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∙ 11y agoAvogadro's number is the number of molecules in a mole of a substance. This is expressed as 6.022 141 29 E23 /mol. This is defined as the number of atoms in 12 grams of carbon12. A mole of any gas has this number of molecules. Any fraction of that mole must be divided into the number.
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∙ 11y agoNone of those!
True
0.7334 liters
Cubic measures of length, or litres.
The volume cannot be 1 centimetre since that is not an appropriate unit for measuring volume.
None of those!
Increasing the number of molecules in a fixed volume will result in an increase in pressure due to more frequent collisions between molecules. This relationship is described by the ideal gas law, where pressure is directly proportional to the number of molecules and temperature, and inversely proportional to volume.
When density increases, the number of molecules in a volume stays the same. Density is defined as mass per unit volume, so as the mass increases, there needs to be a proportional increase in the number of molecules to maintain the density.
Yes, molecules play a role in determining the volume of a substance. The number and size of molecules in a substance affect its density, which in turn influences its volume. Additionally, the packing arrangement of molecules in a substance can determine its overall volume.
Heat, number of molecules, atmospheric pressure and volume Volume * Pressure = molecules * molar gas constant * Heat
Assuming the density of acetone is 0.79 g/ml, and the molar mass of acetone is 58.08 g/mol, you can calculate the number of acetone molecules in 330 ml using Avogadro's number. This will give you approximately 6.69 x 10^23 molecules of acetone in a 330 ml bottle of acetone.
Since carbon dioxide (CO2) has a molar mass of 44 g/mol and molecular oxygen (O2) has a molar mass of 32 g/mol, the molar ratio is 44:32. Therefore, you would need less volume of CO2 to contain the same number of molecules as 20 ml of O2 at the same conditions. The exact volume can be calculated using the ideal gas law equation PV = nRT.
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Decreasing the number of gas molecules typically decreases the volume of the gas, assuming pressure and temperature remain constant. This is because there are fewer molecules colliding with the container walls, reducing the pressure and allowing the gas to occupy a larger volume to maintain equilibrium.
The number of molecules in a given amount of volume is called the concentration of the solution. It is typically measured in units such as moles per liter (mol/L) or molarity.
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If the volume is doubled and the number of molecules is doubled while the temperature is held constant, the pressure of the gas sample will remain the same. This is because both the volume and the number of molecules increased by the same factor, resulting in no net change in pressure according to the ideal gas law.