For the reaction show below determine the rate law.

CH3COCH3 + Br2 → CH3COCH2Br + HBr(aq)

The bromination of acetone, an organic solvent, is catalyzed by an acid. The rate of disappearance of bromine was measured for several different concentrations of the reactants including the catalyst, H+. Therefore, the catalyst will appear in the rate law, but not in the overall reaction. The following data were obtained:

[CH3COCH3] [Br2] [H+] Initial Rate (mol/L s)

0.30 0.05 0.05 5.7 x 10-5

0.30 0.10 0.05 5.7 x 10-5

0.30 0.05 0.10 11.7 x 10-5

0.40 0.05 0.05 7.6 x 10-5

Calculate the rate law for this reaction: rate = k [CH3COCH3][ ] [Br2][ ] [H+][ ]

Post Lab Questions:

A perfect percent yield would be 100%. Based on your results, describe your degree of accuracy and suggest possible sources of error.

What impact would adding twice as much Na₂CO₃ than required for stoichiometric quantities have on the quantity of product produced?

Determine the quantity (g) of pure CaCl₂ in 7.5 g of CaCl₂•9H₂O.

Determine the quantity (g) of pure MgSO₄ in 2.4 g of MgSO₄•7H₂O.

Conservation of mass was discussed in the background. Describe how conservation of mass (actual, not theoretical) could be checked in the experiment performed.

Based on these findings:

Data Table 1. Stoichiometry Values

What is cyanoarylate ester? What is it used for? What is the history behind it?

How many grams of AgBr will dissolve in 1.0 L of water containing a Br- concentration of 0.050 M? Ksp= 5.0 * 10^-13

Calculate the ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH°f(kJ/mol) -20.6 296.8 -241.8 S°(J/mol∙K) 205.8 205. 248.2 188.8 ΔG°rxn = ?

Propose a buffer system using ascorbic acid. Explain how this solution can protect against acids and bases, specifically.

Compare the deltaS fusion with the deltaS vaporization for water. Are they reasonable in terms of the relative disorder of the states of matter?

deltaH fusion= 6.10 kJ/mol and deltaH vap= 40.7 kJ/mol

Write balanced net ionic equations for the following reactions in basic solution:

H2O2(aq)+Cr2O2−7(aq)⟶O2(g)+Cr3+(aq)

Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.

a. Assuming that glucose and water form an ideal solution, what is the partial pressure of water at 20o C of a solution of 1.00 g of glucose (mol wt 180 g/mol) in 100 g of water? The vapor pressure of pure water is 2338 Pa at 20o C.

b. What is the osmotic pressure, in Pa, of the solution in part (a) versus pure water?

c. What would be the osmotic pressure, in Pa, of a solution containing both 1.00 g of glucose and 1.00 g of sucrose (mol wt 342) in 100 g of water at 20o C?

What is the pH of 50 ml of a 0.10M weak acid (Ka =1.0x10-5) plus 50ml water?

What is the pH of 50 ml 0.010M weak base plus 100ml water ? Kb =1.0x10-5.

Electronic configurations follow from the principle quantum numbers n, l, m, and s. What is the relationship with n and the periodic table? What is the relationship with n and the number of valance electrons? The ‘l ’ quantum number designates the type of orbital. What is an orbital? Do electrons have to stay in their designated orbital? The ‘m’ quantum number gives the degeneracy of the orbital type. Is there a difference in the px and py orbitals? Why does the spinning of the two electrons sharing an orbital have to be opposite. Are electrons really spinning?

Balance the following oxidation-reduction reactions using the half-reaction method.

a) S^2-(aq) + NO₃^-(aq) ---> S₈(s) + NO₂(g) acidic solution

b) MnO₄^-(aq) + I^-(aq) ---> MnO₂(s) + IO₃^-(aq) basic solution

c) Sb(s) + H₂SO₄(aq) ---> Sb₂(SO₄)₃(s) + SO₂(g) acidic solution

1) Sort the phrases pertaining to pure substances and mixtures as either true or false. Note: If any part of this question is answered incorrectly, a single red X will appear indicating that one or more of the phrases has been placed incorrectly.

a)pure substances cnnot be separated by physical means.

b) homogeneous mixtures have unifform properties throughout.

c) the components of homogeneous and heterogeneous mixtures cannot be separated.

d) components of a homogeneous mixture are visibly distinct.

e) heterogeneous mixtures contain more than one part, and each part has its own properties.

A 110.0 −mL buffer solution is 0.110 M in NH3 and 0.135 M in NH4Br.

Part A What mass of HCl could this buffer neutralize before the pH fell below 9.00? Express your answer using two significant figures.

m=?

Part B If the same volume of the buffer were 0.265 M in NH3 and 0.390 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00? Express your answer using two significant figures.

m=?

What is the difference between absorption and emission? Transmission and reflection?

When plotting a graph of A vs. B, what does it mean if one says that A is directly proportional to B? What would the graph look like?