Question

A student determines the value of the equilibrium constant to be 1.5297 x 10⁷ for the following reaction:

HBr(g) + 1/2 Cl₂(g) --> HCl(g) +1/2 Br₂(g)

Based on this value of K_eq, calculate the Gibbs free energy change for the reaction of 2.37 moles of HBr(g) at standard conditions at 298 K.

Group of answer choices

ΔGº = +97.1 kJ

ΔGº = -82.0 kJ

ΔGº = +194.2 kJ

ΔGº = -97.1 kJ

ΔGº = -194.2 kJ

How long would it take to produce 3.6 g of platinum by passing a 2.0 ampere current through a solution of PtCl₂?

Group of answer choices

30.0 min.

25.0 min

300.0 min.

15.0 min

60.0 min.

What would be the voltage (E_cell) of a voltaic cell comprised of Cd(s)/Cd²⁺⁽aq) and Zr(s)/Zr⁴⁺⁽aq) if the concentrations of the ions in solution were [Cd²⁺] = 0.5 M and [Zr⁴⁺] = 0.5 M at 298K?

Cd²⁺(aq) + 2 e^- → Cd(s)          Eº = -0.40 V

Zr⁴⁺(aq) + 4 e^- → Zr(s)            Eº = -1.53 V

Group of answer choices

1.126 V

2.846 V

1.181 V

0.301 V

1.530 V