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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
SO2+Cl2, CO+Cl2, NO+O2, NH3+HCl and H2 + Cl2
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Community Answer
In which of the following mixtures, Daltons law of partial pressure is...
Explanation:
Dalton's Law of Partial Pressure:
Dalton's Law of Partial Pressure states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of individual gases in the mixture.
Reason why Dalton's Law is not applicable to H2 and Cl2 mixture:
- In a mixture of hydrogen (H2) and chlorine (Cl2) gases, the two gases can react with each other to form hydrogen chloride (HCl) gas. This reaction would change the composition of the mixture and hence the partial pressures of the individual gases.
- As a result, Dalton's Law of Partial Pressure would not be applicable to this mixture as the gases are not behaving independently and the total pressure may not simply be the sum of the partial pressures of the individual gases.
Conclusion:
Therefore, Dalton's Law of Partial Pressure would not be applicable to a mixture of hydrogen (H2) and chlorine (Cl2) gases due to their potential to react with each other, leading to a change in composition and pressure.
Dalton's Law of Partial Pressure:
Dalton's Law of Partial Pressure states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of individual gases in the mixture.
Reason why Dalton's Law is not applicable to H2 and Cl2 mixture:
- In a mixture of hydrogen (H2) and chlorine (Cl2) gases, the two gases can react with each other to form hydrogen chloride (HCl) gas. This reaction would change the composition of the mixture and hence the partial pressures of the individual gases.
- As a result, Dalton's Law of Partial Pressure would not be applicable to this mixture as the gases are not behaving independently and the total pressure may not simply be the sum of the partial pressures of the individual gases.
Conclusion:
Therefore, Dalton's Law of Partial Pressure would not be applicable to a mixture of hydrogen (H2) and chlorine (Cl2) gases due to their potential to react with each other, leading to a change in composition and pressure.
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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)H2 and CO2 mixtured)None of theseCorrect answer is option 'B'. Can you explain this answer?
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