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HELP! Volume at STP question, must be done ASAP! PLEASE?
An experiment is conducted in which 0.000535 mol of H2(g) is chemically generated in a closed headspace of volume 119.9 cm3 at 24.0 °C, thereby raising the total pressure by 0.109 atm.
What would be the corresponding volume of that same amount of H2(g) if it were isolated under STP conditions (exactly 0 °C and 1 atm)?
Use this to calculate the molar volume of the gas at STP.
- 9 years agoFavorite Answer
PV=nRT, where P is pressure in atm, V is volume in L, n is the number of moles, R is a constant and T is the temperature in kelvin. Based on the data in the problem, we can determine all but V.
P = 1 atm
n = 0.000535 mol
R = 0.0821 L * atm / (mol * K)
T = 273 K
Solve for V in the equation --> V = (nRT) / P
Plug in the values --> V = [(0.000535 mol)(0.0821 L*atm/(mol*k))(273 K)] / (1 atm) = .01199 L
Convert L to mL and to cm3 --> 0.01199 L * (1000 mL / L) * (1 cm3 / mL) = 11.99 cm3
Molar volume as STP is just the liters per mol under standard conditions. So to calculate, just divide the volume in liters by the number of moles.
M.V. = V / n = (.01199 L / .000535 mol) = 22.4 L
Which is the volume one mole of any gas occupies under standard conditions.