The partial pressures of each gas in the given sample containing mixture of 50 % helium and 50 % xenon by mass are needed to be determined, it the total pressure of sample is given as 600 torr . Concept introduction: Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone. Partial pressure of a gas in terms of its mole fraction and total pressure is, ` P A = χ A × P TOTAL Mole fraction of a molecule in a mixture is the ratio of number of moles of particular molecule to the sum of number of moles of all molecules in the mixture. Equation for mole fraction of a molecule in a mixture of two molecules (A and B) is, molecule fraction of A, ( χ A ) = numbers of moles of A (n A ) numbers of moles of A (n A ) + numbers of moles of B (n B ) Number of moles of a substance from its given mass is, Number of moles = Given mass Molecular mass Total pressure of a mixture of gases is the sum of individual partial pressures of constituted gases. To determine: the partial pressure of each gas in the given mixture of 50 % helium and 50 % xenon by mass.
The partial pressures of each gas in the given sample containing mixture of 50 % helium and 50 % xenon by mass are needed to be determined, it the total pressure of sample is given as 600 torr . Concept introduction: Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone. Partial pressure of a gas in terms of its mole fraction and total pressure is, ` P A = χ A × P TOTAL Mole fraction of a molecule in a mixture is the ratio of number of moles of particular molecule to the sum of number of moles of all molecules in the mixture. Equation for mole fraction of a molecule in a mixture of two molecules (A and B) is, molecule fraction of A, ( χ A ) = numbers of moles of A (n A ) numbers of moles of A (n A ) + numbers of moles of B (n B ) Number of moles of a substance from its given mass is, Number of moles = Given mass Molecular mass Total pressure of a mixture of gases is the sum of individual partial pressures of constituted gases. To determine: the partial pressure of each gas in the given mixture of 50 % helium and 50 % xenon by mass.
Solution Summary: The author explains the partial pressures of each gas in a given sample containing mixture of helium and xenon by mass are needed to be determined, and the total pressure of sample is given as
Interpretation: The partial pressures of each gas in the given sample containing mixture of
50% helium and
50% xenon by mass are needed to be determined, it the total pressure of sample is given as
600torr.
Concept introduction:
Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone.
Partial pressure of a gas in terms of its mole fraction and total pressure is,
`
PA=χA×PTOTAL
Mole fraction of a molecule in a mixture is the ratio of number of moles of particular molecule to the sum of number of moles of all molecules in the mixture.
Equation for mole fraction of a molecule in a mixture of two molecules (A and B) is,
b) Certain cyclic compounds are known to be conformationally similar to carbohydrates, although they are not
themselves carbohydrates. One example is Compound C shown below, which could be imagined as adopting
four possible conformations. In reality, however, only one of these is particularly stable. Circle the conformation
you expect to be the most stable, and provide an explanation to justify your choice. For your explanation to be
both convincing and correct, it must contain not only words, but also "cartoon" orbital drawings contrasting the
four structures.
Compound C
Possible conformations (circle one):
Дет
Lab Data
The distance entered is out of the expected range.
Check your calculations and conversion factors.
Verify your distance. Will the gas cloud be closer to the cotton ball with HCI or NH3?
Did you report your data to the correct number of significant figures?
- X
Experimental Set-up
HCI-NH3
NH3-HCI
Longer Tube
Time elapsed (min)
5 (exact)
5 (exact)
Distance between cotton balls (cm)
24.30
24.40
Distance to cloud (cm)
9.70
14.16
Distance traveled by HCI (cm)
9.70
9.80
Distance traveled by NH3 (cm)
14.60
14.50
Diffusion rate of HCI (cm/hr)
116
118
Diffusion rate of NH3 (cm/hr)
175.2
175.2
How to measure distance and calculate rate
For the titration of a divalent metal ion (M2+) with EDTA, the stoichiometry of the reaction is typically:
1:1 (one mole of EDTA per mole of metal ion)
2:1 (two moles of EDTA per mole of metal ion)
1:2 (one mole of EDTA per two moles of metal ion)
None of the above
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