Question

11. During laparoscopic surgery, carbon dioxide gas is used to expand the abdomen to help create a larger working space. If 4.80 L of CO2 gas at 18°C at 785 mmHg is used, what is the final volume, in liters, of the gas at 37 °C and a pressure of 745 mmHg, if the amount of CO2 does not change? 12. A mixture of nitrogen (N2) and helium has a volume of 250 ml at 30 °C and a total pressure of 745 mmHg. a. If the partial pressure of helium is 32 mmHg, what is the partial pressure of the nitrogen? b. What is the final volume, in liters, of the nitrogen at STP? 13. What is the total pressure, in millimeters of mercury, of a gas mixture containing argon gas at 0.25 atm, helium gas at 350 mmHg, and nitrogen gas at 360 Torr? 14. Calculate the mass percent (m/m) of a solution containing 26 g of K2CO3 and 724 g of H2O.

Answer 1

11. Initial volume of Co₂ (V4) = 4.80L Initial temperature (Tl) = 18°c Initial pressure (P₂) = 785 mm Hg Final temperature (I.)= 37°C final pressure (12) = 745 mm Hg Final Volume of Co (V2) = ? Amount of Co, remains constant. Ans. From ideal gas equation, we have As per the question, y = 2 Rearrange for a P₂ T1 Convert temperature to Kelvin scale, Ti = 18°C → (18+273 = 291 K) T = 37C (37+273 = 310k) Solve for by substituting values in equation (1): V = (785 mm Hg) (4.80L) ( 310K) - 745 mm Hg) (291K) Hence, the final volume of Co, is 5.39 h. = 5:39)

12. Volume of mixture (v)= 250 ml Temperature = 30°c Pressure (P) = 745 mmHg a) Partial pressure of He (Pre) = 32 mm Hg Partial pressure of ₂ (PN, ) = ? P = Pp-Phe - (1) Calculate PN by substituting values in equation (1), = 745 mm Hg - 32 mm Hg = 713 maig Hence, the partial pressure of ų is 713 mm Hg. - b) Final volume of M at STP=? Here we have mixture (intially) STP(finally) Pressure 713 mm Hg 760 mm Hg Temperature | 30°c (3036) 273K Volume 250 mL (0.25L) 1 Using there values and ideal gas equation, - PA V Tz (113 mm Hg)(0.25L) (273K) BTA - (760 mm Hg) (303 k) = 0.21L Hence, the final volume of at STP is 0.21L.

13. Partial pressure of Ar (PAM) = 0.25 atm Partial pressure of He (PH2) = 350 mm Hg Partial pressure of N (PN) = 360 Toor Ans. convert the units of Pari 0.25 atrix (760 mm Mo) - 190 mmila Convert the units of Prei 360 Tone X / 1 mm Hg) = 360 mmily ( 1 abm To tal pressure (P) = Part Phet PN = (190 + 350+360) mm Hg - 900 mm Hg Hence the total pressure is 900 mm Hg. Mass of K₂ CO₂ = 26 g Mass of H₂O = 724g Mass percent (m/m) = ? Mass of the solution (M) = m. lo + mago 14. Ans. = (26 +124) g = 750g Mass percent = (mass of solute x100- (mass of solution) (750g) 409 Jy 100% = 3.47), Hence, the mass percent of the solution is 3.47% = 1269