For the follow reaction under standard state conditions answer the following statements below: Pb2+(aq) +Fe(s)

Which of the following statements is/are true about graphs regarding rate data below? The half-life, t1/2, is independent of concentration Changing the concentration of A will not affect the rate of the reaction The units for the rate constant k are s-1

Determine if the following statements about the solubility of a gas are true or false.  The solubility of a gas increases as the strength of the intermolecular forces increases between the solute (gas) and the solvent. The solubility of a gas decreases as temperature increases. The solubility of a gas decreases as pressure increases.

Which of the following statements is/are correct about the graph shown below?   The graph represents a strong acid/strong base titration The pH at the equivalence point in approximately 8.25 The pKa is approximately 8.25

The decomposition of MZ is second order in MZ and has a rate constant of 3.60 x 10-3 M-1s-1 at a certain temperature. If the initial concentration of XY is 0.234 M, what will be the concentration of MZ after 248 mins?

Determine if the following statements regarding buffers are True of False? HF would be a good choice for a buffer with a desired pH of 6.75 HCN would be a good choice for a buffer with a desired pH of 9.50 HC2Cl3O2 would be a good choice for a buffer with a desired pH of 13.75 HIO would be a good choice for a buffer with a desired pH of 11.25

Which of the following statement(s) is/are correct (true) about a system at equilibrium            X3 (aq) + Z3 (aq) ⇌ 3 XZ (aq)                 K = 6.7 x 10-4 The concentration of the reactants is greater than the concentration of products. The rate of the forward reaction is less than the rate of the reverse reaction. Both the forward and the reverse reactions continue to occur once the system has reached equilibrium.

Use the reaction shown below and the given equilibrium concentrations to determine the value of K for the reaction at 37 oC eq = 2.3 M, eq = 1.1 M, eq = 0.90 M

What is the pH of a solution when 70.0 mL of 0.090 M HCl is added to 50.0 mL 0.550 M LiOH at 25OC?

Comment on the spontaneity of the reaction given:  ΔH = 301.8 kJ and  ΔS = 267.5 J/K The reaction will be spontaneous