Three moles of oxygen gas (O 2 ) are placed in a container with a volume of 0.00

Question

Three moles of oxygen gas (O2) are placed in a container with a volume of 0.0035 m3. If the temperature of the gas is 295oC. A) Find the pressure of the gas and the average kinetic energy of a molecule of the oxygen. B) Suppose the volume of the gas is doubled while the temperature and the number of moles are held constant, find the new pressure and average kinetic energy of a molecule. Three moles of oxygen gas (O2) are placed in a container with a volume of 0.0035 m3. If the temperature of the gas is 295oC. A) Find the pressure of the gas and the average kinetic energy of a molecule of the oxygen. B) Suppose the volume of the gas is doubled while the temperature and the number of moles are held constant, find the new pressure and average kinetic energy of a molecule.

Explanation / Answer

Number of moles of the oxygen gas   n = 3 volume of the gas is V = 0.0035 m^3 Temperature of the gas is T = 295 C                                            = 568 K a ) Pressure of the gas PV = n R T                                  P = 3 * 8.31 J /mol .K * 568 K / 0.0035 m^3                                      = 40.4 *10^5 pa Average kinetic Energy   U = 3/ 2 n RT                                           = 3 /2 * 3* 8.31 * 568                                           = 2.12*10^4 J b ) If the volume of the gas is doubled                                           P = 3 * 8.31 J /mol .K * 568 K /2* 0.0035 m^3                                      = 20.2 *10^5 pa Kinetic energy will remains same                                  P = 3 * 8.31 J /mol .K * 568 K /2* 0.0035 m^3                                      = 20.2 *10^5 pa Kinetic energy will remains same

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