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How much energy is released when 496 g of ethanol 46 g mol vapor condenses The heat of vaporization of ethanol is 38 6 kJ mol?
The number of moles of ethanol can be calculated as 496 g divided by the molar mass of ethanol, which is 46 g/mol. This equals 10.78 mol. The energy released can be calculated by multiplying the number of moles by the heat of vaporization: 10.78 mol * 38.6 kJ/mol = 416.25 kJ.
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 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 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 glucose are required to form 127g of ethanol?
To form ethanol, the chemical equation shows that one mole of glucose is converted to two moles of ethanol. The molar mass of glucose is around 180 g/mol and that of ethanol is around 46 g/mol. Therefore, to produce 127g of ethanol, you would need 127g/(46g/mol) = 2.76 moles of ethanol. Since glucose to ethanol is a 1:2 ratio, you would need half as many moles of glucose, which would be 1.38 moles of glucose.
How many moles are represented by 16.0 g of ethanol C2H5OH?
To find the number of moles of ethanol (C2H5OH) in 16.0 g, first calculate its molar mass. The molar mass of C2H5OH is approximately 46.07 g/mol. Using the formula: moles = mass (g) / molar mass (g/mol), we have moles = 16.0 g / 46.07 g/mol, which equals approximately 0.347 moles of ethanol.
How many moles are there in 3.00 g of ethanol CH3CH2OH?
To find the number of moles in 3.00 g of ethanol (C₂H₅OH), first calculate its molar mass. The molar mass of ethanol is approximately 46.07 g/mol. Using the formula ( \text{moles} = \frac{\text{mass}}{\text{molar mass}} ), we have ( \text{moles} = \frac{3.00 , \text{g}}{46.07 , \text{g/mol}} \approx 0.065 , \text{moles} ). Thus, there are approximately 0.065 moles of ethanol in 3.00 g.
What is the mass of 0.5623 moles of ethanol ch3ch2oh?
To calculate the mass of 0.5623 moles of ethanol (C2H5OH), you need to use the molecular weight of ethanol, which is approximately 46.07 g/mol. Multiply the number of moles by the molecular weight to get the mass: 0.5623 moles x 46.07 g/mol ≈ 25.89 grams. Therefore, the mass of 0.5623 moles of ethanol is approximately 25.89 grams.
What is the mole fraction of ethanol in a solution of 47.5 grams of ethanol in 850 grams of water?
Unless I've completely forgotten my chemistry, mole fraction is the fraction of moles of a particular solute of the entire number of moles in the solution. So for this question: formula weight of ethanol = 46.07 g/mol formula weight of water = 18.015 g/mol moles of ethanol = 47.5g / 46.07 g/mol = 1.0310 mol moles of water = 850g / 18.015 g/mol = 47.182 mol total number of moles in the solution = 1.0310 + 47.182 = 48.213 mol therefore, the mole fraction of ethanol is 1.0310 mol / 48.213 mol = 0.0214 hope this helps.
How much energy is released when 496 g of ethanol 46 g mol vapor condenses The heat of vaporization of ethanol is 38 6 kJ mol?
The number of moles of ethanol can be calculated as 496 g divided by the molar mass of ethanol, which is 46 g/mol. This equals 10.78 mol. The energy released can be calculated by multiplying the number of moles by the heat of vaporization: 10.78 mol * 38.6 kJ/mol = 416.25 kJ.
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 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 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 glucose are required to form 127g of ethanol?
To form ethanol, the chemical equation shows that one mole of glucose is converted to two moles of ethanol. The molar mass of glucose is around 180 g/mol and that of ethanol is around 46 g/mol. Therefore, to produce 127g of ethanol, you would need 127g/(46g/mol) = 2.76 moles of ethanol. Since glucose to ethanol is a 1:2 ratio, you would need half as many moles of glucose, which would be 1.38 moles of glucose.
How much energy is absorbed when 356 g of ethanol 46.0 g molboils The heat of vaporization of ethanol is 38.6 kJ mol?
To calculate the energy absorbed, first convert the mass of ethanol from grams to moles. 356 g of ethanol is 356/46.0 = 7.74 moles. Then, multiply the moles of ethanol by the heat of vaporization: 7.74 mol * 38.6 kJ/mol = 298.56 kJ of energy absorbed.
How much energy is released when 496 g of ethanol 46.0 g mol vapor condenses The heat of vaporization of ethanol is 38.6 kJ mol?
To calculate the energy released when 496 g of ethanol vapor condenses, first convert the mass of ethanol to moles. Then, use the heat of vaporization value to determine the energy released per mole of ethanol. Finally, multiply the energy released per mole by the number of moles in 496 g to find the total energy released.
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
