What Is The Density Of Ethanol? 

The density of ethanol is one of the important properties of ethanol. Ethanol is a renewable fuel made from corn, sugarcane, and other plant materials, but mostly from corn. Ethanol use is widespread, and more than 98% of gasoline in the United States contains some ethanol. The most common blend of ethanol is E10, which means 10% ethanol and the remaining 90% is gasoline. It is one of the largest organic chemicals used in industrial and consumer products. The main industrial uses of this aliphatic alcohol are as an intermediate in the production of other chemicals and as a colvent. Let’s know the density of ethanol

What Is The Density Of Ethanol? 

The density of ethanol is 789 kg/m3, which is at room temperature. Ethanol density, to an extent, depends on the temperature and pressure of the surroundings. Changes in the temperature and surrounding result in change in the volume of this liquid, which, in turn, results in change in its density. 

Let us know the ethanol density in different units. So, the density of 95% ethanol is 0.805 g/ml at 15.6 degrees C temperature, the density of ethanol kg/l is 0.79 kg/l, the density of ethanol in kg/m3 is 789.3 kg/m3, and the density of ethanol g/ml is 0.789 g/ml.  

The density of ethanol and water is not the same but ethanol has more density than water. Therefore, ethanol is denser than water. 

When you examine the density of ethanol at different temperatures then you will get that the ethanol density is inversely proportional to the temperature. It is because the density is inversely proportional to volume, so no increasing the temperature, volume gets increased, resulting in lower density of the ethanol. 

Now, you know the density of ethanol g ml including other units. Let us have a look at the definition of the ethanol density. 

Definition Of Density Of Ethanol 

The density of ethanol is defined as the ratio of the mass of the ethanol and the unit volume of the ethanol. In other words, it is mass per unit volume. And the average density of ethanol is 0.789 g/cm3, which means, 0.789 mass per cubic cm. 

The ethanol density basically depends upon how closely the atoms are spaced in a particular object or liquid. If the object floats on water, it means it has a lower density than water. But in the case of ethanol, it sinks in the water, it means ethanol has more density than water. 

The definition of the ethanol density can be expressed in equation form as, 

Density of Ethanol = Mass of Ethanol Volume of Ethanol g/cm3 

In the symbolic form, 

                           D = mv g/cm3 

Where, d – the density of ethanol, 

            m – mass of the ethanol, and 

             v – the volume of ethanol 

Let us know how to calculate density of ethanol

How To Calculate Density Of Ethanol? 

The calculation of ethanol density is quite tough because it is liquid. And it is not possible to calculate the density of a liquid. So, if you need to know the ethanol density you can look it up in some chemical database. Don’t worry, it has alternatives, you can measure it experimentally if you have equipment. Let’s understand it step by step. 

  • Take an ethanol in a small quantity and measure its mass by just weighing a glass vial called pyknometer. 
  • Pyknometer having a fixed volume of the liquid. 
  • The volume of pykometer is fixed so, by just weighing pyknometer you will get the mass of ethanol. 
  • Now, you have both mass and volume, just divide mass by volume, you will get the density of ethanol. 

Let’s see the practical use of above-giver formula with the help of an example. 

If the 17.15 moles of ethanol are pured in 1.0 litres of pure ethanol, then what will be the density of ethanol? 

By using density formula, 

 D = mv g/cm3 

 Given, volume of ethanol = 1.0 L = 1000 mL 

            Mass of ethanol = 17.15 mols = 17.15 x 46 grams = 788.9 grams 

So, density of ethanol = 788.9/1000 

                                   = 0.789 g/mL 

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Is Ethanol Denser Than Water?

Which liquid is more dense water or Alcohol? A: Well, I cannot speak for all kinds of alcohols, but the common ones (methanol, ethanol, and isopropyl alcohol) are a little less dense than water. All three of these have densities of about 0.79 g/cc at standard temperature and pressure, compared to 1.0 g/cc for water.

Is Ethanol High Density?

Ethyl alcohol (ethanol) is less dense than water, and it’s boiling point is lower.

How Is Density Of Ethanol Determined?

Determining the density of ethanol-water solutions as a function of the volume concentration of the ethanol. The density of a liquid is defined as the ratio = m V (I), m: mass, V: volume.

Is Ethanol Heavier Than Air?

Ethanol is a polar solvent that is water-soluble and has a 55°F flash point. Ethanol has a vapor density of 1.59, which indicates that it is heavier than air. Consequently, ethanol vapors do not rise, similar to vapors from gasoline which seek lower altitudes.

What Is The Density Of 1 Ton Of Ethanol?

Ethanol weighs 0.7893 gram per cubic centimeter or 789.3 kilogram per cubic meter, i.e. density of ethanol is equal to 789.3 kg/m³; at 20°C (68°F or 293.15K) at standard atmospheric pressure.

What Is The Density Of Ethanol G Ml?

0.789 g/mL

The density of ethanol is 0.789 g/mL and the density of water is 1.0 g/mL.

Does Ethanol Have A Density Of 0.789 G Ml?

Answer and Explanation: To get the volume of ethanol, as asked for in the question, we simply divide the given mass of ethanol by the density of ethanol, and convert this calculated volume from mL to L : 500g(mL0.789g)(L1000mL)=0.633L 500 g ( m L 0.789 g ) ( L 1000 m L ) = 0.633 L .


After reading this article you have learned all about the ethanol density in detail. Ethanol is one of the important substances which is mainly used in the manufacture of drugs, plastic, lacquers, polishes, plasticizer, and cosmetics. Also, it is used in medicine as a topical overdose. Commercial products, such as perfumes, colognes, beverages, aftershaves, medicinal liquids, liniments, mouthwashes, and some rubbing alcohols. So, this was all about the density of ethanol.  

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