Exam 13: Temperature and Kinetic Theory

An ideal gas has a pressure of 2.5 atm, a volume of 1.0 L at a temperature of $30 ^ { \circ } \mathrm { C }$ How many molecules are there in this gas? $\left( R = 8.31 \mathrm {~J} / \mathrm { mol } \cdot \mathrm { K } , 1.00 \mathrm {~atm} = 101 \mathrm { kPa } , N _ { \mathrm { A } } = 6.022 \times 10 ^ { 23 } \right)$

A car starts out when the air temperature is 288 K and the absolute (total) air pressure in the tires is 500 kPa. After driving a while, the temperature of the air in the tires increases to 298 K. What is the pressure in the tires at that point, assuming their volume does not change?

What is absolute zero on the (a) Celsius scale and (b) on the Fahrenheit scale?

On a cold day, you take in 4.2 L of air into your lungs at a temperature of $0 ^ { \circ } \mathrm { C }$ If you hold your breath until the temperature of the air in your lungs reaches $37 ^ { \circ } \mathrm { C }$ what is the volume of the air in your lungs at that point, assuming the pressure does not change?

The volume coefficient of thermal expansion for gasoline is $950 \times 10 ^ { - 6 } K ^ { - 1 }$ By how many cubic centimeters does the volume of 1.00 L of gasoline change when the temperature rises from $30 ^ { \circ } \mathrm { C }$ to $50 ^ { \circ } \mathrm { C } ?$

A balloon originally has a volume of $1.0 \mathrm {~m} ^ { 3 }$ when the gas in it is at $20 ^ { \circ } \mathrm { C }$ and under a pressure of 1.0 atm. As it rises in the earth's atmosphere, its volume expands. What will be its new volume if its final temperature and pressure are $- 40 ^ { \circ } \mathrm { C }$ and 0.10 atm ?

Oxygen condenses into a liquid at approximately 90 K. What temperature, in degrees Fahrenheit, does this correspond to?