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By definition, the empirical formula is the simplest whole numer ratio that defines constituent atoms in a species. Normally we are given percentages, and use this mass percent to determine the elemental composition. Here, we are explicitly given the molar ratios, i.e.
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An alloy of tin is 15% tin and weighs 20 pounds. A second alloy is 10% tin. How many pounds of the second alloy must be added to the first to get a 12% mixture?
Let the mass of the 10 % alloy be $xcolor(white)(l)"lb"$. Then $20 color(red)(cancel(color(black)("lb"))) × 15 color(red)(cancel(color(black)("% Sn"))) + x color(red)(cancel(color(black)("lb"))) × 10 color(red)(cancel(color(black)("% Sn"))) = (20 + x) color(red)(cancel(color(black)("lb"))) ×...
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Copper will react with sulfur to form a copper sulfide, if 1.500g copper reacts with sulfur to form 1.880g of copper sulfide, what is the empirical formula of the copper sulfide?
The idea here is that you need to use the mass of copper and the mass of the copper sulfide to determine how much sulfur the produced compound contains, then...
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A certain ionic compound is found to contain .012 mol of sodium, .012 mol of sulfur, and .018 mol of oxygen. What is its empirical formula?
A compound's empirical formula tells you what the smallest whole number ratio between the that make up that compound is. In your case, you know that this contains...
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A sample of sulfur having a mass of 1.28 g combines with oxygen to form a compound with a mass of 3.20g. What is the empirical formula of the compound?
Since your compound will only contain sulfur and oxygen, you can conclude that the difference between the mass of sulfur and the mass of the final compound will represent the...
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A sample of sulfur having a mass of $1.28$ g combines with oxygen to form a compound with a mass $3.20$ g. What is the empirical formula of the compound?
Your goal when dealing with is to determine the smallest whole number ratio that exists between the that make up the compound. In order to do that, you first need...
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A sample of an iron sulfide contains $2.561*g$ of metal, and $2.206*g$ of sulfur. What is the empirical formula of iron sulfide?
$"Moles of iron"$ $=$ $(2.561*g)/(55.85*g*mol^-1)$ $=$ $0.0459*mol$ $"Moles of sulfur"$ $=$ $(2.206*g)/(32.06*g*mol^-1)$ $=$ $0.0688*mol$ If we divide thru by the lower molar quantity, we get, $FeS_(1.5)$. However, by definition, the...
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What are the empirical formulas for:
calcium chloride,
potassium oxide,
magnesium sulfide,
magnesium chloride,
lithium fluoride,
lithium oxide,
sodium sulfide?
Magnesium, Potassium, Lithium, and Sodium all have an oxidation state of $+1$. Calcium has $+2$. Oxygen and Sulfur have an oxidation state of $-2$. Fluorine and Chlorine have an oxidation...
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The mineral greenockite is a yellow sulfide of cadmium that is 78.0% cadmium and 22.0% sulfur. How do you determine the empirical formula of greenockite?
Start by assuming a mass of $100$ grams of the compound. Then, the percentages can be exchanged for masses. i.e. there are $"78 g"$ of cadmium and $"22 g"$ of...
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The atomic number of sulfur is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, how do you predict the molecular formula of the compound?
We thus predict that hydrogen sulfide would have a formula of $H_2S$, an analogue of the popular $H_2O$ molecule.
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How many grams of sodium sulfide are formed if 1.50 g of hydrogen sulfide is bubbled into a solution containing 2.00 g of sodium hydroxide, assuming that the sodium sulfide is made in 94.0 % yield?
The first step for any chemical reaction is to write out the chemical equation to determine the molar ratios of the reactants and products. Then we will use the molecular...
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