Determine the cell notation (line notation) for the redox reaction given below:             3 Br2 (g) + 2 Fe(s)  →  6 Br- (aq) + 2 Fe3+ (aq)

What type of intermolecular force causes the dissolution of  KCl  in water? ptable_6.pdf 

How much energy (in kJ) is required to heat 36.0g of H2O from a liquid at 65oC to a gas at 115oC? (molar mass of water = 18.02 g/mol)

Which of the following acids (listed with Ka values) and their conjugate base should be used to form a buffer with a pH of 8.10?   Chapter 17 & 18 equations: pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14.00 Kw = 1 x 10-14 Ka x Kb = Kw = [H3O+][OH-] pKa = -log Ka pH = pKa + log    

The rate law for a reaction was determined to be rate = k[A]0[B]2.  The rate of the reaction is equal to 0.0200 M/s when [A] = 0.100M.  What is the new rate if the concentration of [A] is increased to 0.400 M?  

The Brønsted-Lowry model focuses on the transfer of ________ in an acid-base reaction

Calculate ΔG°rxn for the following reaction at 449.0 K:         CH2O(g) + 2 H2(g)  →  CH4(g) + H2O(g)        ΔH°=  -94.9 kJ ΔS°= -224.2 J/K   Chapter 19 Equations:

Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water.  Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.  (molar mass of HCl = 36.46 g/mol) Chapter 14 Equations:

Determine the pH of a 0.18 M carbonic acid (H2CO3) solution.  Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11   Chapter 17 & 18 equations: pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14.00 Kw = 1 x 10-14 Ka x Kb = Kw = [H3O+][OH-] pKa = -log Ka pH = pKa + log  

Which of the following would have the greatest osmotic pressure?   ptable_6.pdf  Chapter 14 Equations: