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It can be shown that for a simple compressible substance, the relationshipcp - cv = - T \(\left(\cfrac{∂V}{∂T}\right)^2_p\)\(\left(\cfrac{∂p}{∂v}\right)_T\) existswhere cp and cv are specific heats at constant pressure and constant volume respectively, T is temperature, V is volume and p is pressure. Which one of the following statements is NOT true ? (a) cp is always greater than cv (b) The right side of the equation reduces to R for an ideal gas(c) Since \(\left(\cfrac{∂p}{∂v}\right)_T\) can be either positive or negative, and \(\left(\cfrac{∂V}{∂T}\right)_p\) must be positive, T must have a sign which is opposite to that of \(\left(\cfrac{∂p}{∂v}\right)_T\)(d) cp is very nearly equal to cv for liquid water. |
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Answer» (b) The right side of the equation reduces to R for an ideal gas |
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