Think about the forces between molecules, and explain why we might expect B ( T )to be negative at low temperatures but positive at high temperatures.Discuss the validity of the ideal gas law under these conditions. For each temperature in the table, compute the second term in the virial equation, B ( T ) / ( V / n ), for nitrogen at atmospheric pressure.Here are some measured values of the second virial coefficient for nitrogen ( N 2): T ( K ) In many situations, it’s sufficient to omit the third term and concentrate on the second, whose coefficient B ( T )is called the second virial coefficient (the first coefficient is 1). When the density of the gas is fairly low, so that the volume per mole is large, each term in the series is much smaller than the one before. Where the functions B ( T ), C ( T ), and so on are called the virial coefficients. P V − n R T ( 1 + B ( T ) ( V / n ) + C ( T ) ( V / n ) 2 + ⋯ ) A systematic way to account for deviations from ideal behavior is the virial Even at low density, real gases don’t quite obey the ideal gas law.
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