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The atomic mass of element A is 63.6 atomic mass units. The only naturally occurring isotopes of element A are A-63 and A-65. What is the percent abundance in a naturally occurring sample of element A closest to?
The average isotopic mass is the weighted average of the mass of the individual . Because the quoted average, $63.6$ $"amu"$, is closer to $""^63A$ than $""^65A$, the $""^63A$...
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What compound is broken down to produce the element used in cans, airplanes, and building materials?
Hard to know for which compound you are looking. $"Alumina"$ is $Al_2O_3$, and occurs naturally as the mineral $"corundum"$. Of course, we refine $"aluminum"$ from the mineral $"bauxite"$, which is...
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How do you write and balance the chemical equation that relates to this word equation: Solid zinc carbonate is heated and broken down into solid zinc oxide and carbon dioxide gas?
What does the $Delta$ symbol mean? Is the equation balanced with respect to mass and charge?
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What type of reaction occurs when one compound reacts and is broken down into different elements or simpler compounds?
When a binary compound breaks down into separate OR when break down into simpler compounds, it is known as a decomposition reaction. The general formula for decomposition reactions are: $AB...
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An unknown compound has a percent composition of 52.10% potassium, 15.8% carbon, and 32.1% oxygen. The molar mass of the compound is 150.22 g/mol. What is the empirical formula and the molecular formula of this compound?
As is typical with these questions, we assume $100*g$ of unknown compound, and work out the MOLAR quantities of each element present: $" moles of C":$ $(15.8*g)/(12.011*g*mol^-1)=1.32*mol$ $" moles of...
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A compound that contains only nitrogen and oxygen is 30.4% N by mass; the molar mass of the compound is 92 g/mol. What is the empirical formula and the molecular formula of the compound?
In $100* g$ of this there are $30.4* g$ $N$, and the balance $O$. We divide thru by the atomic masses in order to approach the empirical formula: $(30.4*g)/(14.01*g*mol^-1)$ $=$...
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If 20.50g of Sn combine completely with 24.49g of Cl to form a compound, what is the percent composition of tin in the compound? What is the empirical formula of the compound?
The of tin in the compound will be equal to the ratio between the mass of tin and the mass of the compound, multiplied by $100$. $color(blue)("% Sn"...
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A compound contains 69.94 percent iron and 30.06 percent oxygen. What is its molecular formula if the molar mass of the compound is 199.55 per mole?
As with all these problems, we ASSUME, that there is a $100*g$ mass of unknown compound. We break this quantity down into atoms. And, there is $(30.06*g)/(15.999*g*mol^-1)$ $=$ $1.88*mol$...
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What is the empirical formula of a compound that contains 32.39 percent sodium, 22.53 percent sulfur, and 45.07 percent oxygen?
First, convert percentages into grams. $ 32.39 % = 32.39 g$ $22.53% = 22.53 g$ $45.07% = 45.07 g$ Second, convert the grams into moles. $"32.39...
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Another compound found on Mars contains iron and oxygen. The compound contains 70% by mass of iron and 30% by mass of oxygen. How do you calculate the empirical formula of this compound?
Your ultimate goal here is to figure out the smallest whole number ratio that exists between iron and oxygen in this unknown compound, i.e. the empirical formula of the compound....
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