Given: Vl = 5.6 L, P1 = 735 mmHg, and V2 = 9.4 L Find: P2 Conceptual Plan: Vlr PI, V2 -» P2 PI v, = P2 v2 Solution: PI V\ = P2 V2 Rearrange to solve for P2. No significant figures to the right of the decimal point can be reported since the mercury height is known only to the 1's place. The magnitude of the answer (820 mm Hg) makes physical sense because the mercury column is higher on the right, indicating that the pressure is above barometric pressure. mm Hg Check: The units (mm Hg) are correct. It will increase as pressure increases or as the molar mass of the gas increases. Since d = - this means that the density will decrease as temperature increases. Substituting these values into the ideal gas law, one can calculate this value as 22.414 L. The molar volume of an ideal gas is the volume occupied by one mole of gas at T = 0 ☌ (273 K) and P = 1.00 atm. Replace the proportional sign with an equal sign by incorporating R (the ideal gas constant) V = RnT / P. Combining these three expressions we get V oc riT / P. We know that V oc 1 / p (Boyle's law) V oc T (Charles's law) V oc n (Avogadro's law). The ideal gas law (PV = nRT) combines all of the relationships between the four variables relevent to gases (pressure, volume, number of moles, and temperature (in kelvin's)) in one simple expression. The warm, less dense air tends to rise in a room filled with colder, denser air. Charles's law also explains why the second floor of a house is usually a bit warmer than the ground floor because when air is heated its volume increases, resulting in a lower density. The gas that fills a hot air balloon is warmed with a burner increasing its volume and lowering its density, and causing it to float in the colder, denser surrounding air.
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It would be impossible to breathe.Ĭharles's law explains why a hot-air balloon can take flight. If the diver had a snorkel that went to the surface-where the air pressure is 1 atm-air would flow out of his lungs, not into them. This is more than the muscles of the chest cavity can overcome- the chest cavity and lungs are compressed, resulting in an air pressure within them of more than 1 atm. A diver at 10 m experiences an external pressure of 2 atm. Extra-long snorkels do not work because of the pressure exerted by water at an increased depth. Because of this pressure differential, the lungs expand, the pressure in them falls, and air from outside our lungs then flows into them.
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When we breathe, we expand the volume of our chest cavity, reducing the pressure on the outer surface of the lungs to less than 1 atm (Boyle's law). What would happen to the volume of air in the diver's lungs? Since the pressure decreases by a factor of 3, the volume of the air in the diver's lungs would increase by a factor of 3, severely damaging the diver's lungs and possibly killing the diver. Suppose that a diver inhaled a lungful of air at a pressure of 3 atm and swam quickly to the surface (where the pressure drops to 1 atm) while holding this breath. For example, when a diver is at a depth of 20 m below the surface, the regulator delivers air at a pressure of 3 atm to match the 3 atm of pressure around the diver (1 atm due to normal atmospheric pressure and 2 additional atmospheres due to the weight of the water at 20 m). The pressure regulator used in scuba diving delivers air at a pressure that matches the external pressure otherwise the diver could not inhale the air. There are 0.9763 Atm in 742 mmHg, or 742 mmHg = 0.9763 Atm.For every 10 m of depth that a diver descends in water, they experience an additional 1 atm of pressure due to the weight of the water above her.
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To calculate how many Atm in 742 mmHg, divide the value by 760. Online Calculators > Conversion > 742 mmHg to Atm 742 mmHg to Atmħ42 mmHg to Atm conversion calculator convert 742 mmHg to Atm and vice versa.