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In which of the following mixtures, Dalton's law of partial pressure is not applicable? (Assume room temperature)
- a)H2 and N2 mixture
- b)H2 and Cl2 mixture
- c)H2 and CO2 mixture
- d)None of these
Correct answer is option 'B'. Can you explain this answer?
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In which of the following mixtures, Daltons law of partial pressure is...
Dalton's law of partial pressure is not applicable to gases which react chemically and produce different number of moles of products than the reactants. Some gases which do not obey this law are
SO2+Cl2, CO+Cl2, NO+O2, NH3+HCl and H2+Cl2
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In which of the following mixtures, Daltons law of partial pressure is...
Explanation:
Dalton's law of partial pressure states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. This law is applicable to ideal gases under certain conditions. However, in some cases, the law may not be applicable due to the non-ideal behavior of gases.
The correct answer is option B, i.e. H2 and Cl2 mixture. This is because H2 and Cl2 are highly reactive gases that can combine to form a product (HCl) under normal conditions. Therefore, it is not possible to separate these gases and measure their individual pressures in a mixture.
In contrast, H2 and N2 are both inert gases that do not react with each other, and therefore, Dalton's law is applicable to their mixture. Similarly, H2 and CO2 are also non-reactive gases and their mixture can be treated as an ideal gas mixture.
In summary, Dalton's law of partial pressure is applicable to ideal gas mixtures under certain conditions. However, in the case of highly reactive gases such as H2 and Cl2, the law may not be applicable due to their tendency to react and form products.
Dalton's law of partial pressure states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. This law is applicable to ideal gases under certain conditions. However, in some cases, the law may not be applicable due to the non-ideal behavior of gases.
The correct answer is option B, i.e. H2 and Cl2 mixture. This is because H2 and Cl2 are highly reactive gases that can combine to form a product (HCl) under normal conditions. Therefore, it is not possible to separate these gases and measure their individual pressures in a mixture.
In contrast, H2 and N2 are both inert gases that do not react with each other, and therefore, Dalton's law is applicable to their mixture. Similarly, H2 and CO2 are also non-reactive gases and their mixture can be treated as an ideal gas mixture.
In summary, Dalton's law of partial pressure is applicable to ideal gas mixtures under certain conditions. However, in the case of highly reactive gases such as H2 and Cl2, the law may not be applicable due to their tendency to react and form products.
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In which of the following mixtures, Daltons law of partial pressure is not applicable? (Assume room temperature)a)H2 and N2 mixtureb)H2 and Cl2 mixturec)H2and CO2 mixtured)None of theseCorrect answer is option 'B'. Can you explain this answer?
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