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The behavior of real gas is usually depicted by plotting compressibility factor z versus p at constant temperature. At high temperature and high pressure z is usually more than one(z>1). This fact can be explained by vanderwaals equation when a)constant a is negligible and not b b)constant b is not negligible and not a c)both constant a and b are negligible d)both constant a and b are not negligible
at high pressure , molar volume is low so we cannot neglect b ... at high pressure , correction term in pressure (a/v2) can be neglected so (p+a/v2)(v-b) = RT this equation becomes P(v-b) = RT PV - Pb = RT PV/RT - Pb/RT = 1 Z = 1 + Pb/RT or Z > 1 option a) is correct
at high pressure , molar volume is low so we cannot neglect b ...
at high pressure , correction term in pressure (a/v2) can be neglected so
(p+a/v2)(v-b) = RT
this equation becomes
P(v-b) = RT
PV - Pb = RT
PV/RT - Pb/RT = 1
Z = 1 + Pb/RT
or
Z > 1
option a) is correct
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