Use the gas constant. 0.0831442 L bar/mol K. and the following conversion factor

Question

Use the gas constant. 0.0831442 L bar/mol K. and the following conversion factors: 76 cm Hg/atm. 1.01325 bar/atm, 1000 mL/L 1 atm/14.7 psi. 1 Torr/1 mm Hg. 1 cm3/mL; to calculate answer the following problems. What la the volume per n>>ole ot gas at 25.0O degree C and 1.00 atm? How many moles are in 64.21 cm^3 O_2 at 22.3degreeC and 0.9531 bar? What pressure will 192 mol of CO_2 exert at 25 degree C when It occupies 2.50L? What is the temperature of 0.01937 mol H_2 at 121.7 Torr when it occupies 4.137L? What is the volume of 1.000 mol Ar at -191 degree C and 23.94 cm Hg?

Explanation / Answer

1. PV = nRT

     V   = nRT/P

         = 1*0.0821*298/1   = 24.4658L

2. P = 0.9531bar = 0.94atm

   V   = 64.21cm3   = 0.06421L

   T = 22.3C0   = 22.3+273 = 295.3K

   PV = nRT

   n   = PV/RT

         = 0.94*0.06421/0.0821*295.3   = 0.00249moles

3. PV = nRT

   P   = nRT/V

         = 192*0.0821*298/2.5   = 1878.97atm

4. P   = 121.7torr = 121.7/760 = 0.16atm

   V = 4.137L

   PV = nRT

   T    = PV/nR

         = 0.16*4.137/0.01937*0.0821   = 416.23K

5. P = 23.94cmHg   = 279.4mmHg = 279.4/760 = 0.367atm

V =

n = 1

T = -191C0 = -191+273 = 82K

PV = nRT

V = nRT/P

      = 1*0.0821*82/0.367   = 18.34L

            

Related Questions

Navigate

• Browse (All)
• Browse U
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.