3.14.2017 | Jennifer Bargeman

The ideal gas law specifies that the **volume** occupied by a gas depends upon the amount of substance (gas) as well as temperature and.

The gas constant is expressed in the International System of Units (SI) and, hence, other parameters in the ideal gas equation must be in SI units as well. Record the molar gas constant "R". R = 8.314472 J/mole x K.

Nitrogen gas has a molar mass of 28 g/mole, so 56 g of the gas is equivalent to 2 moles. Divide the mass of the gas weight by its molar mass to calculate n -- the number of moles.

In our example, the *volume* of the nitrogen gas is 0.022414 x 2 = 0.044828 cubic meters or 44.828 liters. Multiply the coefficient 0.022414 by the number of moles to calculate the gas volume (in cubic meters) at the standard temperature and pressure.

Helium has a molar mass of 4 g/mole, so 1 gram of the gas produces a balloon with a volume of 5.6 liters -- a little over a gallon -- at STP. If you filled the balloon with 1 gram of nitrogen gas instead, the balloon would shrink to 1/7 of that size, or 0.81 liters.

Substituting these conversion in the ideal gas law produces a value of RT/P that is 0.022414 cubic meters/mole at STP. Thus, at STP, the ideal gas law can be written V = 0.022414n. Convert pressure from atmospheres (atm) to Pascals (Pa) -- the SI units -- by multiplying by 101,325. Convert from degree Celsius to Kelvins -- the SI units for temperature -- by adding 273.15.

Standard temperature and pressure -- usually abbreviated by the acronym STP -- are 0 degrees Celsius and 1 atmosphere of pressure. An example would be to calculate the volume that 56 g of nitrogen gas occupies. The ideal gas law specifies that the volume occupied by a gas depends upon the amount of substance (gas) as well as temperature and pressure. Parameters of gases important for many calculations in chemistry and physics are usually calculated at STP.

It can be written as: V = nRT/P. Get familiar with the ideal gas law. "P" is pressure, "V" is volume, n is the number of moles of a gas, "R" is the molar gas constant and "T" is temperature.

9.20.2017 | Jennifer Bargeman

Temperature and pressure are defined as 0°Celsius, and 1.00 atmospheres, respectively. Avogadro determined that the **volume** of any gas measured at STP is.

How many liters does 3.7 moles of oxygen gas (O 2 ) at STP occupy? Answer:. 1.

STP Formula Questions:. It is key to remember that the STP value of 22.4 L can only be considered for gaseous particles. This value is used in many gas conversions from liters to moles, or vice-versa, as long as the STP conditions are met.

This problem requires that the grams of methane gas be converted into moles before using Avogadro's value.

Avogadro determined that the *volume* of any gas measured at STP is 22.4 L. STP is a shortened version of the words standard temperature and pressure. Standard temperature and pressure are defined as 0°Celsius, and 1.00 atmospheres, respectively.

First, find the molar mass of CH 4.

2. How many liters does 45.3 grams of methane gas (CH 4 ) at STP occupy? Answer:.

Now, set up the problem and solve.

12.23.2017 | Logan Miers

Standard Molar **Volume** is the volume occupied by one mole of any gas at STP. Remember that "STP" is Standard Temperature and Pressure. Standard.

Conversely, the number of moles present in any *volume* of gas at STP can also be determined, and if the identity of the gas is known, this number of moles can be converted to a mass. Using this information, the volume occupied by any number of moles (or grams) can be determined. 1 mole of any gas at STP occupies 22.4 liters of volume.

What is the molar mass of gas that has a density of 1.97 g/L at STP?

Identify the gas. One liter of a certain gas has a mass of 0.179 grams at STP.

What volume is occupied by 100.0 grams of chlorine gas (Cl 2 ) at STP?

Which of the following gases is the densest?

What is the density of oxygen gas (O 2 ) at STP?

What volume is occupied by 5 moles of any gas at STP?

What volume is occupied by 12.5 moles of nitrogen gas at STP?

Remember that "STP" is S tandard T emperature and P ressure. Standard Molar Volume is the volume occupied by one mole of any gas at STP. Standard pressure is 1 atmosphere or 760 mm Hg (also called "torr"). Standard temperature is 0 ° C or 273 K.

Show all questions. Standard molar volume is also useful for Density determinations at STP. density at STP = mass of one mole / 22.4 liters If the molar mass can be determined, from the chemical formula, for instance, then the density can be calculated. If the density is known, then the molar mass can be determined.

What is the density of ethane gas, C 2 H 6, at STP?

Use a calculator and a periodic table to complete this exercise.

What is the mass in grams of 17.0 liters of methane gas (CH 4 ) at STP?

How many liters will 48.6 grams of CO 2 occupy at STP?

4.15.2017 | Jennifer Bargeman

Chemistry Gases Molar **Volume** of a Gas. Using the Ideal Gas Law, you would find the volume of 1 mole of a gas at Standard Temperature and Pressure (STP). If 4.00 moles of gasoline are burned, what volume of oxygen is needed if the pressure is 0.953 atm.

#P V = n R T # solves to #V = (n R T) / P#

Describe your changes (optional) 200.

SMARTERTEACHER. I hope this was helpful.

Using the Ideal Gas Law, you would find the *volume* of 1 mole of a gas at Standard Temperature and Pressure (STP).

STP = 1 atm of pressure and 273 K for temperature.

V = 22.41 L of gas @ STP.

#V = (1 cancel(mol) (0.0821 (cancel(atm)L))/(cancel(mol) cancelK) 273cancelK)/(1cancel(atm))#

P = 1 atm V = ??? n = 1 mole R = 0.0821 atm L/mol K K = 273 K.

10.21.2017 | Logan Miers

The **volume** of gas at STP is the volume occupied by gas at standard temperature and pressure. The standard value of temperature is 0oC or 273.15 K and the.

2017 - TutorVista.com.

The most commonly used conditions are STP (Standard temperature and pressure) conditions. The *volume* of a given mass of gas changes with temperature and pressure. Therefore, to compare the *volumes* of different gases, they have to be taken or converted to same conditions of temperature and pressure using ideal gas equation.