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How do i calculate the number of moles of magnesium, chlorine, and oxygen atoms in 7.70 moles of magnesium perchlorate, $"Mg"("ClO"_4)_2$. Express the number of moles of Mg, Cl, and O atoms numerically, separated by commas. moles of Mg, Cl, O =?
$1 "mol" " Mg"("ClO"_4)_2$ contains :- $color(red)(1 "mol Mg atoms")$ $color(blue)(2 "mol Cl atoms"$ $color(green)(8 "mol O atoms"$ To find no. of moles of each element,...
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Iron is extracted from iron ore. Part of the process involves reduction of the ore with carbon monoxide. Iron ore contains iron oxide ($Fe_2O_3$). How would you write a balanced equation for the reaction of iron oxide with carbon monoxide?
And 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...
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If we are converting phosphorus from 3.44 moles to atoms, why do we sometimes do mole -> atoms? Instead of doing moles -> molecules -> atoms?
Phosphorus is an element. Elements are usually converted from moles to atoms using Alvogardo's number $ 6.02 xx 10^23$ If phosphorus is in elemental form it is not necessary to...
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3.55 moles $H_2$ (g), 1.25 moles $CO$ (g), and an unknown number of moles $N_2$ (g) were placed into a 5.00 L flask at $25.0^oC$. Given the density of this gas mixture to be 19.92 g/L, how many moles of $N_2$ were in the flask?
First start by finding the mass of the gas mixture. $density = (mass )/ (volume)$ $mass = density xx volume$ $mass = 19.92 \ g/L xx 5.00 \ L$ $mass...
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Which option contains a $2*g$ mass of sodium atoms....
$1.$ $5.24xx10^22*"sodium atoms?"$
$2.$ $6.022xx10^24*"sodium atoms?"$
$3.$ $3.12xx10^23*"sodium atoms?"$
$4.$ $5.24xx10^22*"sodium atoms?"$
We 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...
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How many moles of chlorine gas will be required to react with sufficient iron to produce 14 moles of iron (III) chloride?
So the mol ratio $Cl_2divFeCl_3=3div2$ So for 14 mols of $FeCl_3$ we need $3/2xx14=21$ mols of $Cl_2$
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7.0 moles of sulfur atoms and 10 moles of oxygen molecules are combined to form the maximum amount of sulfur trioxide, how many moles of which reactant remain unused at the end of the reaction?
.........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...
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When iron rusts in air, iron (Ill) oxide is produced. How many moles of oxygen react with 6.4 mol of iron in the rusting reaction?
Balanced equation $"4Fe(s) + 3O"_2("g")"$$rarr$$"2Fe"_2"O"_3("s")"$ Multiply the given moles of iron by ratio between oxygen and iron from the balanced equation, with moles oxygen in the numerator. $6.4color(red)cancel(color(black)("mol Fe"))xx(3"mol O"_2)/(4color(red)cancel(color(black)("mol...
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When iron rusts in air, iron (III) oxide is produced. How many moles of oxygen react with 12.9 mol of iron in the rusting reaction? $4Fe(s) + 3O_2(g) -> 2Fe_2O_3(s)$?
We 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" \...
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Iron rusts when exposed to oxygen. Iron(II) is produced in the reaction. How many moles of oxygen oxide will react with 2.4 mol of iron in the rusting reaction?
$Fe(s) + 1/2O_2 rarr FeO(s)$ This is a very simplified representation of the oxidation of . But if there are $2.4*mol$ of iron metal, it should react with $1.2*mol$ of...
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