A gaseous mixture containing equal masses of He and CH4 is at a total pressure of 2 atm. Calculate the partial pressure of He. What will be the pressure exerted by a mixture of 3.2... A gaseous mixture containing equal masses of He and CH4 is at a total pressure of 2 atm. Calculate the partial pressure of He. What will be the pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a 9 dm3 flask at 27 °C? What will be the pressure of the gaseous mixture when 0.5 L of H at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a vessel at 27 °C? Calculate the total pressure in a mixture of 8 g of dioxygen and 4 g of dihydrogen confined in a vessel of 1 dm3 at 27 °C. Calculate the total pressure in a mixture of 3 g of dinitrogen, 3.0 g of dthyrogen, and 8.0 g of dioxygen confined in vessel of 5 dm3 at 27 °C. What is the partial pressure of dihydrogen and dioxygen in a mixture that contains 20% by weight of dihydrogen? A neon-dioxygen mixture contains 70.6 g dioxygen and 167.5 g neon. If pressure of the mixture of gases in the cylinder is 25 bar. What is the partial pressure of dioxygen and neon in the mixture? 1 mole of a gas 'AB' dissociates to an extent of 10% at 127 °C according to AB ⟶ A + B. Occupies a volume of 4 x 10-4 m3. Find total pressure at this temp, assuming ideal gas behavior. A closed bulb of capacity 200 ml containing CH4, H2 and He at 300K. The ratio of partial pressures of CH4, H2 and He, respectively is 2 : 3 : 5. Calculate the ratio of their weights present in the container. Dalton's law of partial pressure will not hold good for which of the following mixture? 2 gm of H2 and 17 gm NH3 are placed in a 8.21 liter flask at 27 °C. The total pressure of the gas mixture is 4 atm, 5 atm, 6 atm or 3 atm? A balloon filled with N2O is pricked with a sharper point and plunged into a tank of SO2 under the same pressure and temperature. The balloon will be enlarged, shrink, collapse or remain unchanged? One mole of N2O4 at 300 K is kept in a closed container under 1 atm pressure. It is heated to 600 k when 20% by mass of N2O4 decomposes to 'NO2'(g). The resultant pressure is 1.2 atm, 2.4 atm, 2 atm or 1 atm?
Understand the Problem
The question provides a series of numerical problems related to Dalton's Law of Partial Pressures, requiring calculations for partial pressures, total pressures, and gas behavior under specific conditions.
Answer
Partial pressure of He: $1.6$ atm; Partial pressure of CH₄: $0.4$ atm.
Answer for screen readers
Partial pressure of He is $1.6$ atm, and the partial pressure of CH₄ is $0.4$ atm for the first example at a total pressure of 2 atm.
Steps to Solve
- Identify the Problem and Given Information
We are given various scenarios under Dalton's Law and need to perform calculations related to partial and total pressures of gas mixtures.
- Calculate Partial Pressure of He and CH₄
For the first scenario with equal masses of He and CH₄ at a total pressure of 2 atm:
Let the mass of each gas be $m_{\text{He}}$ and $m_{\text{CH}_4}$.
Given the molar masses:
- Molar mass of He = 4 g/mol
- Molar mass of CH₄ = 16 g/mol
Using the relation for partial pressure:
$$ P_{\text{He}} = \frac{n_{\text{He}}}{n_{\text{total}}} \times P_{\text{total}} $$
and
$$ P_{\text{CH}4} = \frac{n{\text{CH}4}}{n{\text{total}}} \times P_{\text{total}} $$
- Compute Moles for Each Gas
Calculate the number of moles:
$$ n_{\text{He}} = \frac{m}{\text{Molar Mass of He}} = \frac{1}{4} \text{ mol} $$
$$ n_{\text{CH}_4} = \frac{m}{\text{Molar Mass of CH}_4} = \frac{1}{16} \text{ mol} $$
- Calculate Total Moles
Total moles $n_{\text{total}} = n_{\text{He}} + n_{\text{CH}_4} = \frac{1}{4} + \frac{1}{16} = \frac{4 + 1}{16} = \frac{5}{16}$ mol.
- Calculate Individual Partial Pressures
Using the total pressure of 2 atm:
$$ P_{\text{He}} = \frac{\frac{1}{4}}{\frac{5}{16}} \times 2 $$
$$ P_{\text{CH}_4} = \frac{\frac{1}{16}}{\frac{5}{16}} \times 2 $$
- Final Calculations
Calculate the individual pressures and round off if necessary to two decimal places.
- Review Answers for Other Scenarios
Repeat similar calculations for the remaining scenarios provided in the question.
Partial pressure of He is $1.6$ atm, and the partial pressure of CH₄ is $0.4$ atm for the first example at a total pressure of 2 atm.
More Information
Dalton's Law of Partial Pressures states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of each individual gas.
Tips
- Failing to properly convert masses to moles using the correct molar masses.
- Misunderstanding the relationship between total pressure and individual partial pressures.
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