1 Answers
Call
This means that for
The volume of the oxygen is dependant on temperature and pressure.
E.g. : If you cooled it down to
The 22.4 L being the molar volume for ideal gases under those conditions. There are tables for other temperatures.
0
like
0 dislike
Talk Doctor Online in Bissoy App
Iron metal reacts with oxygen to produce iron (lll) oxide. If you have 12.0 moles of iron for a complete reaction, what do you need?
We need a stoichiometric equation: $2Fe(s) + 3/2O_2(g) rarr Fe_2O_3(s)$ And thus if $12.0*mol$ of metal oxidize, then CLEARLY, by the given , $18.0*mol$ of dioxygen gas are required....
1 Answers 1 views
Calcium carbonate decomposes to form calcium oxide and carbon dioxide gas. If 44.5 grams of calcium oxide is produced, how many grams of calcium carbonate had to decomposez?
We need a stoichiometric reaction that represents the decomposition of calcium carbonate: $CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr$ And thus calcium oxide and calcium carbonate are present in equimolar...
1 Answers 1 views
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...
1 Answers 1 views
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...
1 Answers 1 views
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" \...
1 Answers 1 views
Iron (III) oxide reacts with carbon monoxide to form molten iron and carbon dioxide. If .18 g of iron (III) oxide reacts with 0.11 g of carbon monoxide, how many grams of iron would be produced?
$"Moles of ferric oxide "=(0.18*g)/(159.69*g*mol^-1)$ $=$ $1.13xx10^-3*mol" metal oxide"$. $"Moles of carbon monoxide "=(0.11*g)/(28.0*g*mol^-1)$ $=$ $3.93xx10^-3*mol" CO"$. $Fe_2O_3$ 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 views
$2CO(g) + O_2(g) -> 2CO_2(g)$. How many liters of $O_2$ will react with 74.2 liters of CO? If 6.5 g of CO react, how many liters of $CO_2$ are produced?
We calculate the relative quantities from the molar ratios in the balanced reaction equation. $2CO(g)+O_2(g)→2CO_2(g)$. As a pretty good approximation, gas volumes are proportional to molar amounts. Therefore with...
1 Answers 1 views
Iron can be extracted from iron(III) oxide by heating it with coke (carbon). The other product in the extraction reaction is carbon dioxide.
What mass of iron is produced by reacting 550g of iron(III) oxide with 60g of coke?
Balanced 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 views
How do you determine the gram-formula mass of the propane gas? State the mole ratio represented in the equation of oxygen to carbon dioxide. Calculate the number of liters of water vapor produced when 25.0 liters of oxygen gas are consumed?
For propane we have 3 carbons and 8 hydrogen atoms, so the gram-molecular weight is (312 + 81) = 44g/mol. The mole ratio of oxygen to carbon dioxide is 5:3,...
1 Answers 1 views
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...
1 Answers 1 views