Calculate Delta S degree_rxn for the following reaction. The S^+ for each specie

Question

Calculate Delta S degree_rxn for the following reaction. The S^+ for each species is shown below the reaction. N_2H_4(l) + H_2(g) rightarrow 2 NH_3(g) s*(J/mol middot K) 121.2 130.7 192.8 -202.3 J/k +133.7 J/K + 178.9 J/K -59.1 J/K -118.2 J/K Place the following in order of decreasing entropy. N_2O_4(g) NO(g) NO_2(g) N_2O_4 > NO > NO_2 N_2O_4 > NO_2 > NO NO_2 > NO > N_2O_4 NO > NO_2 > N_2O_4 NO > N_2O_4 > NO_2 What is the oxidation number of bromine in the BrO_3^- ion? +5 -1 +7 +1 +3 Identify the location where reduction takes place in an electrochemical cell. the salt bridge the cathode the socket the anode the electrode Use the standard half-cell potentials listed below to calculate the standard cell potential(E degree_cell) for the following reaction occurring in an electrochemical cell at 25 degree C. (The equation is balanced.) 3 Cl_2(g) + 2 Fe(s) rightarrow 6 Cl^-(aq) + 2 Fe^3+(aq) Cl_2(g) + 2e^- rightarrow 2 Cl^-(aq) E degree = +1.36 V Fe^3+(aq)

Explanation / Answer

Q28.

By definition, the change of entropy of a reaction (Srxn°) if given by:

Srxn° = (n*Sproducts - n*Sreactants)

Then; products is NH3 and reactants are N2H4 and H2

Sproducts = NH3

Sproducts = N2H4 and H2

NOTE: make sure the equation is balanced, in this case, it is already balanced...

Srxn° = (2*NH3 - 1*N2H4 - 1*H2)

Srxn° = (2*192.8 - 1*121.2 - 130.7) J/molK

Srxn° = 133.7 J/molK

nearest answer is B; +133.7 J/molK

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