1 Answers
Call
And then we work out the molar composition.
Thus
And
Clearly, there is
The molecular formula is a multiple of the empirical formula, but we have no handle on that here.
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What is the empirical formula of a compound which has a percent composition of 40.04% S and 59.96% O?
An empirical formula represents the lowest whole number ratio of in a compound. Since the percentages of the elements equal 100%, we can assume we have a 100 g sample,...
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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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Part A: Determine the empirical formula when the elemental composition by mass shows: 40.0% C, 6.71% H, 53.3% 0. For that I got CH2010 simplified to CHO5
Part B: Determine the molecular formula when the mole mass of the compound is 90.08 g/mol. (Help?)
To get the molecular formula of the compound, you need to use its empirical formula and its molar mass. The empirical formula tells you what the smallest integer ratio...
1 Answers 1 views
What is the empirical formula and empirical formula mass for the following compound: C3H6O3?
By definition, the empirical formula is the SIMPLEST whole number ratio that defines constituent atoms in a species. The ratio of atoms in that species is 1:2:1 with respect to...
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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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An unknown compound has the formula $C_xH_yO_z$. You burn 0.1523 g of the compound and isolate 0.3718 g of $CO_2$ and 0.1522 g of $H_2O$. What is the empirical formula of the compound?
First, work out the mass of each element that was present in the original compound. Carbon is always present as $CO_2$ in the ratio (12.011 g / 44.0098 g), and...
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Hydrogen peroxide has the empirical formula HO and an empirical formula weight of 17.0 amu. If the molecular weight is 34.0 amu, what is the molecular formula?
First, you want to find the ratio between the empirical formula and molecular formula; that is, how much has the molecular formula been simplified to reach the empirical formula. We...
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An unknown compound was found to have a percent composition as follows: 47.0% potassium, 14.5% carbon, and 38.5% oxygen. What is empirical formula? If the true molar mass of the compound is 166.22 g/mol, what is its molecular formula?
As with all these problems, we assume a $100*g$ mass of unknown compound, and then we work out the molar quantity: $"Moles of potassium"=(47.0*g)/(39.10*g*mol^-1)=1.20*mol$ $"Moles of carbon"=(14.5*g)/(12.011*g*mol^-1)=1.21*mol$ $"Moles of oxygen"=(38.5*g)/(16.0*g*mol^-1)=2.41*mol$...
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For a compound NaAc, the percent composition is that: 29.28% C, 3.68% H, 39.01% O, and 28.03% Na. What is the empirical formula of this compound?
Convert the percentages to grams. If there were 100 g, each 1 % would equal 1 g. So, $"29.28 % C = 29.28g C"$ $"3.68 % H =...
1 Answers 1 views