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6.2 Pressure: The Result of Molecular

- The units of the answer are correct.
- One mole of an ideal gas under standard temperature and pressure is 22.4 L. The answer of 0.219 mol is reasonable.

- Determine the pressure inmmHg of a 0.133-g sample of helium gas in a container at 32 degrees.

- The ideal gas law can be applied to three more applications: molar volume, density, and mass.

- We can easily calculate the density of an ideal gas under these conditions with 1 g of Ar.

- The density of a gas can be calculated by using the molar volume.

- Nitrogen is four-fifths lower than air so it tends to rise in air.
- The detailed composition of air is discussed in Section 6.6.

- A balloon filled with either hydrogen or helium floats in the air.

- The ideal gas law can be used to calculate the density of a gas.

- As expected, density increases with increasing mass.

- The density of nitrogen gas is calculated using a pressure of 755mmHg.

- You are asked to find its density.

- The pressure and temperature are given.

- To calculate density, substitute the quantities into the equation.

- The units of the answer are correct.
- The magnitude of the answer makes sense, because earlier you calculated the density of nitrogen gas at STP as 1.25 g>L.
- The density is lower since the temperature is higher.

- The ideal gas law can be used to calculate the mass of an unknown gas.
- We measure the mass and volume of an unknown gas under pressure and temperature.
- The amount of gas in moles is determined by the ideal gas law.

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