Question

Consider the following gases in separate flasks of equal volume at STP CO2 So На Determine which of the following statements are true. If the statement is false, change the statement to make the statement true. 1. The average kinetic energy of H2 is higher than CO2. 2. The root mean square (ms) speed of H2 is lower than CO2) 3. H2, CO2 and So3 will all have the same kinetic energy. 4. If these gases behave ideally, 1 mol of these gases will have a volume of 22.4 L and contain an equal number of molecules. 5. If these gases behave ideally, 1 mole of these gases will have the same density

Answer 1

Average kinetic energy depends upon absolute temperature.

statements :- 1. false => comect The average kinetic energy of gas molecules is directly proportional to the absolute temperature Keo I does not depend upon molecular mans of gas" is 2. false => correct. The root mean square (rms) speed af H₂ more than CO2" Voms = 3RT My = 2 gm Mcos = 44gm My <mcor in fase Vomste > Vomit. Voms com have - True the Ho CO2 and 503 will all same kinetic energy" 4. True so false correct => If there gases behave ideally, = 1 more of these gases will have - the different density da PM dam] } 92= 2gm, Mcoz= 44gm dlase Miase M 50 = 80gm dsoz> acopo due