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Figure displays the plot of the compress...

Figure displays the plot of the compression factor `Z` verses `p` for a few gases
Which of the following statements is//are correct for a van-der waals gas:

A

The plot I is applicable provided the vander waals constant a is negligible.

B

The plot II is a applicable provided the vander waals constant `b` is negligible.

C

The plot III is applicable provided the vander waals constants `a` and `b` are negligible.

D

The plot IV is applicable provided the temperature of the gas is much higher than its critical temperature

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding the compressibility factor \( Z \) versus pressure \( p \) for van der Waals gases, we need to analyze the provided statements based on the behavior of real gases as described by the van der Waals equation. ### Step-by-Step Solution: 1. **Understanding the Van der Waals Equation**: The van der Waals equation is given by: \[ \left( P + \frac{a n^2}{V^2} \right)(V - nb) = nRT \] where \( a \) and \( b \) are van der Waals constants. The compressibility factor \( Z \) is defined as: \[ Z = \frac{PV}{nRT} \] 2. **Analyzing Statement A**: - The first statement claims that the plot is applicable when the van der Waals constant \( A \) is negligible. - If \( a = 0 \), the equation simplifies to the ideal gas law: \[ PV = nRT \implies Z = 1 \] - As pressure increases, \( Z \) increases linearly, confirming that this statement is correct. 3. **Analyzing Statement B**: - The second statement claims that the plot is applicable when the van der Waals constant \( B \) is negligible. - If \( b = 0 \), we can analyze the equation: \[ Z = 1 - \frac{a}{RT} \cdot \frac{n}{V} \] - As pressure increases (and thus \( V \) decreases), \( Z \) becomes less than 1, confirming that this statement is also correct. 4. **Analyzing Statement C**: - The third statement claims that the plot is applicable when both van der Waals constants \( A \) and \( B \) are negligible. - If both \( a \) and \( b \) are zero, we revert to the ideal gas behavior: \[ Z = 1 \] - This indicates that this statement is correct as well. 5. **Analyzing Statement D**: - The fourth statement claims that the plot is applicable when the temperature of the gas is much higher than its critical temperature. - However, above the critical temperature, all gases behave ideally regardless of their nature (real or ideal). Therefore, this statement is false. ### Conclusion: Based on the analysis: - Statements A, B, and C are correct. - Statement D is incorrect. Thus, the correct answer is that statements A, B, and C are correct.

To solve the question regarding the compressibility factor \( Z \) versus pressure \( p \) for van der Waals gases, we need to analyze the provided statements based on the behavior of real gases as described by the van der Waals equation. ### Step-by-Step Solution: 1. **Understanding the Van der Waals Equation**: The van der Waals equation is given by: \[ \left( P + \frac{a n^2}{V^2} \right)(V - nb) = nRT ...
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Knowledge Check

  • For a real gas , the compressibility factor Z has different values at different temperatures and pressures . Which of the following is not correct under the given conditions ?

    A
    Z < 1 at very low pressure .
    B
    Z > 1 at high pressure .
    C
    Z = 1 under all conditions .
    D
    Z = 1 at intermediate pressure
  • Which of the following expressions represents the value and unit of van der Waals constant a?

    A
    `a = (V)/(n) ," L mol"^(-1)`
    B
    `a = (PV)/(n) , "atm L"^(2) mol^(-1)`
    C
    `a = (PV^(2))/(n^(2)) , "atm L"^(2) mol^(-1)`
    D
    `a = (P)/(n) ," atm mol"^(-1)`
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    Which of the following gas will have highest value of van der Waal's constant 'a' ?

    Which of the following van der Waals radii is the largest ?

    The vander Waal's parameters of two gases are given as: Considering the value of parameters, which of the following statement's is/are correct?

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