A sealed flask contains a mixture of hydrogen, oxygen, and nitrogen gases. The gases 11 A exert a total pressure of 92.6 kPa. If the partial pressure of the hydrogen and the nitrogen are 31.2 kPa and 18.7 kPa respectively, what would be the partial pressure exerted by the oxygen? A 42.7 kPa B 101 kPa C 142.5 kPa D 49.9 kPa

A sealed flask contains a mixture of hydrogen, oxygen, and nitrogen gases. The gases 11 A exert a total pressure of 92.6 kPa. If the partial pressure of the hydrogen and the nitrogen are 31.2 kPa and 18.7 kPa respectively, what would be the partial pressure exerted by the oxygen? A 42.7 kPa B 101 kPa C 142.5 kPa D 49.9 kPa

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Some N2 gas is mixed with some O2 gas, and The picture shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 1.55atm. Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to three significant digits. You may assume each gas behaves as an ideal gas.
43
A 3.35 g sample of an unknown gas at 79 °C and 1.00 atm is stored in a 2.15 L flask. What is the density of the gas? density: g/L What is the molar mass of the gas? molar mass: g/mol
[Review Topics] [References] Use the References to access important values if needed for this question. A mixture of nitrogen and xenon gases is maintained in a 6.27 L flask at a temperature of 75°C. If the partial pressure of nitrogen is 0.221 atm and the partial pressure of xenon is 0.290 atm, the total pressure in the flask is atm. Submit Answer Retry Entire Group G 26c to k - Google 9 more group attempts remaining Previous Next Save and Exit
In a mixture of argon and hydrogen, occupying a volume of 1.54 L at 860.0 mmHg and 31.0 oC, the mass of the argon is 1.6 g. What is the partial pressure of argon? 41.3 mmHg 819 mmHg 491 mmHg 430 mmHg 369 mmH
Sodium chlorite reacts with chlorine gas to form chlorine dioxide gas and sodium chloride. Calculate the liters of chlorine dioxide gas at STP conditions from a reaction with 9.85 g of sodium chlorite. 0.0545 L 1.22 L 2.96 L 2.44 L 110. L
A 3.85 g sample of an unknown gas at 73 °C and 1.05 atm is stored in a 1.35 L flask. What is the density of the gas? density: g/L What is the molar mass of the gas? molar mass: g/mol
A quantity of helium gas is originally held under a pressure of 145 kPa at 18°C. If the volume of the container is tripled, and the temperature is increased to 30°C, what is the resulting pressure in kPa? (Hint, can you make up a volume?) H 322181 Li Na Mg Rb Be Sr Cs Ba Fr 22 Ca Sc Ti Ra Raden Lat 94.5 kPa 46.4 kPa 378.3 kPa 453.9 kPa 50.3 kPa MD 45 83-103 482.2 kPa Zr Hf Atvice Ac Th Series 23 VO Vieta VID 24 2 Ta W Tete 104 105 Rf Db Sg Cr Mn Periodic Table of the Elements VID 75 41. 34445 Nb Mo Tc Ru Rh Pd Ag Cd Abaline Tra Saber 26 27 28 29 30 Fe Co Ni Cu Zn Re Os Symbol S 13 13 FIA B Nawww Al Ga Halagan In La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho D IVA 70 Pt Au Hg Tl Pb B Mar 102108, 109 114 Bh Hs Mt Ds Rg Cn Uut "FI 590 U Np Pu Am Cm Bk Cf Es Sn Sb 14 15 16 17 18 Si CI Ar La 16 3514. Ge As Se Br Kr By 17 VIA 18 VELA He Hek 4000 Ne 62 63 64 SA Te I Xe 16 At Rn Fate Bi Po Uup "Lv Uus Uuo Er Tm Yb Lu C Henan 100 100 Fm Md No L
If 3.220 L of fluorine gas reacts with excess xenon gas both at 2.000 atm and 450.0 K, how many grams of xenon tetrafluoride can form? The balanced equation is 2 F2 (g) + Xe (g) --> XeF4 (s) a. 58.04 g b. 18.08 g c. 10.95 g d. 29.02 g e. 0.1744 g f. 14.51 g g. 21.89 g h. 47.53 g i. None of these j. 0.1056 k. 36.15 g
3. A certain mass of magnesium is reacted with 6M HCl. The hydrogen gas liberated is collected by displacing 200 mL of water. The pressure of the gas and the atmospheric pressure are equalized. The atmospheric pressure is 762 mmHg. The temperature of the experiment is 27°C. How many moles of hydrogen have been liberated, and what is the mass of the magnesium that reacted?
19. 1.18 g of Ar(g) occupies 2.00 L. container at the temperature of 25 °C. Calculate the pressure in mmHg. molar mass of Ar = 39.95 g/mole O 22.1 mmHg O 275 mmHg O 118 mmHg O 0.0156 mmHg
A 3.05 g sample of an unknown gas at 21 °C and 1.10 atm is stored in a 1.95 L flask. What is the density of the gas? density: g/L What is the molar mass of the gas? molar mass: g/mol