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Define Cp and CV. Why is CP gt CV ? For ...

Define `C_p` and `C_V`. Why is `C_P gt C_V` ? For an ideal gas, prove that `C_P - C_V = R` .

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To solve the question, we will break it down into several steps, defining \( C_p \) and \( C_v \), explaining why \( C_p > C_v \), and proving that \( C_p - C_v = R \) for an ideal gas. ### Step 1: Define \( C_p \) and \( C_v \) - **Definition of \( C_p \)**: \( C_p \) is defined as the heat required to raise the temperature of one mole of an ideal gas by 1 degree Celsius (or 1 Kelvin) while keeping the pressure constant. Mathematically, this can be expressed as: \[ Q = n C_p \Delta T ...
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C_(P) -C_(V) for an ideal gas is………….. .

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Knowledge Check

  • For an ideal gas C_(p) and C_(v) are related as

    A
    `C_(p) - C_(v) = R`
    B
    `(C_(p))/(C_(v)) = R`
    C
    `C_(p) + C_(v) = R`
    D
    `C_(v) - C_(p) = R`
  • Molar heat capacity of an ideal gas varies as C = C_(v) +alphaT,C=C_(v)+betaV and C = C_(v) + ap , where alpha,beta and a are constant. For an ideal gas in terms of the variables T and V .

    A
    `Ve^((alphaT//R))=const`
    B
    `T.e^((R//betaV))= const`
    C
    `V=anT`
    D
    `Va=nT`
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