas you have in that sample. This will allow you to...
1 Answers 1 views