1-A helium weather balloon was filled at -20.°C and a certain pressure to a volu
ID: 1036399 • Letter: 1
Question
1-A helium weather balloon was filled at -20.°C and a certain pressure to a volume of 2.5 × 10^4L with 1.2 × 10^3 mol He.What is the molar volume of helium under those conditions?
2-A large natural gas storage tank contains 200. mol CH4 (g) at 1.20atm. An additional 100. mol CH4(g) is pumped into the tank atconstant temperature .What is the final pressure in the tank?
3-Calculate the volume occupied by 2.0 g of helium at 25°C and 1.0 atm.
4-Calculating atmospheric pressure from the height of a column of mercury.Suppose the height of the column of mercury in a barometer is 760. mm (written 760. mmHg, and read "760 millimeters of mercury") at 15°C. What is the atmospheric pressure in pascals? At 15°C the density of mercury is 13.595 g·cm-3 (corresponding to 13,595 kg·m-3) and the standard acceleration of free fall at the surface of the Earth is 9.80665 m·s^-2
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Explanation / Answer
1)
Molar volume is volume of 1 mol
use:
molar volume = total volume / total number of mol
= (2.5*10^4 L) / (1.2*10^3 mol)
= 21 L/mol
Answer: 21 L/mol
2)
Given:
Pi = 1.20 atm
ni = 200 mol
nf = 300 mol
use:
Pi/ni = Pf/Tnf
1.20 atm / 200 mol = Pf / 300 mol
Pf = 1.8 atm
Answer: 1.80 atm
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