1 Mol Boron
Atomic Mass: 10.811
n = m/M therefore m = n x M = 10.811g Boron
volume = mass/density
= 10.811 / 2.36
= 4.5809 cm2Boron
For Ideal gases, mole fraction=volume fraction
For solids and liquids, if you know the density in grams per cubic centimeter, and the atomic mass (grams per mole), then you can calculate it. Moles * (atomic mass) / (density) = volume. For gasses: you need to know the Pressure and Temperature, and use PV = nRT, so V = n*R*T/P, then convert to cubic centimeters. Or if at Standard Temperature and Pressure (0°C and 1 atmosphere), an Ideal Gas has a volume of 22.4 liters/mole (22400 cm3 / mole)
You cannot convert cm3 to moles. They do not measure the same quantity. Cubic centimeters measure volume (the amount of space an object takes up) and moles measure the amount of a substance. The mole is one of the seven fundamental SI units, whereas cubic centimeters is a derived unit.
No. A liter is a volume measurement for fluids (liquids and gases). A mole is 6.022 x 1023 of anything. In gases at STP, 22.4L = 1mole.
if the concentration of sugar solution of volume of 360 cm3 cube is 0.785 mol/ dm3 has the mass of 25g of sugar present in the solution. work out for the mole of the sugar content in the solution.
The molar volume of uranium is approximately 12.5 cubic centimeters per mole.
The atomic volume of nickel is approximately 6.59 cubic centimeters per mole.
1.00*10-7 moles of boron is how many grams is this
The atomic weight of boron is approximately 10.81 grams per mole.
Boron's atomic weight is 10.81 grams per mole.
The ideal gas law states that at STP (Standard Temperature and Pressure), one mole of gas occupies 22.4 L of volume. Boron trifluoride (BF3) has a molar mass of 67.8 g/mol. Therefore, 0.155 g of boron trifluoride is 0.155/67.8 = 0.00228 moles. At STP, this amount of boron trifluoride would occupy 0.00228 * 22.4 = 0.051072 L of volume.
chemistry,elements and compounds, atoms amd atomic structure.
For Ideal gases, mole fraction=volume fraction
Mole is not a unit of volume. Mole deals with numbers like dozen.
For solids and liquids, if you know the density in grams per cubic centimeter, and the atomic mass (grams per mole), then you can calculate it. Moles * (atomic mass) / (density) = volume. For gasses: you need to know the Pressure and Temperature, and use PV = nRT, so V = n*R*T/P, then convert to cubic centimeters. Or if at Standard Temperature and Pressure (0°C and 1 atmosphere), an Ideal Gas has a volume of 22.4 liters/mole (22400 cm3 / mole)
if its dm cubed then that means that's the area in cubic meters taken up by a gas like in chemistry 1 mole takes up 24 dm cubed
The volume fraction of a substance is equal to the mole fraction for ideal gas mixture