steam vary with temperature; for this problem, use the estimate of 0.5 cal/g • K for both.
The specific heat of water is 1.0 cal/g • K.)(A) 7.325 cal
(B) 7.450 cal
(C) 7.325 kcal
(D) 7.450 kcal5 . Using the information given in the reaction equations below, calculate the heat of
formation for 1 mole of carbon monoxide.
(A) −221 kJ/mol
(B) −110 kJ/mol
(C) 110 kJ/mol
(D) 221 kJ/mol6 . If the free energy change accompanying a reaction is negative,
(A) the reaction can occur spontaneously
(B) the reaction can be used to do work by driving other reactions
(C) the entropy must always be negative
(D) both A and B7 . All of the following are correct statements concerning entropy EXCEPT
(A) All spontaneous processes tend toward an increase in entropy.
(B) The more highly ordered the system, the higher the entropy.
(C) The entropy of a pure crystalline solid at 0 K is 0.
(D) The change in entropy of an equilibrium process is 0.