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What is the density of a 25g piece of metal that has a volume of 10 cm cubed?
density = mass/volume,so the density of your metal is:25/10 = 2.5g/cm3 (grams per cm cubed)
What is density of the unknown metal that has of mass 158g and volume of 20mL?
Density is found by dividing Mass by volume where mass is in grams and volume is in milliliters. 20 liters=20,000 ml so the calculation becomes 158/20,000 which yiels a result of .0079
A metal cube volume is 4cm3 and has a mass of 8 grams what is its density?
Assuming that the metal's density is measured in grams per centimeter cubed (and not, for instance, grams per liter), the volume is found by dividing the mass by the density. In this case, it's approximately 2.341 centimeters cubed.
A metal with a mass of 71.68 g occupies a volume of 8.00 cm3. Calculate the density of the metal. Using Table 1 in our lesson determine the identity of the metal?
To calculate the density of the metal, use the formula: density = mass/volume. Given the mass is 71.68 g and the volume is 8.00 cm³, the density is 71.68 g / 8.00 cm³ = 8.96 g/cm³. Referring to Table 1, this density closely matches that of copper, which typically has a density of around 8.96 g/cm³. Therefore, the metal is likely copper.
What formula do you use to calculate the density of an object?
The formula to calculate density is: Density = mass / volume. You simply divide the mass of an object by its volume to find its density. Density is a measure of how much mass is contained in a given volume.
What experimental method can determine the density of metal?
Density is the mass of the object divided by its volume. By this principle, to determine the density of a metal, place the metal onto a scale to measure its mass. After this, place the metal into a beaker of water and measure the volume change in the beaker. Divide the mass by the volume and you get the density.
How do you measure the density of a metal?
-- Get a pure piece of it. The size of the piece doesn't matter. -- Measure the mass of the piece. -- Measure the volume of the piece. -- The density of the substance is mass of the piece/volume of the piece.
What is the density of a metal that has a mass of 35000 KG and a volume of 4.0 m³?
The density of the metal is 8750 kg/m³. Density is calculated by dividing the mass of an object by its volume.
What is the density of an unknow metal that has a mass of 158 g and a volume of 20m?
The density of the metal is calculated by dividing mass by volume. In this case, the density is 7.9 g/cm^3.
What is the density of a piece of metal that has a mass of 277G and a volume of 38cm3?
The density of the metal can be calculated using the formula: Density = Mass / Volume. In this case, Density = 277g / 38cm3 = 7.29 g/cm3.
What two pieces of information about the metal do you need to determine its density?
To determine the density of a metal, you need to know its mass (in grams) and its volume (in cubic centimeters). Density is calculated by dividing the mass of the metal by its volume.
What volume of water would be displaced by 13.3543 g of a metal with a density of 7.51?
The first step is to calculate the volume of the metal using its density and mass. Volume = mass / density = 13.3543 g / 7.51 g/cm^3 = 1.779 cm^3. Therefore, 1.779 cm^3 of water would be displaced by the metal.
What is the equation for mass volume and density?
Mass = Density x Volume Density = Mass/Volume Volume = Mass/Density
What is the density of a metal block that has a mass of 750 g and the volume of 55 cm3?
Density = Mass/Volume = 13.6 g/cm3
What is the volume of a piece of metal if the density is 2.3glml and the mass is 1.5g?
Density = Mass/Volume so Volume = Mass/Density. That is, Vol = 1.5 g/2.3 g/ml = 0.652 ml approx.
What is the density of a metal cube its mass is 0.6g and volume of 1cm3?
If its mass is 0.6 g and its volume is 1 cm3 , then its density is 0.6 g per cm3 .
What is the density of a piece of metal that has a mass of 68g and a volume of 6 cm3?
The density of the metal is 11.33 g/cm3. This is calculated by dividing the mass (68g) by the volume (6 cm3).
