Iron($Fe^(2 or 3)$) reacts with oxygen creating two oxides: $2Fe^(+2) + O_2 -> 2FeO$ If it is Iron(II), create Iron(II) oxide; $2Fe^(+3) +3O_2 ->Fe_2O_3$ If it is Iron(III), create Iron(III)...
1 Answers 1 viewsThe question states the compound is made up of only carbon, oxygen and hydrogen, therefore it narrows it down to Lipids or carbohydrates as a macromolecule choice. Carbohydrates have a...
1 Answers 1 viewsAnd this is the effectual chemical reaction of our civilization. If you ever have a chance to tour a blast furnace (and most are in China and India now) do...
1 Answers 1 viewsWe know that $1*mol$ contains $6.022xx10^23$ individual sodium atoms, and has a mass of $22.99*g$. And thus for $1.$ there is a $2*g$ mass of $Na$. For $2.$ there is...
1 Answers 1 viewsTrying to present a possible Answer We know that the molar mass of carbon and hydrogen are $C=12"g/mol" and H = 1"g/mol"$ When Carbon Hydrogen mass ratio is 11.89 The...
1 Answers 1 views$"Moles of chlorine"=(16.7*g)/(35.45*g*mol^-1)=0.47*mol$ $"Moles of sodium"=(10.8*g)/(22.99*g*mol^-1)=0.47*mol$ $"Moles of oxygen"=(22.5*g)/(16.00*g*mol^-1)=1.41*mol$ We divide thru by the smallest quantity, that of sodium, to give an empirical formula.....of $NaClO_3$, i.e. $"sodium chlorate"$.
1 Answers 1 viewsWe have been given an empirical formula of $C_4H_6O$. We know that the molecular formula is always a whole number multiple of the empirical formula. Thus ${4xx12.01+6xx1.01+16.0}xxn=280*g*mol^-1$. My arithmetic gives...
1 Answers 1 viewsYour ultimate goal here is to figure out the smallest whole number ratio that exists between iron and oxygen in this unknown compound, i.e. the empirical formula of the compound....
1 Answers 1 viewsThe first thing you have to do is determine the formula for iron sulfide by using the known of sulfur in the compound. Let's assume that the formula for iron...
1 Answers 1 viewsThis means that for $6mol$ of $FeO$, only $3mol O_2$ is produced (half the moles). The volume of the oxygen is dependant on temperature and pressure. E.g. : If...
1 Answers 1 views