CHEM 24112 Chapter Notes - Chapter 5: Weather Balloon, Calcium Chloride, Torr

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Chem 112 Quest #5 Practice

Multiple Choice

Identify the choice that best completes the statement or answers the question.

____ 1. The air in the inner tube of the tire of a racing bike has a pressure of 116.8 psi. Convert this pressure to atm.

a. 0.154 atm c. 1717 atm

b. 7.94 atm d. 1.15 atm

____ 2. A gas occupies 18.5 L at 0oC and 760 torr. What volume will it occupy at 735 torr and 57oC?

a. 3.99 L c. 15.8 L

b. 21.6 L d. 23.1 L

____ 3. Mercury vapor contains Hg atoms. What is the volume of 200. g of mercury vapor at 822 K and 0.42 atm?

a. 162 L c. 216 L

b. 27.9 L d. 108 L

____ 4. A flexible weather balloon contains helium gas at a volume of 855 L. Initially the balloon is at sea level,

where the temperature is 25oC and the barometric pressure is 0.947 atm. The balloon then rises to an altitude

of 5500 ft, where the pressure is 0.785 atm and the temperature is 15oC. What is the new volume of the

balloon?

a. 997 L c. 1067 L

b. 618 L d. 614 L

____ 5. A sample of a gas in a ballon has a volume of 2.13 L and a temperature of 11.8oC. Calculate the volume

when the temperature is raised to 42.3oC at constant pressure.

a. 2.36 L c. 7.64 L

b. 2.13 L d. 0.59 L

____ 6. When calcium chloride is placed in water, calcium chloride is the ___ and the ions present (in the correct

ratio) are ____.

a. solvent; Ca2+ and Cl-c. solute; Ca2+ and 2Cl-

b. solute; Ca2+ and Cl-d. solvent; Ca2+ and 2Cl-

____ 7. What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.121 M H2SO4?

a. 104.2 mL c. 1.88 L

b. 140.5 mL d. 128.1 mL

____ 8. An oven cleaning solution is 40.0% (by mass) NaOH. If one jar of this product contains 457 g of solution,

how much NaOH does it contain?

a. 0 g c. 182.8 g

b. 11.43 g d. 18.3 g

____ 9. A 47.7 g sample of SrCl2 is dissolved in 112.5 mL of solution. Calculate the molarity of this solution.

a. 0.301 M c. 0.034 M

b. 2.67 M d. 3.99 M

____ 10. 15.0 mL of 0.30 M sodium phosphate solution reacts with 20.0 mL of 0.30 M lead (II) nitrate solution. How

many moles of solid lead(II) phosphate will be formed?

a. 0.0045 moles c. 0.0020 moles

b. 0.00225 moles d. 0.0060 moles

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Document Summary

Identify the choice that best completes the statement or answers the question. ___: the air in the inner tube of the tire of a racing bike has a pressure of 116. 8 psi. Convert this pressure to atm: 0. 154 atm, 7. 94 atm, 1717 atm, 1. 15 atm. ___: a gas occupies 18. 5 l at 0oc and 760 torr. What volume will it occupy at 735 torr and 57oc: 3. 99 l, 21. 6 l, 15. 8 l, 23. 1 l. What is the volume of 200. g of mercury vapor at 822 k and 0. 42 atm: 162 l, 27. 9 l, 216 l, 108 l. ___: a flexible weather balloon contains helium gas at a volume of 855 l. initially the balloon is at sea level, where the temperature is 25oc and the barometric pressure is 0. 947 atm. The balloon then rises to an altitude of 5500 ft, where the pressure is 0. 785 atm and the temperature is 15oc.

Related Questions

1- (A) A 41 L cylinder containing helium gas at a pressure of 46.7 atm is used to fill a weather balloon in order to lift equipment into the stratosphere. To what maximum pressure (in atm) could a 286 L balloon be filled.

(B) A 38.0 L cylinder containing helium gas at a pressure of 20.9 atm is used to fill a weather balloon in order to lift equipment into the stratosphere. What is the final pressure (in atm) in the cylinder after a 169 L balloon is filled to a pressure of 1.15 atm.

(C)The following procedure provides a crude method of determining the molar mass of a volatile liquid. A liquid of mass 0.0181 g is introduced into a syringe and the end is capped (sealed). The syringe is transferred to a temperature bath maintained at 59.4 ^oC, and the liquid vaporizes. As the liquid vaporizes the plunger is pushed out. At equilibrium, the plunger reads 6.61 mL of gas. Atmospheric pressure is 740. mmHg. What is the approximate molar mass of the compound (in g/mol)?

(D)The reaction of magnesium metal with HCl yields hydrogen gas and magnesium chloride. What is the volume, in liters, of the gas formed at 757 torr and 34 ^oC from 4.59 g of Mg in excess Hal?

(E)What mass of water (in grams) forms from the reaction of 2.60 L of hydrogen gas and 1.97 L of oxygen gas? Both gases are at 698 torr and 12.9 ^oC.

(F)What is the partial pressure of argon, in torr, in a container that also contains neon at 220 torr and is at a total pressure of 439 torr?

(G)What is the total pressure if a container contains 10 torr of He gas, 207 torr of N₂ gas, and 72 torr of Ar gas?

(H)Oxygen gas is collected over water. The total pressure (the O₂ pressure + the water vapor pressure) is 760 torr. The temperature of the water is such that the water vapor pressure is 49 torr. What is the partial pressure of the oxygen gas in torr?

(I)A 5.10 L sample of neon at 10.11 atm is added to a 13.0 L cylinder that contains argon. If the pressure in the cylinder is 7.92 atm after the neon is added, what was the original pressure (in atm) of argon in the cylinder?

(J)Calculate the total pressure, in atm, in a 5 L flask that contains 6.42 g of Ne and 1.55 g of Ar. The temperature of the gases is 32 ^oC.

(K)Calculate v_rms, the root mean square velocity, in m/s of SO₂ molecules at 274 ^oC.

(L)An effusion container is filled with 7 L of an unknown gas. It takes 132 s for the gas to effuse into a vacuum. From the same container under the same conditions--same temperature and initial pressure, it takes 335 s for 7.00 L of O₂ gas to effuse. Calculate the molar mass (in grams/mol) of the unknown gas.

(M)Three bulbs are connected by tubing, and the tubing is evacuated. The volume of the tubing is 28.0 mL. The first bulb has a volume of 83.0 mL and contains 5.10 atm of argon, the second bulb has a volume of 250 mL and contains 1.09 atm of neon, and the third bulb has a volume of 33.0 mL and contains 4.04 atm of hydrogen. If the stopcocks (valves) that isolate all three bulbs are opened, what is the final pressure of the whole system in atm?

(N)Use the van der Waals equation to calculate the pressure, in atm, of 45.61 mol of hydrogen at 443 ^oC in a 2.45 L container.

1. what is the temperature of .49 mol of gas at a pressure of 1.2 atm and a volume of 12.4 L?2. A weather balloon is inflated to a volume of 26.1 L at a pressure of 755 mmHg and a temperature of 23.0. C The balloon rises in the atmosphere to an altitude, where the pressure is 375 mmHg and the temperature is -16.9. C assuming that that balloon can freely expand, calculate the volume of the balloon at this altitude in L. 3. To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 5.8-L bulb, then filled it with the gas at 1.30 atm and 22.0C and weighed it again. The difference in mass was 8.7g . Identify the gas.4. A 1-L flask is filled with 1.30g of argon at 25C . A sample of ethane vapor is added to the same flask until the total pressure is 1.00 atm. What is the pressure of argon Par in the flask? What is the partial pressure of ethane, Pethane, in the flask?5. 14.0 moles of gas are in a 5.00 L tank at 23.4 C. Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are a=2.300 L2*atm/mol2 and b=0.430L/mol

A 7.97 gram piece of solid CO2 (dry ice) is allowed to sublime in a balloon. The final volume of the balloon is 1.00 L at 299 K. What is the pressure of the gas?