According to equation $3$ moles of oxygen gas is required to form arsenic trioxide = $2$ moles $3.4$ moles of O2 will be required to form Arsenic trioxide = ($2$ x $3.4$) / $3$ = $2.26$ moles
.........And oxygen is in deficiency. Given $10$ $mol$ of dioxygen gas, at most, $6.67$ $mol$ of sulfur trioxide can be generated. This is clearly indicated by the stoichometric equation. Should...
As for all these problems, we first need a stoichiometrically balanced equation, $Zn(s) + 1/2O_2(g) rarr ZnO(s)$ And thus between the oxide and the starting metal, there is clearly $1:1$...
Sodium peroxide can be thermolyzed to give dioxygen gas... $Na_2O_2(s) +Delta rarr Na_2O(s) + 1/2O_2(g)uarr$ But with water, we simply get an acid base reaction.... $Na_2O_2(s) +2H_2O(l) rarr 2NaOH(aq) +...
$"Moles of arsenic"$ $=$ $(1.587*g)/(74.92*g*mol^-1)=0.0212*mol$. $"Moles of chlorine"$ $=$ $(3.755*g)/(35.45*g*mol^-1)=0.106*mol$. We divide thru by the lowest molar quantity to give $AsCl_5$. This is not chemical you would find in a...
The reaction happening in solution is the following: $ZnO(aq)+2HCl(aq)->ZnCl_2(aq)+H_2O(l)$ Since the hydrochloric acid ($HCl$) is in excess, therefore, the number of moles of Zinc oxide ($ZnO$) will determine the mass...
Start by balancing the equation for the reaction between hydrogen $"H"_2$ and nitrogen $"N"_2$, which produces ammonia $"NH"_3$: $color(darkgreen)(1) color(white)(.) "N"_2 (g) + color(darkgreen)(3) color(white)(.) "H"_2 to color(darkgreen)(2) color(white)(.) "NH"_3...
We need a stoichiometic equation: $SO_2(g) + 1/2O_2(g) rarr SO_3(g)$ The equation unequivocally tells us that the reaction of $64*g$ $SO_2(g)$ with $16*g$ $O_2(g)$ gives $80*g$ $SO_3(g)$. The given masses...
Limiting reagent problems are all about using the that exists between the reactants to determine if you have enough of each reactant to allow for their complete consumption....
Given: Mass of $"O"_2$; chemical equation (understood) Find: Moles of $"CO"_2$ Strategy: The central part of any problem is to convert moles of something to moles of something else....
This 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...
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