Question

Volume pressure= .785 liters

Unknown 1 = 1884 torr
Unknown 2 = 847 torr
Now that the volume of the pressure vessel is known, the number of moles H2 gas formed can be determined for the unknown samples. Enter the corrected gas pressure after subtracting the water vapor pressure for unknowns 1 and 2
Unknown 1 corrected pressure?
Unknown 2 corrected pressure?
Use the ideal gas equation and the volume obtained above to calculate the number of moles H2 gas produced during each unknown run. Assume again that the gas temperature at the end of each run is 22 degrees C
Unknown 1?
Unknown 2?
Divide the sample mass by the number of moles of H2, calculated above to determine the ratio of sample mass to number of moles of H2, produced.

Answer 1

corrected pressure : unknown 1 = 2.452 Atm, unknown 2 = 1.088 atm

number of moles : unknown 1 = 0.079 moles unknown 2 = 0.035263 moles

Step-by-step explanation:

Given data:

volume pressure = 0.785 liters

Unknown 1 = 1884 torr (1884 mmhg )

Unknown 2 = 847 torr ( 847 mmhg )

vapor pressure at 22⁰c = 19.8 mmhg

Determine the number of moles of H2 gas for the unknowns

unknown corrected pressure for unknown 1 = total pressure - vapor pressure = 1884 - 19.8 = 1864.2 mmhg / 760 = 2.452 Atm

no of moles = PV / RT

T = 22 + 273.15 = 295.15 k

P = 2.452 atm

R = 0.08206L.atm/mole.K

v = 0.785

number of moles = (2.452 * 0.785 ) / (0.08206 * 295.15 ) = 0.079 moles of

Unknown corrected pressure for unknown 2 = total pressure - vapor pressure = (847 - 19.8 ) / 760 = 1.088 atm

number of moles = PV / RT

T = 22 + 273.15 = 295.15 k

R = 0.08206L.atm/mole.K

v = 0.785

P = 1.088 atm

number of moles = (1.088 * 0.785 ) / (0.08206 * 295.15 ) = 0.035263 moles

B ) determine the ratio of sample mass to number of moles

molar mass of H2 = 2.01588 g/mole

for unknown 1 = 2.01588 / 0.079 = 25.51

for unknown 2 = 2.01588 / 0.035263 = 57.167