A car tire is inflated to a pressure of 2.00 atm at a temperature of 300 K. If the temperature increases to 360 K and the volume of the tire remains constant, what is the new pressure of the tire? (Assume the amount of gas does not change.)

Using the Ideal Gas Law, calculate the final temperature when 2.00 L of an ideal gas at 20.0°C is compressed to 1.00 L, assuming constant pressure.

What is the pressure exerted by a 75.0 g sample of N2O confined to a 4.12 L vessel at 298 K, assuming ideal gas behavior? (Molar mass of N2O = 44.01 g/mol, R = 0.0821 L·atm/mol·K)

Using the Ideal Gas Law, what is the pressure exerted by a 75.0 g sample of dinitrogen monoxide (N2O) gas in a 4.21 L vessel at 298 K?

A car tire is initially inflated to a pressure of 2.0 atm at a temperature of 300 K. After driving, the temperature inside the tire increases to 360 K, while the volume and amount of gas remain constant. According to the ideal gas law, what is the new pressure of the tire?

Which of the following factors directly affect the behavior of the gas inside a hot air balloon according to the ideal gas law?

Four containers each hold 1.0 mol of an ideal gas at different conditions. Which container has the gas stored at the highest temperature?A) 2.0 L at 1.0 atmB) 4.0 L at 1.0 atmC) 2.0 L at 2.0 atmD) 1.0 L at 1.0 atm

Under which conditions of pressure and temperature does a real gas behave most like an ideal gas?

At which of the following conditions will a sample of neon gas behave most like an ideal gas?