Consider a reaction that has a negative ΔH and a positive ΔS. Which of the following statements is true?  

Determine the standard entropy change (∆So) for this reaction. 3A2(g) ⟶2A3(g) Substance (state) So (J/mol.K) A(g) 150 A2(g) 200 A3(g) 250

Consider the following redox reaction in an acidic solution: I–(aq)  +  NO3-(aq)  → NO(g)  +  I2(s) When the equation is balanced with smallest whole number coefficients, the coefficient for — (a) NO  = [a] (b) NO3-  = [b] (c) H+  = [c] (d) H2O  = [d]

Calculate the mass of iron metal that will be deposited by passing a 85.0 A current through a solution of iron(II) chloride for 15.0 minutes. Fe2+(aq) + 2 e⁻  →  Fe(s)  You must show all of your work including units for credit.

Calculate the mass of iron metal that will be deposited by passing a 65.0 A current through a solution of iron(III) chloride for 25.0 minutes. Fe3+(aq) + 3 e⁻  →  Fe(s)   You must show all of your work including units for credit.

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 3.00 at 25°C.

Predict the sign (∆S > 0 or ∆S < 0) of the entropy change (∆S) for the following processes. (a) Pb2+(aq) + S2-(aq) ⟶ PbS(s) [a] (b) NaNO3(s) ⟶ Na+(aq) + NO3-(aq) [b] (c) CO2(s) ⟶ CO2(g)[c]

Calculate the cell potential of a voltaic cell, which consists of a Sn/Sn2+ half-cell and a Cu/Cu2+ half-cell. Sn2+ + 2 e⁻  →  Sn Eo = -0.14 V Cu2+ + 2 e⁻  →  Cu Eo = +0.34 V

Are the following solutions acidic, basic, or neutral? a) Ba(NO3)2(aq) [a] b) NaClO2(aq) [b] c) NH4ClO4(aq) [c]

At 298 K , ∆H = -198.4 kJ and ∆S = -187.9 J/K for the reaction shown below. 2SO2(g)  +  O2(g) ⟶ 2SO3(g) (a) Use the data to decide if this reaction is spontaneous at 298 K. [a] (b) What is the temperature below which the reaction is spontaneous? [b]