1. The problem statement, all variables and given/known data You place 83 moles of hydrogen gas in a balloon of volume 2.8 m3, and find the pressure to be 1.4 times atmospheric pressure. What is the typical speed of a hydrogen molecule? 2. Relevant equations v=(sqrt)((3*Boltzmann Constant*T)/mhydrogen T=pv/nr 3. The attempt at a solution I plugged in the values I had: v=(sqrt)((3*(1.3806503*10^-23)*575*2.8)/1.67372354 × 10-27) This doesn't work, though. What's wrong in this procedure?