Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 OC. (The equation is balanced.)  Pb(s) + Br2 (l) à Pb2+ (aq) + 2 Br- (aq) Pb2+ (aq) + 2 e- à Pb (s)                  EO = -0.13 V Br2 (l) + 2 e- à2 Br- (aq)                  EO = +1.07 V

What are funeral goods consumers purchase from a source other than the price list/funeral providers offer?

Which of the following is considered the keystone of “the rule”?

Tangible items which are sold or offered for dale directly to the public for use during the funeral are called

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. SO3 (g) + H2O (g) ↔ H2SO4 (l)                   ΔG O = -90.5 kJ P(SO3) = 0.20 atm; P(H2O) = 0.88 atm

Mrs. Lindes calls you to her home to set up a pre-funded contract. Which is true

Calculate the concentration of H3O+ in a solution that contains 5.5 X 10-5M OH- at 25 ºC. Also , identify the solution as acidic, basic, or neutral. **Submit your answer in scientific notation using the following format. 5.5 X 10^-5 M

The rate constant for the first-order decomposition of N2O is 3.40 s-1. What is the half-life of the decomposition? ** Don’t forget the units. round to the third decimal place

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 M O2 at 25°C. The Henry’s law constant for oxygen in water at 25°C is 1.3 × 10-3 M/atm.  (report you answer WITH UNITS to the second decimal place.)

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2 (g). N2O4 (g) ⇌ 2NO2 (g)                 Kc = 0.21, eq = 0.039 M