Differentiate solids, liquids & gases in terms of volume & shapes.

The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The ideal gas law is typically written as ??=???PV=nRT where ?P is the pressure, ?V is the volume, ?n is the number of moles of gas, ?R is the ideal gas constant, and ?T is the temperature. Rearrange the equation to solve for ?.P. ?=P=     What is the pressure of 0.638 moles0.638 moles of an ideal gas at a temperature of 297.0 K297.0 K and a volume of 5.58 L?5.58 L? ?=P=   atm

(A). A sample of krypton gas at a pressure of 1.00 atm and a temperature of 24.3 °C, occupies a volume of 818 mL. If the gas is compressed at constant temperature until its pressure is 1.27 atm, the volume of the gas sample will be ---------  mL. (B) A sample of neon gas at a pressure of 0.812 atm and a temperature of 29.8 °C, occupies a volume of 16.3 liters. If the gas is compressed at constant temperature to a volume of 5.59 liters, the pressure of the gas sample will be------------  atm.

Determination of the Atmospheric Pressure 1. The atmospheric pressure on a spring day in Minnesota was found to be 762 mm Hg. a. What would the pressure be in cmm H₂O? 762mm Khi ha 10 mmHg •Hg.. 13.57cm 1 cm Ha H₂0 = 1,034.034 h. About how many meters of water would it take to exert that pressure? 1.03x/0³ P=mt + b where m is the slope of the line and b is a constant. a. What is the slope of the lime? (Find the change in P divided by the change in 1.) cmm H₂O 2. In this experiment a student found that when she increased the temperature of a 544 mL sample of air from 22.8°C to 33.6°C, the pressure of the air went from 1012 cm H₂O up to 1049 cm H₂O. Since the air expands linearly with temperature, the equation relating P to t is of the form: b. Find the value of b. (Substitute known values of P and into Equation 9 and solve for b.) H₂O cm H₂O/°C cm H₂O (continued on following page)

A small helium tank is about two feet (60 cm) high. Yet it can fill over 50 balloons! How can sucha small tank contain enough helium to fill so many balloons?

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Answer the following questions:(a) Is the pressure of the gas in the hot air balloon shown at the opening of this chapter greater than, less than, or equal to that of the atmosphere outside the balloon?(b) Is the density of the gas in the hot air balloon shown at the opening of this chapter greater than, less than, or equal to that of the atmosphere outside the balloon?(c) At a pressure of 1 atm and a temperature of 20 °C, dry air has a density of 1.2256 g/L. What is the (average) molar mass of dry air?(d) The average temperature of the gas in a hot air balloon is 1.30 × 102 °F. Calculate its density, assuming the molar mass equals that of dry air.(e) The lifting capacity of a hot air balloon is equal to the difference in the mass of the cool air displaced by the balloon and the mass of the gas in the balloon. What is the difference in the mass of 1.00 L of the cool air in part (c) and the hot air in part (d)?(f) An average balloon has a diameter of 60 feet and a volume of 1.1 × 105…

If an electric current is passed through molten sodium chloride, elemental chlorine gas is generated as the sodium chloride is decomposed. :math>2NaCl(1)2Na(s)+Cl2(g) at volume of chlorine gas measured at 767 mm Hg at 25 °C would be generated by complete decomposition of 1.25 g of NaCl?

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Use the References to access important values if needed for this question. Tire pressure gauges are often calibrated in pounds per square inch. An automobile tire is inflated to a pressure of 31.4 psi. Express this pressure in atmospheres and in millimeters Hg. Hint: 1 atm = 760 mmHg = 14.7 psi %3D Pressure atm %3D Pressure = mmHg