Exam 10: Gases

At what temperature would the root mean square speed of oxygen molecules,O₂,be $14.0 \mathrm {~m} / \mathrm { s }$ if oxygen behaves like an ideal gas? The mass of one O₂ molecule is 5.312 × 10^-26 kg,and the Boltzmann constant is 1.38 × 10^-23 J/K.

If an ideal gas molecule has a speed of 0.50 km/s at 20°C,what is its speed at 80°C?

Express a body temperature 98.6°F in Celsius degrees.

Originally 2.00 mol of gas are at standard temperature and pressure If the temperature changes to 47.0°C and the pressure decreases to half of what it was,how many liters do the two moles now occupy? (1 atm = 101 kPa,R = 8.31 J/mol ∙ K)

How many moles are there in 2.00 kg of copper? The atomic mass of copper is 63.5 g/mol and its density is 8.90 g/cm³.

If the temperature of an ideal gas is increased from 20°C to 40°C,by what percent does the speed of the molecules increase?

The temperature in your classroom is closest to

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?

A plastic block of dimensions 2.00 cm × 3.00 cm × 4.00 cm has a mass of 30.0 g.What is its density?

A flask contains a mixture of argon and neon gases at a stabilized temperature.The root-mean-square speed of the argon gas is determined to be 1.21 km/s.What is the root-mean-square speed of the neon gas? The atomic mass of argon is 39.95 g/mol,and that of neon is 20.18 g/mol.

A 4.2-L flask of ideal neon gas (which is monatomic)is at a pressure of 3.3 atm and a temperature of 450 K.The atomic mass of neon is 20.2 g/mol.How many neon atoms are in the flask? (R = 8.31 J/mol ∙ K,1 atm = 101 kPa,N_A = 6.022 × 10²³ molecules/mol)

A 5.3 L flask of ideal neon gas (which is monatomic)is at a pressure of 6.0 atm and a temperature of $290 \mathrm {~K} .$ The atomic mass of neon is 20.2 g/mol.What is the mass of the neon gas in the flask.(R = 8.31 J/mol ∙ K,1 atm = 101 kPa,N_A = 6.022 × 10²³ molecules/mol)

The absolute temperature of a gas is T.In order to double the rms speed of its molecules,what should be the new absolute temperature?

Calculate the pressure exerted on the ground due to $\text { a } 79 - \mathrm { kg }$ person standing on one foot if the bottom of the person's foot is $13 \mathrm {~cm}$ wide and $28 \mathrm {~cm}$ long.

At what,if any,temperature are the numerical readings on the Fahrenheit and Celsius scales the same?

A 0.40- $m ^ { 3 }$ gas tank holds 7.0 moles of ideal diatomic nitrogen gas at a temperature of $290 \mathrm {~K} .$ The atomic mass of nitrogen is $14.0 \mathrm {~g} / \mathrm { mol }$ What is the pressure of the gas? (R = 8.31 J/mol ∙ K,1 atm = 101 kPa)

A 900-N person is standing on snowshoes.Each snowshoe has area 2500 cm² and has negligible weight.What pressure does this person's exert on the snow due to his interaction with Earth?

A vertical cylinder,closed at the bottom end,contains 0.0100 mol of ideal gas.It is fitted at the top with a piston that can move freely.The mass of the piston is 14.0 kg and the initial height of the piston above the bottom of the cylinder is 25 cm.What is the temperature of the gas? (R = 8.31 J/mol ∙ K)

(a)At what Celsius temperature is the average kinetic energy of a helium gas atom equal to 6.21 × 10^-21 J? The Boltzmann constant is 1.38 × 10^-23 J/K . (b)What would be the temperature for radon gas?

A sample of an ideal gas is heated and its Kelvin temperature doubles.If the root-mean-square speed of its molecules was originally v,what is the new root-mean-square speed?