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How many moles of hydrogen are present in a 26.3 mL sample at 19 degrees celsius and 744 torr? (assume hydrogen is dry).
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This is an Ideal Gas problem.
PV=nRT
P = pressure, 744 torr (1atm/ 760 torr)= 0.978 atm
V = volume, 28.3mL (1L/1000mL)= 0.0283L
n = moles of gas,
T = temperature, 25 deg celcius or 273 +25= 298K
R = 0.0821 (L*atm/K*mol) (constant)
We are solving for n so:
n= PV/RT
n= (0.978atm)(0.0263L)/
(0.0821 L*atm/K*mol) (298K)
n= 0.0011
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