So you're asking.. Is the volume of gas moles?
In a simple answer, no it is not.
Moles is yes, a unit of measurement.
A mole is a unit of measurement used in chemistry to express the amounts of molecules within a substance.
1 mole is equal to = 6.0022x10^23.
For example, to get one mole of CARBON
You need to get 12g. (Atomic Mass)
But some things can be interpreted as mol/L (this is the molarity of a substance)
the pressure and temperature are held constant. ideal gas law: Pressure * Volume = moles of gas * temperature * gas constant
The space that a gas takes up is called its volume.
The ideal gas law states P*V=n*R*T where P is the pressure of the gas, V is the volume of the gas, n is the amount of substance of gas (also known as number of moles), T is the temperature of the gas and R is the ideal, or universal, gas constant, equal to the product of Boltzmann's constant and Avogadro's constant.
The volume of gas that 3.5 moles of oxygen occupy can be easily found using the relationship of PV=nRT where P is the pressure, V is the volume, n is the moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
1 standard volume of 1 mole of any gas @ STP is 22.4 LSo the # of moles in a 1 L sample will be:1 L*(1 mol/22.4 L) = 0.04464 molSince you already know the mass of the gas @ STP, the molar mass will be mass/#moles1.92 g/ 0.04464 mol = 43.01 g/mol
In the ideal gas law, n represents the number of moles of gas present in the system. It is a measure of the quantity of gas particles and is used to calculate the amount of gas based on the number of moles rather than individual particles.
Properties which a certain amount of gas will maintain include its mass, and the number of moles.
There are three variables in gas work that go into volume: amount of gas, pressure of gas, temperature of gas. If we double the amount of gas - the moles - and maintain the temperature and pressure, the volume must double.
One still has to know the pressure and the amount(moles) of that gas, not which gas is concerned.
The amount of gas (moles) is constant in the combined gas law.
The gas pressure depends on the amount (number of moles), volume and temperature. It is independent from the kind of gas.
The energy needed to go from a liquid to a gas is referred to as heat of vaporization.
The answer is 1,72 moles.
Change it's gram weight into moles using the periodic table.
Yes.The amount of gas is determined by its pressure, volume, and temperature. The equation is:PV = nRTwhere:P = pressure, measured in pascals (the SI derived unit of pressure)V = volumen = amount of substance of gas (moles)R = universal gas constantT = temperature
To calculate the number of moles in 15g of chlorine gas, you need to use its molar mass. The molar mass of chlorine is approximately 35.5 g/mol. Divide the given mass by the molar mass to find the number of moles. For 15g of chlorine gas, you will have about 0.42 moles.
pV_-_nRT">pV_-_nRT">pV - nRTwhere p is the absolute pressure of the gas; V is the volume of the gas; n is the amount of substance of the gas, usually measured in moles; R is the gas constant (which is 8.314472 J·K−1· mol−1 in SI Units); and T is the absolute temperature.boobie jiji