A jar holds 2.78 L of ideal nitrogen gas (N2, which is a diatomic gas) at...

 

    

Transcribed Image Text:

A jar holds 2.78 L of ideal nitrogen gas (N2, which is a diatomic gas) at -0.86 C and at pressure 2.92 atm. The atomic mass of nitrogen is 14.0 g/mol. The ideal gas constant is 8.31 J/mol.k, Avogadro's Number is NA = 6.022x1023 molecules/mol, and 1.00 atm = 101.3 kPa. How many moles of gas are contained in the jar? A student wakes up late on a cool spring morning and realizes they are late for Physics class. They run to their car, start it, and begin driving to school immediately. Before the car is driven, the (absolute) tire pressure is 547.7 kPa and the air temperature is 284.1 K. As the car is driven down the road, the tires heat up and by the time the student reaches the parking lot, the temperature of the air inside the tires is 297.8 K. Assuming that the volume of the tires does not change, what is the pressure in the tires when the student reaches the parking lot? Give your answer in kPa. On a cool spring morning (T = 5.74 oC), a mechanic inflates a customer's tires to the manufacturer's recommended pressure of 32.9 PSI. That afternoon, the temperature unexpectedly soars to 22 oC. Assuming there is no change in the volume of the tires, determine the pressure in the tires in the afternoon. Give your answer in PSI. (1 PSI = 6894.76 Pa) A large balloon has an original volume of 1.0 m3 when it is released from the ground. When the balloon is released, the pressure of the helium inside is 0.815 atm and the temperature is 15.8 oC. What is the final volume of the balloon when it rises high in the atmosphere where the temperature is -41.6 oC and the pressure is only 0.12 atm? Give your answer in m3. A quantity of an ideal gas is stored in a rigid container of constant volume. If the gas is originally at a temperature of 16.3 oC, at what temperature will the pressure of the gas double from its original value? Give your answer in degrees C. A jar holds 2.78 L of ideal nitrogen gas (N2, which is a diatomic gas) at -0.86 C and at pressure 2.92 atm. The atomic mass of nitrogen is 14.0 g/mol. The ideal gas constant is 8.31 J/mol.k, Avogadro's Number is NA = 6.022x1023 molecules/mol, and 1.00 atm = 101.3 kPa. How many moles of gas are contained in the jar? A student wakes up late on a cool spring morning and realizes they are late for Physics class. They run to their car, start it, and begin driving to school immediately. Before the car is driven, the (absolute) tire pressure is 547.7 kPa and the air temperature is 284.1 K. As the car is driven down the road, the tires heat up and by the time the student reaches the parking lot, the temperature of the air inside the tires is 297.8 K. Assuming that the volume of the tires does not change, what is the pressure in the tires when the student reaches the parking lot? Give your answer in kPa. On a cool spring morning (T = 5.74 oC), a mechanic inflates a customer's tires to the manufacturer's recommended pressure of 32.9 PSI. That afternoon, the temperature unexpectedly soars to 22 oC. Assuming there is no change in the volume of the tires, determine the pressure in the tires in the afternoon. Give your answer in PSI. (1 PSI = 6894.76 Pa) A large balloon has an original volume of 1.0 m3 when it is released from the ground. When the balloon is released, the pressure of the helium inside is 0.815 atm and the temperature is 15.8 oC. What is the final volume of the balloon when it rises high in the atmosphere where the temperature is -41.6 oC and the pressure is only 0.12 atm? Give your answer in m3. A quantity of an ideal gas is stored in a rigid container of constant volume. If the gas is originally at a temperature of 16.3 oC, at what temperature will the pressure of the gas double from its original value? Give your answer in degrees C.

Answer rating: 100% (QA)

To solve these problems we can use the ideal gas law which is given by the equation PV nRT where P i... View the full answer