Whenever a substance is heated, its enthalpy increases, as suggested by the relation, ∆?=Cp∆?. However, the molar heat capacity itself is a function of temperature, and for N2 this function can be modeled as ?p(?)=? + ?? + c / T2 where a= 28.58 J/mol·K, b= 0.00377 J/mol·K2, and
Whenever a substance is heated, its enthalpy increases, as suggested by the relation, ∆?=Cp∆?. However, the molar heat capacity itself is a function of temperature, and for N2 this function can be modeled as
?p(?)=? + ?? + c / T2
where a= 28.58 J/mol·K, b= 0.00377 J/mol·K2, and
c= –5.0 x 104J·K/mol.
(a) What does this formula for heat capacity predict for the value of ?p(?)at 300K?
(b) Now, compute the enthalpy change associated with heating 0.62 moles of N2 from 300 to 600 K using the formula for ?p (?), and report the answer in J.
(c) What is the difference between this value and one computed using the constant value for Cp at 300 K from part (a)? Report the absolute value of the difference in J.
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