Hi, the question, I'm having problems with is this: A 1.0 mol sample of hydrogen gas has a temperature of 30 C. What is the total kinetic energy of all the gas molecules in the sample? How fast would a 75 kg person have to run to have the same kinetic energy? Relevant equations: K = (3/2)kT or K = (3/2)nRT Ok, so I tried using both formulas: (3/2)(1.38*10^-23)(30+273) = 6.2721 * 10^-21 Then, since its one mole and the question asks for the total KE, I multiplied this answer by Avogadro's number (6.02*10^23) and got = 3775.8042 Joules. For the second part, I would just set this number equal to 0.5mv^2 and solve for v but since I got the first one wrong, it doesn't quite work :( I really need help; I thought I had the right idea but it's not working out. Thanks
Your method is right. Using [itex]U = \frac{3}{2}nRT[/itex], U = 1.5*8.314*303 = 3778.7 Joules. Think of one mole or 1 gram of hydrogen possessing 3778.7 J of kinetic energy. The effective average (rms) velocity is: [tex]v = \sqrt{2E/m}[/tex] AM
I thought my method was right but my homework web-assign isn't accepting that answer :( It asked for it in 2 sig figs so i put it in as 3.8 *10^3 but it still said no...