A mixture of two gases (gas X and gas Z) is pumped into a sealed container half-way filled with 5.0 L of water. The total pressure of the gases over the water is 1.34 atm. If the pressure of gas Z is 0.52 atm. How many grams of gas X are in the water if the molar mass for gas X is 22.31 g/mol? The Henry's law constant for gas X is 0.0266 mol/(L-atm).

A mixture of two gases (gas X and gas Z) is pumped into a sealed container half-way filled with 5.0 L of water. The total pressure of the gases over the water is 1.34 atm. If the pressure of gas Z is 0.52 atm. How many grams of gas X are in the water if the molar mass for gas X is 22.31 g/mol? The Henry's law constant for gas X is 0.0266 mol/(L-atm).

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

A bubble has a volume of 5.00 at the surface of an outdoor bathtub where the total pressure is 0.975 atm. What is the volume of the bubble when it floats far away from where the pressure is only 0.500 atm Assume that the outdoor temperature remains the same.
What is the mole fraction of O2 in a mixture of 6.00 g He, 19.0 g O2, and 21.0 g N2? 0.608 0.253 0.410 0.209 0.267
5. A sample of helium gas, He, has a volume of 1.80 L, a pressure of 8.00 atm at a temperature of 39 °C. At what temperature (°C) will the helium have a volume of 49.0 mL and a pressure of 420 mmHg (n constant)? 6. How many milliliters of 8.95% (v/v) ethanol solution can be prepared from 50.25 mL of ethanol?
If a gaseous mixture of He, Ne, and N2 has a pressure of 871 mm Hg, what is the partial pressure of N2, in mm Hg, if He and Ne have partial pressures of 775 mm Hg and 83 mm Hg, respectively?
Use Charles's law to complete the table. (Assume pressure and number of moles of gas to be constant.) Part V1V1 T1T1 V2V2 T2T2 A 117 LL 10.5 ∘C∘C __ 122.0 ∘C∘C B __ 133 KK 174 LL 319 KK C 2.08 LL 14.5 ∘C∘C 2.33 LL __ D 16.2 cm3cm3 __ 18.9 cm3cm3 11.1 ∘C∘C Complete the first row of the table. Express the volume in liters to three significant figures.
b In the boiling-water bath, the gas pressure increased. In the ice-water bath, the gas pressure decreased. Explain why these pressure changes did not affect your Charles' law calculation. 234 5 Did your experiment provide evidence consistent with Gay-Lussac's and Boyle's laws? Explain your answer. 6 When canning jams and jellies, a small air space is left between the top of the jam and the jar lid, which is only loosely tightened. The jar is then submerged in boiling water for several minutes. During this time, bubbles are observed emerging from the jar. After the jar is removed from the hot water, the lid is soon heard "popping down" tightly on the jar to seal it. a Explain why bubbles are observed to emerge from the jar when it is in the boiling water. b Explain why the lid "pops down" on the jar top soon after removing the jar from the boiling water. Ven Exercises for the General, Organic, & Biochemistry Laboratory
Describe Boyle's Law, Charles' Law, and Avogadro's Law in your own words? What is the ideal gas constant? Describe how the volume of a gas can be determined using the ideal gas constant?
7. A sample of an ideal gas has a volume of 2500 ml at STP. What is the volume if the pressure is doubled and the temperature is decreased to 75°K? 8. Explain, in terms of electronegativity difference, why the bond between hydrogen and oxygen in a water molecule is more polar than the bond between hydrogen and nitrogen in an ammonia molecule. How many grams of each solute will dissolve in 100 g of water? a) KI at 10°C 9. c) KCIO, at 90°c b) HCl at 60°C d) KNO, at 50°C 10. Find the percent composition of nitrogen in ammonium bromide.
A gaseous mixture contains 401.0 Torr H2(g), 367.7 Torr N2(g), and 89.9 Torr Ar(g). Calculate the mole fraction, ?, of each of these gases. ?H2= ?N2= ?Ar=