# What is the pressure in #mm*Hg# if a #4.0*g# mass of oxygen gas at #303*K# was confined to a container whose volume of #3000*mL#?

Using the Ideal Gas Equation, we can obtain.....

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To find the pressure, we can use the ideal gas law equation: PV = nRT. First, convert grams to moles: ( n = \frac{m}{M} ). ( n = \frac{4.0 , \text{g}}{32.00 , \text{g/mol}} = 0.125 , \text{mol} ). Next, plug the values into the ideal gas law equation: ( P = \frac{nRT}{V} ). ( P = \frac{(0.125 , \text{mol})(0.08206 , \text{atm} \cdot \text{L/mol} \cdot \text{K})(303 , \text{K})}{3.00 , \text{L}} ). ( P = 3.74 , \text{atm} ). To convert atm to mmHg, use the conversion factor: 1 atm = 760 mmHg. ( P = 3.74 , \text{atm} \times 760 , \text{mmHg/atm} ). ( P = 2842.4 , \text{mmHg} ).

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

- What mole is occupied by #1*mol# of gas under standard conditions?
- How should liquid nitrogen and liquid oxygen be stored and dispensed? What safety equipment and precautions are employed?
- What happens to hydrogen atoms at very high temperatures?
- Given equal masses of dihydrogen, and other gases, which gas will exert MORE pressure?
- Who discovered the Ideal Gas Law?

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