The weighted average is the sum of each individual nuclide, multiplied by its isotopic abundance. So, we simply do the arithmetic: $0.7577xx34.969+0.2423xx36.966 = ???$ amu Then look at to...
1 Answers 1 viewsStart by writing the unbalanced chemical equation that describes this double displacement reaction $"FeCl"_ (3(aq)) + "NaOH"_ ((aq)) -> "Fe"("OH")_ (3(s)) darr + "NaCl"$ In order to balance...
1 Answers 1 viewsWe have the balanced equation: $4Fe(s)+3O_2(g)->2Fe_2O_3(s)$ And so, $4$ moles of iron react with $3$ moles of oxygen, and therefore, $12.9 \ "mol"$ of iron would react with: $12.9color(red)cancelcolor(black)("mol" \...
1 Answers 1 views$"Moles of sodium chloride"$ $(581*cancelg)/(58.44*cancelg*mol^-1)$ $=$ $"approx. "10*mol$ Thus $10$ $mol$ sodium metal are required.
1 Answers 1 viewsFirst you need to write the correct BALANCED chemical reaction equation. Then you can determine how many moles of $Cl_2$ would be produced from the available moles of Cl in...
1 Answers 1 views$"Moles of ferric oxide "=(0.18*g)/(159.69*g*mol^-1)$ $=$ $1.13xx10^-3*mol" metal oxide"$. $"Moles of carbon monoxide "=(0.11*g)/(28.0*g*mol^-1)$ $=$ $3.93xx10^-3*mol" CO"$. $Fe_2O_3$ is the reagent in deficiency (why?), and thus $2xx1.13xx10^-3*molxx55.85*g*mol^-1~=0.150*g$ iron metal are...
1 Answers 1 viewsYou know that $2"Na"_ ((s)) + "Cl"_ (2(g)) -> 2"NaCl"_ ((s))$ and that the reaction produced $"234 g"$ of sodium chloride. Convert this to moles by using the...
1 Answers 1 viewsBalanced Equation $"2Fe"_2"O"_3 + "3C"$$rarr$$"4Fe + 3CO"_2$ This is a limiting reactant question. The maximum amount of $"Fe"$ that can be produced is determined by the limiting reactant. We have...
1 Answers 1 viewsYou need to start by writing the balanced chemical equation that describes the of sodium chloride $color(red)(2)"Na"_ ((s)) + "Cl"_ (2(g)) -> 2"NaCl"_ ((s))$ The balanced chemical...
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