Explain in terms of kinetic theory, each of the following:

1. Temperature and volume are directly proportional for a given sample of gas at constant pressure.
2. Pressure and volume are inversely proportional for a given sample of gas at constant temperature.
3. As the number of moles of gas increased, at constant temperature, the volume must be increased in order to keep the pressure constant.
4. The number of moles of gas present in a sample is directly proportional to the pressure at constant volume and temperature.
5. Number of moles and temperature are inversely proportional at constant pressure and volume.

A sample of nitrogen gas in a 1.94-L container exerts a pressure of 1.54 atm at 21 ∘C.What is the pressure if the volume of the container is maintained constant and the temperature is raised to 344 C?

The volume of the container is held constant. Pressure is directly proportional with temperature. Use the pressure-temperature law.

P1 / T1 = P2 / T2

P1 = 1.54 atm
T1 = 21°C (301K)
T2 = 344°C (605K)

Asked: P2 (what is the final pressure when the temperature is increased? Expect a higher final pressure).

*** convert Celsius temperatures to Kelvin by adding 273.

Derive the formula for P2.

P2 = P1T2 / T1
= (1.54)(605) / 344
= 2.708 atm (this is the worng answer) Please help

Sketch four graphs and show the correlation among these gas properties that are listed in below.

Part I Pressure, P, and volume, V (temperature and number of molecules constant).

Part II Pressure, P, and absolute temperature, T (volume and number of molecules constant).

Part III Volume, V, and absolute temperature, T (pressure and number of molecules constant).

Part IV Pressure, P, and number of molecules, n (volume and absolute temperature constant).