Dry ice is solid carbon dioxide. It sublimes readily. Suppose there is a 25.0 liter glass bottle containing nitrogen at 382 mm Hg and 31 °C. A 31.8 gram sample of dry ice is placed into this bottle without any nitrogen escaping. There is no chemical reaction and the temperature remains constant. After the entire sample of dry ice has sublimed: 8-6. What is the partial pressure of the CO, gas in the bottle? a. b. What is the total pressure in the bottle? C. What is the mole fraction of CO, gas in the bottle?

Dry ice is solid carbon dioxide. It sublimes readily. Suppose there is a 25.0 liter glass bottle containing nitrogen at 382 mm Hg and 31 °C. A 31.8 gram sample of dry ice is placed into this bottle without any nitrogen escaping. There is no chemical reaction and the temperature remains constant. After the entire sample of dry ice has sublimed: 8-6. What is the partial pressure of the CO, gas in the bottle? a. b. What is the total pressure in the bottle? C. What is the mole fraction of CO, gas in the bottle?

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

In Dalton's Law of Partial Pressures: Ptrapped gas = Pdry gas + Pwater vapor Why must the pressure of water vapor be included in this calculation? a. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor, thus Pwater vapor has to be added to Pdry gas. b. Some of the liquid water evaporates into the gas, and increases the total pressure generated by the trapped gas. c. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by water in the aqueous solution, effectively decreasing the measured pressure above. d. The pressure contributed by the H2(g) is greater than the measured total pressure because of the contribution of partial pressure of water vapor.
A gas storage cylinder in an ordinary chemical laboratory measures 7.1 cm wide and 28. cm high. This is the label on it. Contents: N₂ gas Pressure: 16.2 atm If the cylinder is opened and the gas allowed to escape into a large empty plastic bag, what will be the final volume of nitrogen gas, including what's collected in the plastic bag and what's left over in the cylinder? Write your answer in liters. Be sure your answer has the correct number of significant digits. L x10 X S
A 3.75 L sample of gas from a chemical plant is collected and analyzed st 25 degrees celisus. It is found to contail 0.0674 g NO, 0.00459 g C2H6, 0.00275 g CO2, and 0.185 g of H2O. a. What are the partical pressures in atmospheres of each component of gas? b. What is the total pressure in mmHg of the sample? c. What is the mole fraction of each gas?
The four most common gases in the atmosphere are N2, O2, Ar, and CO2. The gas with the highest average molecular speed at 25oC is-- A. N₂ B. O₂ C. Ar D. CO₂ E. All have the same average rate of effusion. The gas with the lowest rate of effusion at 25oC is A. N₂ B. O₂ C. Ar D. CO₂ E. All have the same average rate of effusion. . The gas with the highest average kinetic energy at 25oC is-- A. N₂ B. O₂ C. Ar D. CO₂ E. All have the same average rate of effusion.
receive ceredit. 1. Calculate the volume of gas at 175°C if its volume is 132 mL at 24°C at a constant pressure. 2. A tank contains 725 mL of compressed air at 1350. mmHg. Calculate the volume the compressed air will occupy at a pressure of 1860. mmHg at the same temperature. 6s Aus boo in . A sample of neon gas has a volume of 365 mL at 18°C and 675 torr. Calculate 855 m Hg and 38°C.
If 6.00 L of gas at 19.7 is compressed to 2.50 L, at a constant pressure, what is the new temperature of the gas? a. – 8.21 ℃ b. – 85.3 ℃ c. 122 ℃ d. – 151 ℃ e. 39.7 ℃ f. None of these g. 8.21 ℃
A 2.00 L container at 22.00C contains a mixture of 1.00 g H2 (g) and 1.00 g H2(g) and 1.00 g He(g). a. What is the partial pressure of H2 and He? What is the total pressure? b. What is the mole fraction of H2 and He?
If 6.00 L Cl2 gas at 20.0℃ and 1 atm, is allowed to react with excess phosphorous forming PCl3, also at 20.0℃ and 1 atm, what is the volume of PCl3 formed? (Write the balanced equation first!) a. 1.00 L b. 8.21 L c. 4.37 L d. None of these e. 6.00 L f. 4.00 L g. 122 L
Consider the following balanced chemical reaction: 2H₂ + O₂ → 2H₂O How many liters of oxygen gas (0₂) are needed to produce 43.2 liters of water at STP? A. 0.51 liters 0₂ B. 10.5 liters 0₂ C. 21.6 liters 0₂ D. 86.4 liters 0₂
3. A sample of 3.8 moles of a single gas is placed in a 5.500 L tube at 85.0 °C. The density of the gas is 2.76 g/L. What is the pressure of the gas in the tube? a. b. What is the molar mass of the gas in the tube?
A fire extinguisher with a volume of 3.0 liters is filled with 150.0 grams of CO2.a. Assuming that it is an ideal gas, what is the pressure at 20.0 °C?b. What is the volume of the CO2 at 1.0 atm and 25 °C after the CO2 is released from the fire extinguisher?
1 A gas has an initial pressure of 2.50atm and volume of 3.50L at a temperature of 27.2°C. What is the temperature when the pressure equals 4.00atm and the volume is 2.25L? P.V₁ T₁ K=C+273 P₂V₂ T₂ 35.8C 022.3°C O 15.2°C Ⓒ59.2°C ola Ar Submit Assignme