The molar heat capacity of silver, measured at atmospheric pressure, is found to vary with temperature between 50 and 100 K by the empirical equation C = 0.318T – 0.00109T 2 – 0.628,where C is in J/mol . K and T is in K. Calculate the quantity of heat required to raise 316 g of silver from 50.0 to 90.0 K. the molar mass of silver is 107.87 g/mol.

Question

Deepak Patra · Answer

To obtain Q, substitute 0.318T &ndash; 0.00109T 2 -0.628 for C in the equation Q = n &int; CdT, we get, Q = n &int; 90 K 50 K CdT = n [(0.318 J/mol.K 2 ) T 2 /2 &ndash; (0.00109 J/mol.K 3 ) T 3 /3 &ndash;(0.628 J/mol.K)T] 90 K 50 K = n (645.8 J/mol) As the molar mass of silver is 107.87 g/mol, thus the quantity of heat required to raise 316 g of silver from 50.0 to 90.0 K will be, Q = n (645.8 J/mol) = [316 g/(107.87 g/mol)] (645.8 J/mol) =189 J From the above observation we conclude that, the quantity of heat required to raise 316 g of silver from 50.0 to 90.0 K would be 189 J.

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