what is the mass of 4.86 x 10^21 molecules of ethanol, C2H5OH?
step 1. We first calculate the number of moles present in Ethanol ,then in the next step we shall move to calculate the mass of ethanol present.
We know that,
6.023*10^23 molecules of ethanol will have = 1 mol.
So, 4.86*10^21 molecules of ethanol will have = 4.86*10^21/ 6.023*10^23 moles
=0.8069 * 10^ -2 moles.
= 0.008069 moles.
Step 2. In the step ,we shall calculate the mass of ethanol.
We know that ,No. Of Mole = mass in gm/ molar mass
Therefore, Mass = NO. Of mole * Molar mass
= 0.008069 mole * 46.07 g/mol
=0.3717 g
Please upvote
What is the molarity of a 12.1% (v/v) solution of ethanol (C2H5OH)? The density of ethanol is 0.785g/mL and the molar mass of ethanol is 46g/mol.
2.21 g of ethanol C2H5OH and 3.55 of oxygen O2 are reacted. Molar mass of C2H5Oh 46.08 g/mol. O2 32.00 g/mol. Co2 44.01 g/mol. H20 18.02 g/mol a)What is the limiting reactant? b) what is the theoretical yield of carbon dioxide in grams will be obtained in the combustion reaction. starting with the amount of reagents given in part (a). assuming the reaction goes in 100% yield. c) If 0.951 f of CO2 is obtained from the reaction above, what...
An aqueous solution of ethanol is prepared by dissolving 19.00 g of ethanol, C2H5OH, in 100.0 g of water. What is the molality of the ethanol solution? The formula mass of ethanol is 46.07 g/mol, and assume the density of water to be 1.000 g/mL
What is the MOLALITY of Ethanol , C2H5OH (46.08 g/mol), in an aqueous solution that is 51.0% ethanol by mass? (correct answer is 22.6 m, I'm just not sure of the steps) Please include step by step with units! Thanks!
A bottle of wine contains 11.0% ethanol by volume. The density of ethanol (C2H5OH) is 0.789 g/cm^3. Calculate the concentration of ethanol in wine in terms of mass percent and molality. Mass percent = ________% Molality = ___________m
What is the molarity of a 97.0−mL ethanol solution containing 5.05 g of ethanol (C2H5OH)?
Determine the mole fraction of ethanol, C2H5OH (Molar mass = 46.08 g/mol) when 12 grams of ethanol is dissolved in 49.7 grams of water, H2O (Molar mass = 18.02 g/mol).
Calculate the heat released when 135 grams of ethanol C2H5OH, burns. The heat of combustion of ethanol is 1233 kJ/mol. Molar mass of ethanol C2H5OH = 46.07 g/mol C2H5OH(g) + 3 O2(g) → 2 CO2 (g) + 3 H2O(l) LaTeX: \DeltaΔH = -1233 kJ/mol
Determine the molarity of a solution containing 17.2 grams of ethanol, C2H5OH (Molar mass = 46.08 g/mol) dissolved in 3.1 liters of solution. Answer to 2 decimal places.
1.Pentane (C5H12) has a surface tension of 1.61 x 10 ^ -2, while ethanol (C2H5OH) has a surface tension of 2.23 x 10 ^ -2, which would have the highest viscosity? A) pentane B) ethanol C) both have the same viscosity D) cannot be determined with the information provided 2.Which of the following is true for surface tension? l is a measure of the surface area exposed by the liquid ll increases with increasing intermolecular attraction forces lll decreases with...