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Use Boyle's law
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What is universal molar gas constant?
The gas constant (also known as the molar, universal, or ideal gas constant, normally indicated by the symbol R) is a physical constant which is used in many of the fundamental equations in the physical sciences, such as the ideal gas law and the Nernst equation. It is equivalent to the Boltzmann constant, but expressed in units of energy (i.e. the pressure-volume product) per kelvin per mole (rather than energy per kelvin per particle). The gas constant uses the same units as specific entropy.Its value is: : R = 8.314472(15) J · K-1 · mol-1The two digits in parentheses are the uncertainty (standard deviation) in the last two digits of the value. The gas constant occurs in the simplest equation of state, the ideal gas law, as follows: : PV = nRT = nRT / V = RT / Vmwhere: : P: is the absolute pressure : T: is absolute temperature : V: is the volume the gas occupies : n: is the amount of gas (the number of gas molecules, usually in moles) : Vm: is the molar volume
When can volume fraction be equal to mole fraction?
The volume fraction of a substance is equal to the mole fraction for ideal gas mixture
How many kilograms in one cubic meter gas?
That depends upon the temperature, pressure, and type of gas. For more information, study the ideal gas law. One form of the ideal gas law is PV=nRT, where P=pressure, V=volume, n=number of moles of gas, R=0.08206 L-Atm-mol-1-K-1, T=temperature in degrees K. By rearranging this equation, you could calculate the number of moles of gas if you knew the volume, temperature, and pressure of the gas. Then multiply by the molecular weight of the gas to get the grams, and divide by 1000 to get kilograms.
What is the formula for finding pressure?
I suppose you mean the formula for the variation in pressure. The simplest expression of this is, at a fixed temperature,and for a given mass of gas, pressure x volume = constant. This is known as Boyle's Law. If the temperature is changing, then we get two relations: 1. If the pressure is fixed, volume = constant x temperature (absolute) 2. If the volume is fixed, pressure = constant x temperature (absolute) These can be combined into the ideal gas equation Pressure x Volume = constant x Temperature (absolute), or PV = RT where R = the molar gas constant. (Absolute temperature means degrees kelvin, where zero is -273 celsius)
What are two possible uses for physics equations?
Using information about a force to calculate the resulting acceleration..Using the change in the volume of a gas to calculate the change in its pressure.
What is molar and molal volume?
The molar volume at STP(22.4 L/mol) can be used to calculate the molar mass of the gas.
How does the molar volume at standard temperature and pressure depend upon the identity of the gas?
The molar volume doesn't depend on the identity of the gas. One mole of any ideal gas at STP will occupy 22.4 liters.
When a mole of gas occupies 22.4 Liters this is known as?
This is the molar volume of an ideal gas at a given temperature and pressure.
Calculate the density of nitrogen gas, in grams per liter, at STP?
At Standard Temperature and Pressure (STP), which is defined as 0 degrees Celsius (273.15 Kelvin) and 1 atmosphere pressure, the molar volume of an ideal gas is approximately 22.4 liters/mol. The molar mass of nitrogen gas (Nā) is approximately 28.02 grams/mol. To calculate the density (D) of nitrogen gas at STP, you can use the ideal gas law: ļæ½ = Molar mass Molar volume at STP D= Molar volume at STP Molar mass ā ļæ½ = 28.02 ā g/mol 22.4 ā L/mol D= 22.4L/mol 28.02g/mol ā ļæ½ ā 1.25 ā g/L Dā1.25g/L Therefore, the density of nitrogen gas at STP is approximately 1.25 grams per liter.
The molar volume for CO2 and HCl are 22.262 Lmol and 22.244 Lmol Why are these molar volumes slightly less than the ideal molar volume of 22.4 Lmol?
Because neither is an ideal gas. Ideal gas molecules are assumed to be points with no spatial extensions, gas molecules have a finite size. The van der Waals equations of state need to be applied. This is the main reason.
Molar volume of liquid is greater than molar volume of gas. why?
That's not true. The molar volume of a gas is always greater than the molar volume of a liquid. I can't think of any exceptions to this.
What does molar volume mean for a gas?
Molar gas volume is the volume of ONE moel of gas. It only depends on the pressure and temperature, not on the kind of gas. Molar volume at standard temperature and standard pressure is always 22,4 Litres (for any gas)
What form of the ideal gas law would you use to calculate the volume of a gas?
V=nRT/P
What is the volume of one ounce mole of a gas at STP in cubic feet?
The molar volume of an ideal gas at 25 0C and 100 kPa is 0,875 436 4 cubic feet.
How do you calculate the amount of gas required to raise the pressure of a closed vessel to a known value?
If you know the temperature, pressure and volume of the vessel, you can calculate the amount of moles through the Ideal gas law. PV = nRT That is assuming you have ideal conditions. If not, a variance of the ideal gas law can be used in order to get the moles of your gas.
The Combined Gas Law deals with what quantities?
The combined gas relates the variables of pressure (P), volume (V), temperature (T), and molar amount (n). The equation relating these four variables is the Ideal Gas Law of PV = nRT, where R is the Ideal Gas Constant.
How does molar mass effect pressure at a constant temp and volume?
Assuming we are dealing with a gas, the ideal gas equation can be used.P*V = n*R*Twe can solve for n asn = (P*V)/(R*T)R can be defined for a specific gas to give the specific gas constant. In which case, we notate as "R-bar".R-bar = R/atomic massIf the solution under consideration is a liquid or a solid, the ideal gas equation is not valid. Given the volume of the liquid or solid, we can calculate the mass from the density sincedensity = mass/volumeThen we can find the number of moles of the substance by dividing the mass by the molar mass (check your units on this step).mass/molar mass = number of moles
