# Gas Problem Set 3

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Gas Problem Set 3
A sealed balloon is filled with 1.00 L of helium at 23oC and 1.00 atm. The balloon rises to a point in the
atmosphere where the pressure is 220 torr and the temperature is -31oC. What is the new volume of the
balloon? (2.82 L)
If 60.0 mL of oxygen are collected over water at 21oC and 0.833 atm, what will be the pressure of dry
oxygen at 0oC in a 180.0 mL container? (0.250 atm)
A synthetic atmosphere is created by blending 2% CO2, 20% O2 and 78% N2.
a)If the total pressure is 750 torr, calculate the partial pressure of each gas. (15torr,150torr,585torr)
b) If 25 liters of this atmosphere, at 37oC, have to be produced, how many moles of O2 are needed?
(0.193 mol)
What volume of carbon dioxide will be produced if 146 grams of hydrogen chloride are mixed with
excess sodium carbonate at 25 C and 100 KPa? Assume the gas is collected over water. (51.2 liters)
a. Write a balanced equation
b. Convert grams of HCl to moles
c. Determine moles of gas produced
d. You will need to use the ideal gas law to calculate volume, so you will need to adjust the lab
pressure by subtracting water vapor.
e. Use the ideal gas law to calculate the volume of gas produced.
If you want to create 650 liters of dry hydrogen at 25 C and 750 mm Hg, what mass of Al would you
need to react with excess HCl? (472 g Al)
a. Write a balanced equation
b. Convert liters of hydrogen to moles. You will need to use the ideal gas equation.
c. Determine moles of Al needed
d. Convert moles of Al to grams.
Gas Problem Set 3
1. A sealed balloon is filled with 1.00 L of helium at 23oC and 1.00 atm. The balloon rises to a point in the
atmosphere where the pressure is 220 torr and the temperature is -31oC. What is the new volume of the
balloon? (2.82 L)
2. If 60.0 mL of oxygen are collected over water at 21oC and 0.833 atm, what will be the pressure of dry
oxygen at 0oC in a 180.0 mL container? (0.250 atm)
3. A synthetic atmosphere is created by blending 2% CO2, 20% O2 and 78% N2.
a)If the total pressure is 750 torr, calculate the partial pressure of each gas. (15torr,150torr,585torr)
b) If 25 liters of this atmosphere, at 37oC, have to be produced, how many moles of O2 are needed?
(0.193 mol)
4. What volume of carbon dioxide will be produced if 146 grams of hydrogen chloride are mixed with
excess sodium carbonate at 25 C and 100 KPa? Assume the gas is collected over water. (51.2 liters)
a. Write a balanced equation
b. Convert grams of HCl to moles
c. Determine moles of gas produced
d. You will need to use the ideal gas law to calculate volume, so you will need to adjust the lab
pressure by subtracting water vapor.
e. Use the ideal gas law to calculate the volume of gas produced.
5. If you want to create 650 liters of dry hydrogen at 25 C and 750 mm Hg, what mass of Al would you
need to react with excess HCl? (472 g Al)
a. Write a balanced equation
b. Convert liters of hydrogen to moles. You will need to use the ideal gas equation.
c. Determine moles of Al needed
d. Convert moles of Al to grams.
Water Vapor Pressure Table
T
P
T
P
(°C) (mmHg) (°C) (mmHg)
0.0
5.0
10.0
12.5
15.0
15.5
16.0
16.5
17.0
17.5
18.0
18.5
19.9
4.6
6.5
9.2
10.9
12.8
13.2
13.6
14.1
14.5
15.0
15.5
16.0
16.5
19.5
20.0
20.5
21.0
21.5
22.0
22.5
23.0
23.5
24.0
24.5
25.0
26.0
17.0
17.5
18.1
18.6
19.2
19.8
20.4
21.1
21.7
22.4
23.1
23.8
25.2
Water Vapor Pressure Table
T
P
T
P
(°C) (mmHg) (°C) (mmHg)
0.0
5.0
10.0
12.5
15.0
15.5
16.0
16.5
17.0
17.5
18.0
18.5
19.9
4.6
6.5
9.2
10.9
12.8
13.2
13.6
14.1
14.5
15.0
15.5
16.0
16.5
19.5
20.0
20.5
21.0
21.5
22.0
22.5
23.0
23.5
24.0
24.5
25.0
26.0
17.0
17.5
18.1
18.6
19.2
19.8
20.4
21.1
21.7
22.4
23.1
23.8
25.2
T
P
(°C
(mmHg)
27.0 26.7
28.0 28.3
29.0
30.0
30.0
31.8
35.0
42.2
40.0
55.3
50.0
92.5
60.0 149.4
70.0 233.7
80.0 355.1
90.0 525.8
95.0 633.9
100.0 760.0
T
P
(°C
(mmHg)
27.0 26.7
28.0 28.3
29.0
30.0
30.0
31.8
35.0
42.2
40.0
55.3
50.0
92.5
60.0 149.4
70.0 233.7
80.0 355.1
90.0 525.8
95.0 633.9
100.0 760.0
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