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A chemical compound requires 8 ounces of Chemical A and 12 ounces of Chemical B. A mixture contains 24 ounces of Chemical A and 30 ounces of Chemical B. How can you fix the mixture to make the chemical compound?
Since 8x3=24 and since 12x3=36 you need to add 6oz of chemical B to have 24oz of chemical A and 36oz of chemical B. Take 1/3 of the total mixture...
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How do you write "Iron (III) chloride plus aluminum yields aluminum chloride and iron" in a chemical equation?
You don't need to note charges in the equation, if that's what you meant. The charge is implied because of the three Chlorides. Hope this helps!
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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....
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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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What mass in grams of iron(III) oxide contains 71.6 g ofiron? Iron(III) oxide is 69.94% iron by mass.
A substance's essentially tells you how many grams of each constituent element you get per $"100 g"$ of said substance. In this case, a percent composition of $69.94%$...
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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...
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Aluminum oxide is decomposed to extract pure aluminum from the mineral. If 6.7 tons of aluminum oxide is mined, calculate the mass of pure aluminum produced?
1 mole of aluminum oxide has a molecular weight of 102 grams (Al=27 grams and O=16 grams). It means that for 1000 kg of compound you can get 529 kilograms...
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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...
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A compound containing $"36.5%"$ of sulfur and $"63.5%"$ of iron reacts with a compound containing $"27.6%"$ oxygen and $"724%"$ of iron. What is the balanced equation and the theoretical yield of iron oxide?
The 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...
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If iron (II) oxide gas decomposes into iron liquid and oxygen gas and 6 moles of iron (II) oxide gas are used, how of liters of oxygen gas are produced?
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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