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A 1.15 −g sample of dry ice is added to a 745 −mL flask containing nitrogen...

A 1.15 −g sample of dry ice is added to a 745 −mL flask containing nitrogen gas at a temperature of 25.0 ∘C and a pressure of 720 mmHg . The dry ice is allowed to sublime (convert from solid to gas) and the mixture is allowed to return to 25.0 ∘C. What is the total pressure in the flask?

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Answer #1

PV = nRT

molar mass of dry ice (cO2) = 44

no of moles of dry ice = W/G.M.Wt

                                  = 1.15/44 = 0,026 moles

V = 745ml = 0.745L

T = 25C0 = 25+273 = 298K

R =0.0821L-atm/mole-K

P   = nRT/V

= 0.026*0.0821*298/0.745 = 0.85384 atm

Pco2 = 0.85384 *760mmhg =648.9mmHg

Total pressure = PN2   + Pdry ice(co2)

                             = 720+ 648.9 = 1368.9 mmHg >>> answet

                            

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