I have this sheet to do but I think its really hard! I've tried most of the questions but I need someone to tell me if what I've done is right or wrong and what is wrong if it is wrong because I'm not sure on a lot of it! 1. A cylinder contains 2.3 x 10^4 cm3 of an ideal gas at a pressure of 1.8 x 10^7 Pa and a temperature of 27C. Calculate the amount, in mol, of gas in the cylinder The main thing here I'm not too sure about is the conversion of the volume into m3. Will it be 2.3 x 10^-2m3? Because this gave me an end answer of 166 moles which seems like quite a lot.. 2. Some neon-20 gas, assumed to be ideal, has a volume of 160 cm3 at a pressure of 1.2 x 10^5Pa and a temperature of 23C. Calculate: a) the amount of substance in mol again not really too sure about converting to m3 but this is what ive done: 160 cm3 = 160 x 10^-6m3 pV = nRT 1.2 x 10^5 x 1.6 x 10^-4 = n x 8.31 x 296 n = 7.81 x 10^-3 b) the number of atoms of neon present Ermm don't know if what is right but I multiplied my answer from a) by Avogadros constant (6.02 x 10^23) to get 4.7 x 10^21. c) the mass of a neon atom I used this moles formula here moles = mass Mr mass = 7.81 x 10^-3 x 10 = 7.81 x 10^-2 d) the rms speed of the atoms Well I guess this depends on whether my previous answers are correct but this is what I did! pV = 1/3Nm(mean square speed) 1.2 x 10^5 x 160 x 10^-6 = 1/3 x 7.81 x 10^-2 x (mean square speed) mean square speed = 73.8 root mean square speed = 8.59 m/s 3. Last question now! Calculate the factor by which the rms speed of the molecules of an ideal gas will change when temperature of the gas changes from 20C to 120C. I'm just pretty much stuck with this question! Thanks very much for any help!!