At 137°C and under a pressure of 3.11 atm, a 276 g sample of an unknown noble gas occupies 13.46L of space. What is the gas? I just need to know how to go from grams to moles if I dont know the mass in grams. Thanks
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Really ?!
WOW
I guess you either (or both) have never heard of the ideal gas law or are ilnumerate.
Here is the ideal gas law. It is called 'ideal' because most gasses are within a few % of obeying it at normal (or lower) pressures. I believe I know of one compound that has a pressure 14% lower than what the Ideal Gas Law predicts. Most are within 3 - 5%, and of course the noble gases will be very close because the errors are due to the Ideal assumption of "non-interaction" between particles being violated.
PV = nRT. R is a constant whose value depends on its units. n is the number of moles.
P is Pressure (units variable), V is Volume (units variable) and T is ABSOLUTE temperature (units either Rankin or Kelvin ie also variable)
You claim that you don't know the mass in grams. Does the quantity 276 g mean anything to you, or are you really that screwed up?
Solve the IDG for n, mass/n = MW. duh!!!
WOW
I guess you either (or both) have never heard of the ideal gas law or are ilnumerate.
Here is the ideal gas law. It is called 'ideal' because most gasses are within a few % of obeying it at normal (or lower) pressures. I believe I know of one compound that has a pressure 14% lower than what the Ideal Gas Law predicts. Most are within 3 - 5%, and of course the noble gases will be very close because the errors are due to the Ideal assumption of "non-interaction" between particles being violated.
PV = nRT. R is a constant whose value depends on its units. n is the number of moles.
P is Pressure (units variable), V is Volume (units variable) and T is ABSOLUTE temperature (units either Rankin or Kelvin ie also variable)
You claim that you don't know the mass in grams. Does the quantity 276 g mean anything to you, or are you really that screwed up?
Solve the IDG for n, mass/n = MW. duh!!!