Take all the thermodynamic data from your textbook. Assume the data do not vary

Question

Take all the thermodynamic data from your textbook. Assume the data do not vary with temperature. Calculate Delta S_univ for the reaction H_2O_2(l) rightarrow H_2O_2(g) at 175.0 degree C. Enter your answer in the box provided. Is the reaction spontaneous, nonspontaneous, or an equilibrium process? Select the best single answer. spontaneous nonspontaneous an equilibrium process The reaction NH_3(g) + HCl(g) rightarrow NH_4 Cl(s) is spontaneous in the forward direction at room temperature. Determine the temperature at which it is no longer spontaneous in the forward direction.

Explanation / Answer

a) Entropy of H2O2(g) = 232.95 J/K (data taken from my class notes. plug in your values)

Entropy of H2O2(l) = 110 J/K (data taken from my class notes. plug in your values)

Entropy of the Reaction = Entropy of the Product - Entropy of the Reactant

=> 232.95 - 110

=> 122.95 J/K

(b) The reaction will be spontaneous since entropy of the reaction is positive

c) NH3 + HCl ----- NH4Cl

entropy of NH3 = 192.3

Entropy of HCl = 186.8

Entropy of NH4Cl(s) = 94.6

Entropy of the reaction = 94.6 - (192.3+186.8) = -284.5 J/K

Delta H of the reaction = -314.4 + 45.94 + 92.31 = -176.15 KJ/mol

Temperature = DeltaH/Delta S = 176.15 Kj/284.5 J/K = 619.15 K

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