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11 Dec 2019

The Pressure in the flask is atmospheric, or 760 torr, or 1 atm. The volume of the flask to begin with is 1100 mL. If the flask is equipped with a 100 mL syringe and the syringe is compressed so that the new volume is 1000 mL, what is the new pressure assuming the temperature did not change?

Given: PV=nRT; and: PV/T = PV/T

a. 836 torr

b. 0.836 atm

c. 691 torr

d. 11 atm

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Bunny Greenfelder
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13 Dec 2019

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Related questions

Experiment 3: Charles’ Law (Part 2)

Using the air in a flask, measure the change in volume with temperature.

Materials:

2-Hole Rubber stopper
250 mL Erlenmeyer flask
Thermometer
100 mL Graduated cylinder
10 mL Syringe
Syringe dispensing tip

*Microwave or stovetop
*Ice
*Water
*Water bath container

*You must provide

Procedure

Connect the syringe dispensing tip to the end of the syringe.

Set up your experiment by unscrewing the cap off the 250 mL Erlenmeyer flask. Then, press the 2-hole rubber stopper into the 250 mL Erlenmeyer flask. Push the thermometer into one of the holes in the stopper, and the syringe dispensing tip (connected to the syringe) in the remaining hole.

Create an ice water bath by filling an empty container (large enough to fit the 250 mL Erlenmeyer in it) with water and ice. The exact volumes do not matter.

Place the flask in the bath and allow the flask to cool to 0 °C (32 °F). You may need to pour additional ice around the flask to sufficiently decrease the temperature.

Monitor the temperature until the air reading in the flask is 0 °C.

Remove the flask from the ice bath and discard the ice/water from the bath container.

Allow the flask to warm to room temperature. As the flask warms up, record the volume on the syringe and the temperature on the thermometer in Table 4. The volume and temperature at room temperature are the initial (Time = 0) data. Note: The gas in the flask expands as it warms, slowly pushing the piston out of the syringe. The total volume of the gas in the system is equal to the volume of the flask plus the volume of the syringe.

Use the graduated cylinder to measure and add 100 mL of hot (but not boiling) water to the water bath container and place the flask in the warm water.

Continue to record the volume reading on the syringe and the temperature on the thermometer as the gas in the flask heats every five minutes for 30 minutes. Record your results in Table 4.

Table 4: Temperature vs. Volume Data

Syringe Volume (mL) and Temperature (°C) at Room Temperature (Step 7)

Time (minutes)

Temperature (°C)

Total Volume (mL)

0

5

10

15

20

25

Post-Lab Questions:

Graph your results as temperature vs. total volume. Draw a best-fit straight line through your data pointsand determine the formula for the line in Y = mx +b form. Don’t forget to title your graph and label your axes. You may also use a graphing software program for more accurate data plots.

According to your graph, what would the total volume be at a temperature of 70 °C? 30 °C?

How do your results demonstrate Charles’ Law? Use mathematical expressions to explain your answer.

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 vrms, 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.


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