Density Calculator

Our highly versatile density calculator makes it effortless to calculate the density, mass, and volume of any object or substance. Because these three physical properties are inherently connected, knowing any two allows you to instantly find the third. For example, if you know an object's mass and volume, you can quickly calculate its density. Alternatively, you can use the density calculator to determine an object's mass if you already know its volume and density.

This calculator is incredibly convenient because it supports a wide variety of measurement units. For mass, you can input grams, kilograms, ounces, or pounds. For volume, the tool seamlessly accepts milliliters, cubic centimeters, cubic meters, liters, cubic feet, and cubic inches—saving you the hassle of manual conversions.

What is the Density of a Substance?

In physics, the density of a substance is defined as its mass per unit of volume under standard conditions.

The world's most universally used density units are the International System (SI) unit of kilograms per cubic meter (kg/m³) and the CGS unit of grams per cubic centimeter (g/cm³). For reference, 1 kg/m³ is exactly equal to 1000 g/cm³.

In the United States, traditional measurements often express density in pounds per cubic foot (lb/ft³).

One pound per cubic foot is equal to 16.01846337395 kilograms per cubic meter. Accordingly, to convert a material's density from SI units to traditional U.S. units, you divide the value by 16.01846337395 (or simply by 16 for a quick estimate). To convert from U.S. units back to SI units, multiply your figure by 16.

The Greek letter ρ (rho) is the standard symbol used to represent density. In some cases, the Latin letters D and d (derived from the Latin densitas) are also used in density formulas.

To find a substance's density, you divide its mass by its volume. The density ρ is calculated using the standard density formula:

$$ρ=\frac{m}{V}$$

Where V is the volume occupied by a substance of mass m.

Since density, mass, and volume are mathematically interrelated, we can easily calculate mass if we know the density and volume:

$$m=ρ V$$

Likewise, if we know the density and mass of a substance, we can calculate its volume:

$$V=\frac{m}{ρ}$$

Densities of Various Substances

The densities of different materials and substances can vary significantly based on their environment and state.

A single substance will have different densities depending on whether it is in a solid, liquid, or gaseous state. For example, the density of liquid water is approximately 1000 kg/m³, solid ice is about 900 kg/m³, and water vapor is just 0.590 kg/m³.

Density also fluctuates based on temperature, the substance's aggregate state, and external pressure. When external pressure increases, a substance's molecules are forced closer together, resulting in a higher density.

Similarly, temperature changes heavily influence density. When temperatures drop, the molecular movement within a substance slows down, requiring less space and causing density to increase. Conversely, as temperatures rise, molecules expand and take up more space, which typically leads to a decrease in density.

Notable exceptions to this rule include water, cast iron, bronze, and a few other materials that exhibit unique behaviors at specific temperatures.

Water reaches its maximum density at exactly 4 °C (39.2 °F), measuring 997 kg/m³. For everyday calculations, this is often rounded up to 1000 kg/m³. As the temperature rises above or falls below 4 °C, water's density decreases. This explains why ice floats on the surface of liquid water—its density drops to 916.7 kg/m³ when frozen.

This unique property of ice is caused by hydrogen bonds. The crystal lattice of ice resembles a honeycomb, with water molecules connected by hydrogen bonds at each of its six corners. The distance between water molecules in this solid state is actually greater than in liquid form, where molecules move freely and pack closer together. The densities of bismuth and silicon also decrease upon solidification.

Ultimately, a material's density dictates whether it will float or sink. Objects less dense than water (under 1 g/cm³) will float, such as Styrofoam or wood. Materials with a higher density than water (over 1 g/cm³), such as solid metal, concrete, or glass, will sink.

For example, a solid iron cannonball sinks rapidly because it is much denser than water. However, a massive iron ship floats beautifully on the ocean. While the iron hull itself is dense, the vast interior of the ship is filled with air, which drastically lowers the vessel's overall average density. If the ship were a solid block of iron, it would immediately sink.

Furthermore, objects submerged in saltwater exhibit higher buoyancy than they do in clear or tap water. This happens because saltwater is denser than freshwater, thereby exerting a stronger upward buoyant force on submerged objects.

Density Chart for Solids

Solid Material	kg/m³	g/cm³
Osmium	22 600	22.6
Iridium	22 400	22.4
Platinum	21 500	21.5
Gold	19 300	19.3
Lead	11 300	11.3
Silver	10 500	10.5
Copper	8900	8.9
Steel	7800	7.8
Tin	7300	7.3
Zinc	7100	7.1
Cast iron	7000	7.0
Aluminum	2700	2.7
Marble	2700	2.7
Glass	2500	2.5
Porcelain	2300	2.3
Concrete	2300	2.3
Brick	1800	1.8
Polyethylene	920	0.92
Paraffin	900	0.90
Oak	700	0.70
Pine	400	0.40
Cork	240	0.24

Calculation Example

Imagine you are a sculptor planning to purchase a marble block for a new statue. You find a high-quality block measuring 0.3 × 0.3 × 0.6 meters. How do you calculate the weight of this block to arrange proper transportation?

First, multiply the block's dimensions together to find its volume:

0.3 × 0.3 × 0.6 = 0.054 m³

By consulting the density chart above, we know that marble has a density of 2700 kg/m³. Now, we can find the mass of the block using the formula:

$$m=ρ V$$

Calculating 0.054 × 2700 = 145.8 kg. Therefore, your beautiful marble block will weigh exactly 145.8 kilograms.

Density Chart for Liquids

Liquid	kg/m³	g/cm³
Mercury	13 600	13.60
Sulfuric acid	1 800	1.80
Honey	1 350	1.35
Seawater	1 030	1.03
Whole milk	1 030	1.03
Pure water	1 000	1.00
Sunflower oil	930	0.93
Machine oil	900	0.90
Kerosene	800	0.80
Alcohol	800	0.80
Oil	800	0.80
Acetone	790	0.79
Gasoline	710	0.71

Density Chart for Gases

Gas	kg/m³	g/cm³
Chlorine	3.210	0.00321
Carbon dioxide	1.980	0.00198
Oxygen	1.430	0.00143
Air	1.290	0.00129
Nitrogen	1.250	0.00125
Carbon monoxide	1.250	0.00125
Natural gas	0.800	0.0008
Water vapor	0.590	0.00059
Helium	0.180	0.00018
Hydrogen	0.090	0.00009

Understanding the density of gases like carbon monoxide can be lifesaving. During a fire, poisonous carbon monoxide is produced. Because it has a density of 1.250 kg/m³, which is slightly less dense (lighter) than standard room air (1.290 kg/m³), carbon monoxide naturally rises toward the ceiling. Therefore, if you are ever trapped in a burning building, it is highly recommended to stay as low to the floor as possible to avoid inhaling toxic fumes.

Bulk Densities of Common Foods

Bulk Materials	kg/m³	g/cm³
Fine table salt	1 200	1.2
Granulated sugar	850	0.85
Powdered sugar	800	0.8
Beans	800	0.8
Wheat	770	0.77
Corn grains	760	0.76
Brown sugar	720	0.72
Rice grains	690	0.69
Peeled peanuts	650	0.65
Cocoa powder	650	0.65
Dried walnuts	610	0.61
Wheat flour	590	0.59
Powdered milk	450	0.45
Roasted coffee beans	430	0.43
Desiccated coconut	350	0.35
Oatmeal	300	0.3

Calculation Example

Suppose you buy a 900-gram bag of premium roasted coffee beans. You have an empty 1.5-liter storage jar at home. Will all the coffee fit inside?

First, remember that one liter equals 1000 cm³. Therefore, your jar has a volume capacity of 1500 cm³.

Next, calculate the total volume your coffee beans will occupy using their mass and bulk density (0.43 g/cm³ for roasted coffee beans):

$$V=\frac{m}{ρ}$$

The volume of the coffee will be:

$$\frac{900}{0.43}= 2093.023255814\ cm³$$

Since the beans require nearly 2093 cm³ of space, your 1500 cm³ jar is unfortunately too small to hold the entire bag.

Bulk Densities of Building Materials

Bulk Materials	kg/m³	g/cm³
Wet sand	1920	1.92
Wet clay	1600 - 1820	1.6 - 1.82
Crushed gypsum	1600	1.6
Soil, loam, wet	1600	1.6
Crushed stone	1600	1.6
Cement	1510	1.51
Gravel	1500 - 1700	1.5 - 1.7
Gypsum lumps	1290 - 1600	1.29 - 1.6
Dry sand	1200 - 1700	1.2 - 1.7
Soil, loam, dry	1250	1.25
Dry clay	1070 - 1090	1.07 - 1.09
Asphalt crumb	720	0.72
Wood chips	210	0.21

In construction and engineering, the concept of bulk density is crucial when analyzing loose construction materials like sand, gravel, and crushed stone. This metric is essential for calculating the cost-effective usage of different components when mixing concrete or filling large spaces.

Bulk density is a variable metric. Under different conditions, the exact same weight of a material might occupy a different volume. The finer the particles are, the more densely they pack together in a pile. Sand, for example, boasts one of the highest bulk densities among common construction materials. Conversely, larger grains create more empty voids between them. Beyond size, the shape of the granules plays a major role; regularly shaped particles compact much better than irregularly shaped ones.

Knowing the bulk density is incredibly useful for practical logistics. If you know the volume of a trench that needs filling, bulk density tells you exactly how many kilograms or tons of material to purchase. It is also vital for calculating shipping constraints and figuring out how many trucks are required to transport your purchased materials to the job site.

Average Density of Complex Objects

When an object contains internal voids or is constructed from multiple different materials (such as a ship, a soccer ball, or the human body), we measure its average density. This can still be easily calculated using the standard formula:

$$ρ=\frac{m}{V}$$

For instance, the average density of the human body ranges from 940 to 990 kg/m³ upon full inhalation, and increases to 1010 to 1070 kg/m³ upon full exhalation. A person's exact body density is heavily influenced by their unique physical composition, specifically the ratio of bone mass, muscle tissue, and body fat.

Fascinating Examples of Density in Nature

• The intergalactic medium boasts the lowest density in nature, ranging from just 2×10⁻³¹ kg/m³ to 5×10⁻³¹ kg/m³.
• The average density of our Sun is approximately 1,410 kg/m³, which is about 1.4 times the density of liquid water.
• Granite, a common crustal rock, has a density of 2,600 kg/m³.
• The overall average density of Planet Earth is 5,520 kg/m³.
• Iron has a highly compact density of 7,874 kg/m³.
• Silver's density sits at an impressive 10,490 kg/m³.
• Gold is incredibly dense, measuring 19,320 kg/m³.
• The densest known substances under standard atmospheric conditions are osmium (22,600 kg/m³), iridium (22,400 kg/m³), and platinum (21,500 kg/m³).
• The absolute highest density in the known Universe belongs to black holes. A black hole's average density depends on its mass. A black hole with a mass similar to our Sun has a mind-boggling density of roughly 10¹⁹ kg/m³, far exceeding standard nuclear density (2 × 10¹⁷ kg/m³). Curiously, a supermassive black hole with a mass of 10⁹ solar masses has an average density of just 20 kg/m³—which is vastly less dense than a glass of water (1000 kg/m³).

How to Calculate Density

Today, scientists and engineers utilize several advanced methods and specialized tools to measure the density of materials. These methods include the use of:

• A hydrometer (buoyancy method specifically for liquids).
• A hydrostatic balance (buoyancy method for liquids and solids).
• The submerged body method (buoyancy method for diverse fluids).
• A pycnometer (for liquids and solids).
• An air comparison pycnometer (for solids).
• An oscillating densitometer (for fluids).
• The fill-and-release method (for solids).

However, you can easily calculate the density of a substance or the average density of an object right at home by simply measuring its volume and mass.

First, determine the mass of the object using an accurate digital scale.

Next, determine its volume. For liquids, simply pour the substance into a standard measuring cup or graduated cylinder. For regular solids, you can mathematically calculate the volume by measuring its dimensions (length × width × height). If the object has a complex or irregular shape, you can measure the volume of water the object displaces when fully submerged.

Finally, divide the mass by the volume to find the object's exact density using the formula:

$$ρ=\frac{m}{V}$$

Industrial and Practical Applications of Density

One of the most common everyday applications of density is determining whether an object will float on water. If an object's density is less than water's density, it floats. If it is greater, it sinks.

This is the foundational principle behind maritime engineering. Massive steel ships stay afloat because they are equipped with specialized ballast tanks filled with air. These tanks provide a massive volume with very little mass, drastically reducing the ship's overall average density. This lowered density, paired with the buoyant force of the ocean, keeps the vessel floating smoothly.

Density also plays a critical role in environmental cleanups. Crude oil floats on the surface of the ocean because it is significantly less dense than water. While oil spills are devastating to marine ecosystems, oil's inherent buoyancy keeps it at the surface, making skimming and cleanup operations physically possible.

In manufacturing, the average density index dictates how building materials will behave under real-world stresses, such as prolonged moisture exposure, freezing temperatures, and mechanical load.

Utilizing low-density, high-strength materials in construction and aerospace engineering provides massive environmental and economic benefits. Historically, aircraft and rocket fuselages were built primarily using heavier aluminum and steel. Modern aerospace engineering heavily relies on lighter, less dense materials like titanium and carbon fiber composites. This drastically reduces overall vehicle weight, saves vast amounts of jet fuel, and increases cargo capacity.

Understanding soil density is equally critical in the agricultural sector. If farming soil is too densely packed, it fails to transmit heat properly and can freeze to devastating depths during the winter. When plowed, overly dense soil shatters into massive, unworkable blocks, stunting root development and yielding poor crops.

Conversely, if soil density is too low, water drains through it far too rapidly, depriving plant roots of essential moisture. Additionally, excessively loose soil is highly susceptible to erosion, where heavy rains can wash away the fertile topsoil. Agronomists continually monitor and adjust soil density to guarantee bountiful, healthy harvests.

The Legendary History of Density: Archimedes and the Golden Crown

The fascinating history of density measurement originates in ancient Greece with the brilliant polymath Archimedes. King Hiero II of Syracuse tasked Archimedes with uncovering whether a deceitful goldsmith had embezzled pure gold while forging the King's new crown, secretly replacing it with cheaper silver.

Scientists of the era already knew that pure gold was roughly twice as dense as silver. However, to verify the crown's true composition without destroying it, Archimedes first needed to calculate its exact volume.

The most straightforward method would have been to melt the crown down and hammer it into a perfectly uniform cube. From there, measuring the volume and calculating the density to expose the fraud would have been simple—but King Hiero strictly forbade damaging his royal crown.

The solution came to Archimedes while he was drawing a bath. As he stepped into the tub, he noticed the water level visibly rising. In a stroke of genius, he realized he could calculate the exact volume of the intricately shaped gold crown simply by measuring the volume of water it displaced when submerged.

Overwhelmed by this monumental discovery, Archimedes allegedly leapt out of the bath and ran completely naked through the streets of Syracuse, triumphantly shouting, "Eureka! Eureka!" (In Greek, "Εύρηκα!" translates to "I have found it!").

Archimedes proceeded to test the royal crown. He measured the volume of water displaced by the crown and compared it to the water displaced by a solid bar of pure gold sharing the exact same mass. The experiment revealed that the crown displaced significantly more water than the gold bar. This proved beyond a shadow of a doubt that the crown was larger in volume and therefore made of a less dense, cheaper alloy rather than pure gold. The dishonest jeweler was swiftly caught and punished.

This legendary story gave birth to the popular exclamation "Eureka!", which is still universally used today to celebrate a sudden moment of brilliant insight or a major scientific breakthrough.