1.20 g of an unknown liquid is placed into a 2.3 L container under vacuum. (No gases present.) The liquid completely evaporates at 25.03°C and becomes a gas with a pressure of 325.3 torr. What is the molar mass of the the unknown substance?

The data to the below were collected for the bovine carbonic anhydrase-catalyzed reaction described by

CO2 (aq) + H2O (l) -->H+ (aq) + HCO3- (aq)

Use these values to determine the value of KM, the Michaelis-Menten constant. Answer the four parts below.

a) If you were to plot this data to graphically determine Rmax and KM using a Lineweaver-Burk plot, what would you plot for the following data? If you would plot the original data, enter the original value in the corresponding blank.

[CO2] (mmol * L^-1) graph as R (ݵmol * L^-1 * s^-1) graph as

1.25--> ________ 28.74 --> ________

20.00--> ________ 155.59 --> ________

b) Calculate the slope using the data points from part (a). Then determine the y-intercept using the second point.

Slope= _______ s y-intercept= ___________ L * s * mmol^-1

c) Use the y-intercept to calculate Rmax.

Rmax=___________ mmol * L^-1 * s^-1

d) Use Rmax and the slope to calculate Km.

Km=___________ mmol * L^-1

Using Crystal Field Theory explain how d orbital splitting arises in an octahedrarl field.

Construct a table to show how to make the standard solutions from serial dilution, starting with a stock solution of 1000 ppm in 100 mL volumetric flask.

Use 1000 ppm standard soltuions of Co, Cr, Pb, Cd, and Zn to prepare the following five standard solutions with 10% HNO₃ in 100 mL volumetric flask:

Std 1: 100 ppm of Co, Cr, Pb, Cd, Zn

Std 2: 50 ppm of Co, Cr, Pb, Cd, Zn

Std 3: 10 ppm of Co, Cr, Pb, Cd, Zn

Std 4: 5 ppm of Co, Cr, Pb, Cd, Zn

Std 5: 1 ppm of Co, Cr, Pb, Cd, Zn

The heat energy associated with a change in temperature that does not involve a change in phase is given by

q=msΔT

where q is heat in joules, m is mass in grams, s is specific heat in joules per gram-degree Celsius, J/(g⋅∘C), and ΔT is the temperature change in degrees Celsius. The heat energy associated with a change in phase at constant temperature is given by

q=mΔH

where q is heat in joules, m is mass in grams, and ΔH is the enthalpy in joules per gram.

Physical constants

The constants for H2O are shown here:

Specific heat of ice: sice=2.09 J/(g⋅∘C)

Specific heat of liquid water: swater=4.18 J/(g⋅∘C)

Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g

Enthalpy of vaporization (H2O(l)→H2O(g)): ΔHvap=2250 J/g

Part A

How much heat energy, in kilojoules, is required to convert 63.0 g of ice at −18.0 ∘C to water at 25.0 ∘C ?

Express your answer to three significant figures and include the appropriate units.

Part B

How long would it take for 1.50 mol of water at 100.0 ∘C to be converted completely into steam if heat were added at a constant rate of 15.0 J/s ?

Express your answer to three significant figures and include the appropriate units.

1.2 Which strategy is not a viable “green” option in the chemical industry?
(a) Using catalysts to reduce energy consumption
(b) Reducing the number of steps in a multistep synthesis
(c) Maximizing yield
(d) Running the reaction on a smaller scale

Why would atomic absorption spectroscopy be less sensitive to low source temperature, assuming efficient atomization?

Chloroform, CHCl3, is formed by the following reaction:

CH4(g) + 3 Cl2(g) → 3 HCl(g) + CHCl3 (g)

Determine the enthalpy change for this reaction (ΔH°rxn), using the following:

enthalpy of formation of CHCl3 (g), ΔH°f = – 103.1 kJ/mol

                                CH4(g) + 2 O2(g) → 2 H2O(l) + CO2(g)        ΔH°rxn = – 890.4 kJ/mol

                                2 HCl (g) → H2 (g) + Cl2(g)                              ΔH°rxn = + 184.6 kJ/mol

                                C (graphite) + O2(g) → CO2(g)                     ΔH°rxn = – 393.5 kJ/mol

                                H2 (g) + ½ O2(g) → H2O(l)                              ΔH°rxn = – 285.8 kJ/mol

+ 145.4 kJ

– 305.3 kJ

– 145.4 kJ

+ 305.3 kJ

– 103.1 kJ

Classify each of the following as strong electrolytes, weak electrolytes or nonelectrolytes.

The photoionization of O2 produces O2+. Would you expect higher intensity for 0-0 or 0-2 transitions?

A solution is prepared using a sodium salt of an unknown diprotic base. The unknown diprotic weak base solution will be analyzed for concentration by titration with a strong acid. The unknown is placed in an Erlenmyer flask, and small, measured volumes of a standard strong acid solution are added until the final equivalence point is reached. Then the concentration of the base is calculated fromthe known volumes, the one known concentration and stoichiometry. All solutions are kept at room temperature.

A. Before the titration starts, is the solution in the flask acidic, neutral or alkaline?

B. Write a complete ionic equation for the complete (Bronsted-Lowry) acid-base neutralization reaction of a generic weak diprotic base B^2- with hydrochloric acid.

C. List the most commonform of each solute species that is present in the reaction mixture at the final equivalence point, and label each as a strong acid, weak acid, neutral, weak base, or strong base.

D. At the final equivalence point, will the overall solution be strongly acidic, weakly acidic, neutral, weakly basic, or strongly basic?

E. List the solute species that are present when more standard is added after the final equivalence point, and label each as either a strong acid, weak acid, neutral, weak base or strong base.

F. If extra titrant is added tto the flask after the final equivalence point has been reached, will the mixture be strongly acidic, weakly acidic, neutral, weakly basic, or strongly basic?

A buffer that contains 0.16 M of a base, B and 0.27 M of its conjugate acid BH+, has a pH of 8.56. What is the pH after 0.02 mol of Ba(OH)2 are added to 0.52 L of the solution?

Determine the term symbols for :

A) 3P² , B) s¹p¹d¹ electron configuration.

C) Determine the energy free ion spectroscopic state (ground state) of a d³ species.