Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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2. You have a 965 mL sample of methane at 92°C and a pressure of 1.29×10' torr.
A. How many moles of methane are in the sample?
B. If you add 1.200 moles of oxygen to the methane while keeping temperature and volume
constant, what will the mole fraction of methane and oxygen be?
C. What is the total pressure with methane and oxygen?
D. What is the partial pressure of methane and the partial pressure of oxygen?
1. A mixture of 4.0g H2(g) and 10.0g He(g) in a 5.2L flask is maintained at 0oC.
A. Calculate the total pressure in the container.B. Determine the partial pressure of each gas.C. Calculate the mole fraction of H2(g).
- Consider a mixture of 15.08 g O,, 8.17 g of N2, and 2.64 g of H2.
a. Calculate the mole fraction of each gas in the mixture.
b. Calculate the total number of moles of gas in the mixture.
c. If the mixture is contained in a 15.50L vessel at 15 °C, calculate the total pressure of the
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mixture.
d. Calculate the partial pressure of each gas in the mixture.
Chapter 10 Solutions
Chemistry: An Atoms-Focused Approach
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Similar questions
- If equal masses of O2 and N2 are placed in separate containers of equal volume at the same temperature, which of the following statements is true? If false, explain why it is false. (a) The pressure in the flask containing N2 is greater than that in the flask containing O2. (b) There are more molecules in the flask containing O2 than in the flask containing N2.arrow_forwardAnswer the following questions: (a) If XX behaved as an ideal gas, what would its graph of Z vs. P look like? (b) For most of this chapter, we performed calculations treating gases as ideal. Was this justified? (c) What is the effect of the volume of gas molecules on Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (d) What is the effect of intermolecular attractions on the value of Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (e) In general, under what temperature conditions would you expect Z to have the largest deviations from the Z for an ideal gas?arrow_forwardThe density of air at 20C and 1.00 atm is 1.205 g/L. If this air were compressed at the same temperature to equal the pressure at 50.0 m below sea level, what would be its density? Assume the barometric pressure is constant at 1.00 atm. The density of seawater is 1.025 g/cm3.arrow_forward
- How would the use of a volatile liquid affect the measurement of a gas using open-ended manometers vs. closed-end manometers?arrow_forwardA 1-L sample of CO initially at STP is heated to 546 K. and its volume is increased to 2 L. (a) What effect do these changes have on the number of collisions of the molecules of the gas per unit area of the container wall? (b) What is the effect on the average kinetic energy of the molecules? (c) What is the effect on the root mean square speed of the molecules?arrow_forwardYou have two pressure-proof steel cylinders of equal volume, one containing 1.0 kg of CO and the other containing 1.0 kg of acetylene, C2H2. (a) In which cylinder is the pressure greater at 25 C? (b) Which cylinder contains the greater number of molecules?arrow_forward
- 13. Consider two containers of volume 1.0 L at 298 K, as shown below. One container holds 0.10 mol N2 and the other holds 0.10 mol H2. The average kinetic energy of the nitrogen molecules is 6.2 X 10 -21 J. Assume that the N2 and the H2 exhibit ideal behavior. a. Is the pressure in the container holding the H2 less than, greater than, or equal to the pressure in the container holding the N2. Justify your answer. b. What is the average kinetic energy of the H2 molecules? c. The molecules of which gas, N2 or H2, have the greater average speed? Justify your answer. d. What change could be made that would decrease the average kinetic energy of the molecules in the container?arrow_forwardHydrogen peroxide (H2O2) decomposes in the presence of a catalyst to form water and oxygen. The catalyst is added to 5.00 mL of a hydrogen peroxide solution at 25.0 °C, and 49.5 mL of gas is collected over water at a total pressure of 763.8 mmHg.a. Write and balance the chemical reaction. (Note: catalysts do not appear in balanced chemical equations.)b. Look up the vapor pressure of water under these conditions.c. What is the partial pressure of oxygen collected over the water?d. How many moles of oxygen are collected? e. How many grams of hydrogen peroxide were in the original sample?f. What is the concentration (in mol>L) of the hydrogen peroxide solution?g. Which part of this process is conceptually most difficult for your group?arrow_forward
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