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How many moles of ethanol C2H5OH are in a sample which weighs 39.2g?
Wiki User
∙ 10y ago
Because the formula shows that each molecule of ethanol contains 2 atoms of carbon, 6* atoms of hydrogen, and 1 atom of oxygen, the gram molecular mass of one mole of ethanol is the sum of twice the gram Atomic Mass of carbon, 6 times the gram atomic mass of hydrogen, and the atomic mass of oxygen: 46.07. Therefore, 39.2 grams of ethanol constitutes 39.2/46.07 or 0.851 mole, to the justified number of significant digits.
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The subscript 5 immediately after the first appearance of the atomic symbol for hydrogen in the formula, plus the implied subscript 1 of the second appearance of the atomic symbol for hydrogen in the formula.
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∙ 10y ago
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How many moles of carbon are in 1.271 grams of ethanol?
For this you need the atomic (molecular) mass of C2H5OH. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel. C2H5OH= 46.1 grams1.271 grams C2H5OH / (46.1 grams) = .0276 moles C2H5OH
What is the total sample size (in grams) for a sample of ethanol (CH3CH2OH) which contains 3.36 g of oxygen?
9.675 g Since oxygen has an average atomic weight of 15.999 g/mol that would make it 0.21 moles of oxygen. Ethanol has one atom of oxygen per molecule so that means 0.21 moles of ethanol. Since ethanol has a molecular weight of 46.07 g/mole, 0.21 moles of ethanol would have a mass of 9.675 g.
The formula for ethyl alcohol is C2H5OH. The mass of 2 moles of ethyl alcohol would be how many grams?
The mass of 2 moles of ethyl alcohol would be 92,14 grams.
What is the mole fraction of ethanol in a solution of 3.00 moles of ethanol and 5.00 moles of water?
0.375
How many molecules of ethanol are contained in a 19.6 mL sample of ethanol?
The density of ethanol is 0.789 g/mL. So 19.6 mL of ethanol weighs 0.789 g/mL * 19.6 mL = 15.464 g. The molar mass of ethanol is 2*12.011 + 6*1.008 + 15.999 = 46.069 g/mol. So, in 15.464 grams, there are 15.464 g / 46.069 g/mol = 0.33567 moles In one mole, there are 6.022*1023 molecules, so we have: 0.33567 moles * 6.022*1023 molecules/mole= 2.0214*1023 molecules. Using correct significant digits, that gives: 2.02*1023 molecules (or particles).
How many moles of carbon are in 1.271 grams of ethanol?
For this you need the atomic (molecular) mass of C2H5OH. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel. C2H5OH= 46.1 grams1.271 grams C2H5OH / (46.1 grams) = .0276 moles C2H5OH
How many moles in 11.5 g of C2H5OH?
1.5 - your welcome
What is the total sample size (in grams) for a sample of ethanol (CH3CH2OH) which contains 3.36 g of oxygen?
9.675 g Since oxygen has an average atomic weight of 15.999 g/mol that would make it 0.21 moles of oxygen. Ethanol has one atom of oxygen per molecule so that means 0.21 moles of ethanol. Since ethanol has a molecular weight of 46.07 g/mole, 0.21 moles of ethanol would have a mass of 9.675 g.
How many moles of ethyl alcohol C2H6O are in a 32.0 g sample Express your answer using three significant figures.?
32 g ethanol is equivalent to 0,695 moles.
The formula for ethyl alcohol is C2H5OH. The mass of 2 moles of ethyl alcohol would be how many grams?
The mass of 2 moles of ethyl alcohol would be 92,14 grams.
How many moles of specified particles are present in a sample of N'O if each sample weighs 7.00 g?
the mole is 30 g.
What is the mole fraction of ethanol in a solution of 3.00 moles of ethanol and 5.00 moles of water?
0.375
How many moles of CO2 are produced from each mole of C2H5OH completely burned?
In each mole of ethanol there are two moles of carbon atoms. One mole of carbon atoms is required to form one mole of carbon dioxide, so two moles will form two moles. Thus each mole of ethanol completely combusted will form two moles of carbon dioxide.
How much CO2 does a car running on ethanol fuel produce?
Assuming the fuel is 100% ethanol the reaction is: C2H5OH +3O2 --> 2CO2+3H20 or 1 mole of ethanol (46 g) creates 2 moles (44 x 2=88) of carbon dioxide The density of ethanol is 0.78 g/cm3 or .78 kg/L So the amount of carbon dioxide created by a car fueled by ethanol is about 1.56 kg/liter used. This excludes CO2 from ethanol manufacture.
How many molecules of ethanol are contained in a 19.6 mL sample of ethanol?
The density of ethanol is 0.789 g/mL. So 19.6 mL of ethanol weighs 0.789 g/mL * 19.6 mL = 15.464 g. The molar mass of ethanol is 2*12.011 + 6*1.008 + 15.999 = 46.069 g/mol. So, in 15.464 grams, there are 15.464 g / 46.069 g/mol = 0.33567 moles In one mole, there are 6.022*1023 molecules, so we have: 0.33567 moles * 6.022*1023 molecules/mole= 2.0214*1023 molecules. Using correct significant digits, that gives: 2.02*1023 molecules (or particles).
What is the mass of 0.5623 moles of ethanol ch3ch2oh?
The molar mass of ethanol is 46g/mol. Using the formula mass = (molar mass) x (no. of moles), the mass of 0.5623mol of ethanol is approximately 25.9g.
How many moles of ethanol per liter?
AnswerThe density of ethanol is 0.789 g/cm³ , and there are 1000 cm3 in a liter, so 1 liter weighs 0.789 kilograms.Density = mass/volume, So mass=density*volume.So, weight of 1L ethanol = 0.789*1 => 0.789KG
