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Show that the volume thermal expansion coefficient for an ideal gas at constant pressure is `(1)/(T)`.

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To show that the volume thermal expansion coefficient (γ) for an ideal gas at constant pressure is \( \frac{1}{T} \), we can follow these steps: ### Step 1: Define the volume thermal expansion coefficient The volume thermal expansion coefficient (γ) is defined as: \[ \gamma = \frac{\Delta V}{V \Delta T} \] where \( \Delta V \) is the change in volume, \( V \) is the original volume, and \( \Delta T \) is the change in temperature. ### Step 2: Use the ideal gas law For an ideal gas, the relationship between pressure (P), volume (V), and temperature (T) is given by the ideal gas equation: \[ PV = nRT \] where \( n \) is the number of moles and \( R \) is the ideal gas constant. ### Step 3: Differentiate the ideal gas equation At constant pressure, we can differentiate the ideal gas equation with respect to temperature: \[ P \frac{dV}{dT} = nR \] This implies: \[ \frac{dV}{dT} = \frac{nR}{P} \] ### Step 4: Substitute \( nR \) using the ideal gas law From the ideal gas law, we know that \( nR = \frac{PV}{T} \). Substituting this into the equation we derived in Step 3 gives: \[ \frac{dV}{dT} = \frac{PV}{PT} = \frac{V}{T} \] ### Step 5: Relate \( \Delta V \) to \( \Delta T \) Now, we can express \( \Delta V \) in terms of \( \Delta T \): \[ \Delta V = \frac{V}{T} \Delta T \] ### Step 6: Substitute \( \Delta V \) back into the definition of γ Now, substituting \( \Delta V \) into the definition of γ: \[ \gamma = \frac{\Delta V}{V \Delta T} = \frac{\frac{V}{T} \Delta T}{V \Delta T} = \frac{1}{T} \] ### Conclusion Thus, we have shown that the volume thermal expansion coefficient for an ideal gas at constant pressure is: \[ \gamma = \frac{1}{T} \] ---

To show that the volume thermal expansion coefficient (γ) for an ideal gas at constant pressure is \( \frac{1}{T} \), we can follow these steps: ### Step 1: Define the volume thermal expansion coefficient The volume thermal expansion coefficient (γ) is defined as: \[ \gamma = \frac{\Delta V}{V \Delta T} \] where \( \Delta V \) is the change in volume, \( V \) is the original volume, and \( \Delta T \) is the change in temperature. ...
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Knowledge Check

  • If an ideal gas is heated at constant pressure :

    A
    the volume increases
    B
    the mass of gas remains same
    C
    the kinetic energy of the molecules increases
    D
    attraction forces between gas particles increases
  • Work done during expansion of an ideal gas against constant opposing pressure is given by

    A
    `W=2.303" RT log "(V_(2))/(V_(1))`
    B
    `W=2.303" RT log "(V_(1))/(V_(2))`
    C
    `W=-P(V_(2)-V_(1))`
    D
    `W=0`
  • The volume-temperature graphs of a given mass of an ideal gas at constant pressures are shown below. What is the correct order of pressures ?

    A
    `p_(1) gt p_(3) gt p_(2)`
    B
    `p_(1) gt p_(2) gt p_(3)`
    C
    `p_(2) gt p_(3) gt p_(1)`
    D
    `p_(2) gt p_(1) gt p_(3)`
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