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?

NAD^+(aq)+2H^+(aq)+2e^- --> NADH(aq)+H^+(aq) E= -0.320V

Oaloacetate^2-(aq)+2H^+(aq)+2e^- --> malate^2-(aq) E= -0.166V

a. Calculate the standard potential for the following reaction: Oxaloacetate^2- (aq) +NADH(aq)+H^+(aq) --> malate-(aq)+NAD^+(aq)

b. Calculate the equilibrium constant for the reaction at 298K

The Na –glucose symport system of intestinal epithelial cells couples the \"downhill\" transport of two Na ions into the cell to the \"uphill\" transport of glucose, pumping glucose into the cell against its concentration gradient. If the Na concentration outside the cell ([Na ]out) is 163 mM and that inside the cell ([Na ]in) is 23.0 mM, and the cell potential is -51.0 mV (inside negative), calculate the maximum ratio of [glucose]in to [glucose]out that could theoretically be produced if the energy coupling were 100% efficient. Assume the temperature is 37 °C.

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?

Two sig. figs.

m= ?

For a molecule of fluorous acid, the atoms are arranged as HOFO. (Note: In this oxyacid, the placement of fluorine is an exception to the rule of putting the more electronegative atom in a terminal position.) What is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed. Express your answers as charges separated by comma. For example, a positive one charge would be written as +1.

Discuss the difference of the following sample preparation: (a) Liquid-liquid extraction (LLE) (b) Soxhlet extraction (c) Solid phase extraction (SPE) in terms of application, cost, extraction time, solvent usage.

1.) Determine the energy change (in Joules) associated with the transition from n=2 to n=4 in the Hydrogen atom.

2.) Calculate the wavelength (in nm) of the red line in the visible spectrum of excited H atoms using Bohr Theory.

3.) What is the energy (in Joules) of the X-ray radiation at 2.00x10^-10 m that are used for medical diagnosis?

4.) What is the binding energy of an electron in a photosensitive metal (in kj/mol) if the minimum frequency of light that can eject electrons from the metal is 6.3x10^14 Hz?

5.) How many photons are contained in a burst of yellow light (589nm) for a sodium lamp that contains 609 kJ of energy?

Which of the following hydrocarbons is expected to be the most reactive in ethanloic silver nitrate? Why? Write the organic product that you expect when your chosen substrate reacts.

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Draw the conjugate acid of compound A. Explain you choice.

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Provide a mechanism. Include all intermediates. Show all electron pushing.

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