DUMMYChapter 10 Problems 1. A helium filled party balloon has a volume of 4.50 L at sea level,...

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DUMMYChapter 10 Problems  1.  A helium filled party balloon has a volume of 4.50 L at sea level, where the atmospheric  pressure is 748 Torr.  Assuming that the temperature remains constant, what will be the  volume of the balloon when it is taken to a mountain resort at an altitude of 2500 m where  the atmospheric pressure is 557 Torr?  (What gas law does this problem use?) 2.  A sample of helium occupies 535 mL at 988 Torr and 25°C.  If the sample is transferred to a  1.05 L flask at 25 °C, what will be the gas pressure in the flask? 3.  A balloon indoors, where the temperature is 27°C, has a volume of 2.00 L.  What will its  volume be outdoors, where the temperature is -23°C?  Assume no change in the gas pressure.  (What gas law does this problem use?) 4.  A sample of hydrogen gas occupies 692 L at 602 °C.  If the pressure is held constant, what  volume will the gas occupy after cooling to 23°C? 5.  Calculate the volume occupied by 4.11 kg of methane gas, CH4 (g) at STP.  (What gas law  does this problem use?) 6.   What is the mass of propane, C3H8, in a 50.0 L container of the gas at STP? 7.  What is the pressure exerted by 0.508 mol O2 in a 15.0 L container at 303K? 8.  How many moles of nitrogen, N2, are there in a sample that occupies 35.0 L at a pressure of  3.15 atm and a temperature of 852 K? 9.  Calculate the molecular weight of a gas, of which a 0.550 g sample occupies 0.200 L at  0.968 atm and 289 K. 10.  Calculate the molecular weight of a liquid which, when vaporized at 100°C and 755 Torr  yields 185 mL of vapor with a mass of 0.523 g. 11.  Calculate the density of methane gas, CH4, in grams per liter at 25 °C and 0.978 atm. 12.  How many liters of O2(g) are consumed for every 10.0 L of CO2 (g) produced in the  combustion of liquid pentane, C5H12, if each gas is measured at STP?   C5H12 (l)  +     8 O2 (g)   →  5 CO2 (g)    +  6 H2O (l) 13.  A 1.00 L sample of dry air at 25 °C contains 0.0319 mol N2, 0.00856 mol O2, 0.000381 mol  Ar, and 0.00002 mol CO2.  Calculate the partial pressure of N2 in the mixture. 14.  What it is the total pressure exerted by a mixture of 4.05 g N2, 3.15 g H2, and 6.05 g He  when confined to a 6.10 L container at 25°C? 15.  Calculate the speed of an ozone molecule (O3) in the stratosphere, where the temperature  is 270 K. 16.  Calculate the speed of a carbon monoxide molecule (CO) at 300 K.

Jatin · Accepted Answer

1. Initial conditions:
P1= 748 torr
V1= 4.50 L
Final conditions:
P2= 557 torr
To find: V2
Applying Boyle’s law:
= 6.04 L
The volume of the balloon will be = 6.04 L
The problem uses Boyle’s law.
2. Initial conditions:
P1= 988 torr
V1= 535 mL = 0.535 L
T1= 25˚C = 298 K
Final conditions:
V2= 1.05 L
T2= 25˚C = 298 K
To find: P2
Applying the equation:
= 503.41 torr
The gas pressure in the flask will be = 503.41 torr.
3. Initial conditions:
V1= 2.0 L
T1= 27˚C = 300 K
Final conditions:
T2= -23 ˚C = 250 K
To find: V2
Applying the Charles’s law: 
= 1.67 L
The gas will occupy a volume of 1.67 L outdoors.
This problem uses Charles’s law.
4. Initial conditions:
V1= 692 L
T1= 602˚C = 875 K
Final conditions:
T2= 23 ˚C = 300 K
To find: V2
Applying the Charles’s law: 
= 237.26 L
After cooling, the gas will occupy a volume of 237.26 L.
5. At STP: 
Pressure(P)= 1 atm
Temperature(T)= 273 K
To find: Volume(V) occupied by methane gas
Universal gas constant(R)= 0.08206 L atm K-1 mol-1
Molar mass of methane= 12+4=16 g mol-1
Number of moles(n) of methane gas= 4.11×1000 g /16 g mol-1
                                                                                        = 685 moles
Applying the ideal gas equation and substituting the values:
PV= nRT 
= 15345.63 L
Volume(V) occupied by methane gas is = 15345.63 L
This problem uses the Ideal gas law.
6. At STP: 
Pressure(P)= 1 atm
Temperature(T)= 273 K
Given: Volume of container= 50.0 L
Universal gas constant(R)= 0.08206 L atm K-1 mol-1
Applying the ideal gas equation and substituting the values:
PV= nRT 
= 2.232 mol
Mass of 1 mole of propane= (12×3) + (8×1) = 44 g
Mass of 2.232 moles of propane= 2.232× 44= 98.208 g
7. Volume of the container(V)= 15.

Chapter 10 Problems 1. A helium filled party balloon has a volume of 4.50 L at sea level, where the atmospheric pressure is 748 Torr. Assuming that the temperature remains constant, what will be the...

Answer To: Chapter 10 Problems 1. A helium filled party balloon has a volume of 4.50 L at sea level, where the...

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