1. (3 & 4) Give the value for standard atmospheric pressure in each of the follo

Question

1. (3 & 4) Give the value for standard atmospheric pressure in each of the following units: A) millimeters of mercury B) centimeters of mercury C) inches of mercury D) PSI 2. (5) If oxygen gas in a steel container is at a pressure of 5.00 atm, what is the pressure expressed in each of the following units? A) psi B) inch Hg C) pascals 3. (63)If 0.500 mol of hydrogen gas occupies 5.00 liters @ 25 degree C, what is the pressure in atmospheres? 4. (47)Air contains nitrogen, oxygen, argon, and trace gases. If the partial pressure of nitrogen is 592 mm Hg, oxygen is 160 mm Hg, argon is 7 mm Hg, and trace gas is 1 mm Hg, what is the atmospheric pressure? 5. (76)What volume in liters is occupied by 3.38 x 10^22 nitrogen molecules at 100 degree C and 255 mm Hg?

Explanation / Answer

1) standard atmospheric pressure

760 mm of Hg

76 cm og Hg

29.92 inches of Hg

14.696 psi ( pounds per square inch)

2) oxygen has a pressure of 5 atm

A) in psi = 5*14.696 = 74.845 psi

B) in inches of Hg = 5*29.92 = 149.6 inches of Hg

C) 1 atm = 101.325 kPa

5 atm = 5*101.325 kPa = 506625 Pa.

3) PV = nRT

V = 5 litres and T = 25 C = 25 + 273 = 298 k.

n= 0.5 and R=0.0821

so P=nRT/V = 0.5*0.0821*298/5 = 2.44 atm

4) here all the gases given are non reacting gases theerfore according to

Dalton's Law the total pressure is equal to the individual partial pressures.

total pressure = 592 mm + 160 mm + 7 mm + 1 mm = 760 mm of Hg = 1 atm

5) 1 mole contains 6.022 * 10^23 molecules

given are 3.38*10^22 molecules

so number of moles = 0.056 mol = n

T = 100C = 100 + 273 = 373 K

P=255 mm of Hg

1 atm = 760 mm of Hg

so 255 mm of Hg = 0.335 atm

PV = nRT

V = nRT/P = 0.056*0.0821*373/0.335 = 5.12 litres

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