The volume of 1 ml. of water equals 1 cm3.
A 1.0000 g sample of water will occupy 1.0000 ml in volume, as water has a density of 1 g/ml at 24Β°C. Water's density is close to 1 g/ml across a wide range of temperatures.
A 0.50 mole sample of helium will occupy a volume of 11.2 liters under standard temperature and pressure (STP) conditions, which are 0 degrees Celsius (273.15 K) and 1 atmosphere pressure. At STP, one mole of any gas occupies a volume of 22.4 liters.
A gas sample is most likely to take the shape of and occupy the total volume of its container because gas particles are highly compressible and move freely within the container to fill all available space. Liquids also take the shape of their container but may not occupy the total volume due to intermolecular forces preventing complete expansion. Solids have a fixed shape and volume, so they do not conform to the shape of their container.
419 mL
A 0.50 mole sample of any ideal gas, including helium, will occupy 11.2 liters at standard temperature and pressure (STP), which is defined as 0 degrees Celsius and 1 atm pressure.
Using the ideal gas law, V = (nRT)/P, where V is volume, n is moles, R is the gas constant, T is temperature in Kelvin, and P is pressure, we can calculate the volume to be 7.34 L.
A 0.50 mole sample of helium will occupy a volume of 11.2 liters under standard temperature and pressure (STP) conditions, which are 0 degrees Celsius (273.15 K) and 1 atmosphere pressure. At STP, one mole of any gas occupies a volume of 22.4 liters.
423mL
multiply the mass and the density
A gas sample is most likely to take the shape of and occupy the total volume of its container because gas particles are highly compressible and move freely within the container to fill all available space. Liquids also take the shape of their container but may not occupy the total volume due to intermolecular forces preventing complete expansion. Solids have a fixed shape and volume, so they do not conform to the shape of their container.
419 mL
A 0.50 mole sample of any ideal gas, including helium, will occupy 11.2 liters at standard temperature and pressure (STP), which is defined as 0 degrees Celsius and 1 atm pressure.
If the pressure on a sample of gas is raised three times and the temperature is kept constant, according to Boyle's Law, the volume of the gas will decrease proportionally to maintain a constant temperature. This means the gas will be compressed and occupy a smaller volume.
Liquids and solids are the states of matter that occupy a definite volume. Gases have neither a definite volume nor shape.
mass and volume measurements for any sample liquid should fall along the graph line because liquids have a constant density. Density is mass over volume. Mass equals density which is a constant time volume.
volume =mass/ density volume = 55.932/8.92 = 6.27 cm3
No it does not.
To find the new volume, you can use the combined gas law formula: (P1 * V1) / T1 = (P2 * V2) / T2. Since pressure is constant, it can be eliminated. Rearrange the formula to solve for V2: V2 = (V1 * T2) / T1. Plug in the values: V2 = (20 ml * 323 K) / 141 K = 45.1 ml. So, the sample of gas would occupy 45.1 ml at 50 C.