You'll check the temp at 3000 meters altitude. make sure the balloon doesnt burst before it reaches that height. The balloon is guaranteed up to 60.0 liters in size will the balloon make it to the the height and not burst? The temp at ground level is 20C. The pressure is 755 mm hg. The volume when released is 44.8 liters It's filled with helium. For both calculations use PV =nRT show all work 1. What amount in grams of helium is in the balloon? remember n = moles. 2. Can the balloon ascend to 3000 meters and not burst? the Temp, pressure at 3000 meters are Temp = -4 C, Pressure = .686 atm

Question

You'll check the temp at 3000 meters altitude. make sure the balloon doesnt burst before it reaches that height. The balloon is guaranteed up to 60.0 liters in size will the balloon make it to the the height and not burst? The temp at ground level is 20C. The pressure is 755 mm hg. The volume when released is 44.8 liters It's filled with helium. For both calculations use PV =nRT show all work 1. What amount in grams of helium is in the balloon? remember n = moles. 2. Can the balloon ascend  to 3000 meters and not burst? the Temp, pressure at 3000 meters are Temp = -4 C, Pressure = .686 atm

anonymous · Answer

It's a simple plug and chug. First figure out the moles of helium. The only help i'll give is R is equal to $$62.4\  mm\ Hg\ L \over mol\ K$$ and solving for n is $$PV= nRT$$$$n={PV\over RT}$$ then the second part would be solving for the volume. Since it's limited to 60.0L if we find it exceeds that then we can assume it will burst. We use the amount of moles found and then all the values at the height of three thousand meters. $$V={nRT\over P}$$ let me know if it works out!