9.30 Perform the following pressure conversions.
(a) 1.15 atm to torr
(b)
968 torr to atm
(c)
2.50 × 105 Pa to atm
(d)
695 mm Hg to torr
(e)
0.953 atm to Pa
(f)
653 torr to mm Hg
(g)
1545 mm Hg to Pa
(h)
3.73 kPa to atm
9.38 Given a fixed quantity of a gas at constant temperature, calculate the new volume the gas
would occupy if the pressure were changed as shown in the following table.
Hint:
𝑃1 𝑉1
𝑇1
=
𝑃2 𝑉2
𝑇2
Initial
Volume
Initial
Pressure
Final Pressure
Final Volume
2.50 L
2.50 atm
725 atm
?
6.25 mL
825 torr
456 torr
?
450 mL
50.0 torr
30.0 torr
?
9.41 What pressure is required to compress 925 L of N2 at 1.25 atm into a container whose volume
is 6.35 L?
9.42 What will be the final volume of 186 mL of Cl2 if the pressure increases from 0.945 atm to
1.76 atm?
9.49 For a fixed amount of gas held at constant pressure, calculate the new volume the gas would
occupy if the temperature were changed as shown in the following table.
Hint:
𝑃1 𝑉1
𝑇1
=
𝑃2 𝑉2
𝑇2
T must be in Kelvin!
Initial Volume
Initial
Temperature
Final
Temperature
Final Volume
6.00 L
30.0°C
0.0°C
?
212 mL
−60.0°C
401.0°C
?
47.5 L
212 K
337 K
?
9.50 For a fixed amount of gas held at constant pressure, calculate the new volume the gas would
occupy if the temperature were changed as shown in the following table.
Hint:
𝑃1 𝑉1
𝑇1
=
𝑃2 𝑉2
𝑇2
T must be in Kelvin!
Initial
Volume
224 L
Initial
Final
Temperatur Temperature
e 0.0°C
100.0°C
Final
Volume
?
152 mL
45 K
450 K
?
156 mL
45°C
450°C
?
9.51 For a fixed amount of gas held at constant pressure, calculate the temperature in degrees
Celsius to which the gas would have to be changed to achieve the change in volume shown in the
following table.
Hint:
𝑃1 𝑉1
𝑇1
=
𝑃2 𝑉2
𝑇2
Initial
Temperature
Initial
Volume
Final
Volume
Final
Temperature
0.0°C
70.0 mL
140.0 mL
?
−37°C
2.55 L
85 mL
?
165 K
87.5 L
135 L
?
9.64 For a gas under a given initial set of conditions, calculate the final value for the variable
indicated if the other two variables change as described in the following table.
Hint:
𝑃1 𝑉1
𝑇1
=
𝑃2 𝑉2
𝑇2
Initial volume
601 mL
237 mL
1.12 L
Initial
pressure
Initial
temperature
Final volume
900.0 torr
75.0 atm
760.0 torr
−10.0°C
147 K
0.0°C
1200.0 mL
474 mL
Final pressure
Final
temperature
?
0.0°C
150.0 atm
?
?
700.0 torr
25.0°C
9.71 Given the following volumes of gases at STP, calculate the number of moles of each gas and
the mass of the gas.
(a) 8.62 L CH4
(b) 350.0 mL Xe
(c) 48.1 L CO
9.75 Given the following amounts of gases, calculate the number of moles of each gas. Calculate
the volume each amount of gas would occupy at STP.
(a) 5.8 g NH3
(b) 48 g O2
(c) 10.8 g He
9.90 Calculate the density in grams per liter of the following gases at STP.
Hint: 𝑑 =
ℳ𝑅𝑇
𝑃
(a) NO
(b) NO2
(c) O2
9.91 Calculate the density in grams per liter of the following gases at 25.0°C and 735 torr.
Hint: 𝑑 =
(a) NH3
(b) N2
(c) N2O
ℳ𝑅𝑇
𝑃
9.98 A total of 0.400 L of hydrogen gas is collected over water at 18°C. The total pressure is 742
torr. If the vapor pressure of water at 18°C is 15.5 torr, what is the partial pressure of hydrogen?
9.99 A tank contains 78.0 g of N2 and 42.0 g of Ne at a total pressure of 3.75 atm and a
temperature of 50.0°C.
Calculate the following quantities.
(a) moles of N2
(b) moles of Ne
(c) partial pressure of N2
(d) partial pressure of Ne
9.118
When nitric acid is synthesized from ammonia, the first step in the process is
4NH3(g) + 5O2(g)  4NO(g) + 6H2O(g)
What volume of NO at STP can be formed from 1250 L of NH3 at 325°C and 4.25 atm, assuming
temperature and pressure conditions remain constant?
9.120
Nitric oxide is produced in the reaction between copper metal and nitric acid:
3Cu(s) + 8HNO3(aq) 3Cu(NO3)2(aq) + 4H2O(l) + 2NO(g)
What mass of copper is required to produce 15.0 L of NO at 725 torr and 20.0°C?