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There are 3 isotopes of carbon. Carbon-12, Carbon-13 and Carbon-14. The average atomic mass of carbon is 12.011. Which isotope of carbon is the most abundant? Why?
The relative of carbon is 12.011, which is extremely close to 12.0. This means that the masses C-13, and C-14 are practically negligible when contributing to the relative atomic mass...
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Carbon has a third isotope, named carbon-13. How many protons and neutrons are found in each atom of carbon-13. Carbon-13 is a stable isotope, like carbon-12. How useful would carbon-13 be for radiometric dating?
This is called the of the element. To make it up to 13 in carbon-13, you will need 7 neutrons. Stable isotopes are not useful at all in radio-dating,...
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You are a compound in the laboratory. You find that it is made up of carbon, hydrogen, and oxygen in a ratio of two hydrogen atoms for each carbon atom. How will you classify the compound?
The question states the compound is made up of only carbon, oxygen and hydrogen, therefore it narrows it down to Lipids or carbohydrates as a macromolecule choice. Carbohydrates have a...
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A carbon compound contains 12.8% of carbon, 2.1% of hydrogen and 85.1% of bromine. The molecular weight of the compound is 187.9. What is the molecular formula of the compound?
(Atomic weight: H = 1.008, C = 12.0, Br = 79.9)
As always with these problems, it is useful to assume $100*g$ of unknown compound....and thus find an empirical formula... $"Moles of carbon"=(12.8*g)/(12.011*g*mol^-1)=1.066*mol.$ $"Moles of hydrogen"=(2.1*g)/(1.00794*g*mol^-1)=2.084*mol.$ $"Moles of bromine"=(85.1*g)/(79.90*g*mol^-1)=1.066*mol.$ And we...
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A compound containing only carbon and hydrogen has a carbon-to-hydrogen mass ratio of 11.89. Which carbon-to-hydrogen mass ratio is possible for another compound composed only of carbon and hydrogen?
Trying to present a possible Answer We know that the molar mass of carbon and hydrogen are $C=12"g/mol" and H = 1"g/mol"$ When Carbon Hydrogen mass ratio is 11.89 The...
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A compound of 2.225 g, known to be a carbohydrate, was analyzed and found to contain 0.890 g of carbon, 0.148 g of hydrogen and the rest was oxygen. How do you determine the percentage composition by mass of the compound?
The mass percentage of a substance in a compound is represented by the equation $%compon ent = (g_(compon ent))/(g_(t otal)) xx 100%$ What we can do first is find it...
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An organic compound is known to be composed of 46.60% carbon, 6.800% hydrogen, and 46.60% oxygen. What is its empirical formula?
Step 1: For this type of problem, if the percentages add up to 100% (and it almost always is), then it safe to assume 100g sample. By assuming that...
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A compound containing only carbon and hydrogen is analyzed, and is found to contain 20.11% hydrogen on a mass basis. How can the empirical formula of the compound be calculated?
In 100 g hydrocarbon, there are $(20.11*g)/(1.00794*g*mol^(-1)) = 19.95$ $mol$ $H$, and $(79.89*g)/(12.011*g*mol^(-1)) = 19.95$ $mol$ $C=6.65*mol$ $C$. We then divide thru by the lowest ratio to give the empirical...
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What is the empirical formula of a compound composed of 3.25% hydrogen (H), 19.36% carbon (C), and 77.39% oxygen (O) by mass?
We assume $100*g$ of unknown compound, and work out the elemental proportions in terms of moles: $H:$ $(3.25*g)/(1.00794*g*mol^-1)$ $=$ $3.22*mol;$ $C:$ $(19.36*g)/(12.01*g*mol^-1)$ $=$ $1.61*mol;$ $O:$ $(77.39*g)/(15.99*g*mol^-1)$ $=$ $4.84*mol;$ We divide...
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A compound is composed of 85.64% carbon and 14.36% hydrogen. The compound has a formula mass of 42.08 grams. What is the molecular formula?
As with all of these problems, we assume $100*g$ of unknown compound. And thus, we determine the elemental composition by the given percentages. $"Moles of carbon"=(85.64*g)/(12.011*g*mol^-1)=7.13*mol$. $"Moles of hydrogen"=(14.36*g)/(1.00794*g*mol^-1)=14.25*mol$. Clearly,...
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