1. The molar mass of a compound is 126 g/mol, and it's empirical formula is C2H2O. What is compound's molecular formula?

2. A compound consist of 26.18g Si and 29.82g O. Calculate its empirical formula?

3. Calculate the empirical formula of the compound that consist of 70.4%F and 29.6%O.

1. Which assay is more likely to be accurate for BSA concentrations: ninhydrin or Bradford, and why?
2. (a) Tell me the different forms of Coomassie Blue at different pH's (b) Tell me what causes Coomassie Blue in acid to change its color when meeting a protein. (c) Tell me to which parts of a protein molecule the Coomassie Blue binds.  

C: CaCO3 (s) ----> CaO (s) + CO2 (g) delta H= +178 kJ/mol
D: PCl3 (g) + Cl2 (g) -----> PCl5 (g) delta H= - 88 kJ/mol

Classify these changes as either LEFTWARD SHIFT, RIGTHWARD SHIFT, or NO SHIFT

System C increase temperature
System C decrease temperature
System D increase temperature
System D decrease temperature

What products result when calcium carbide is combined with water?

Molarity of standard NaOH solution: x/1 H 2/3 Unknown + 2/3 NaOH -> 2/3 H2O +Na 2/3 Acetate

Unknown Acid code and number of reactive hydrogens: H+3

4. Find the molarity of the vinegar for each of your three vinegar titrations, then find the average molarity of the acid.

5. Find the percent deviations for your three vinegar molarities for the vinegar titrations.

6. From the moles of acetic acid for each vinegar titration, find the mass of acetic acid for that titration

A fire extinguisher has a pressure of 12 atm at 25∘C.What is the final pressure, in atmospheres, when the fire extinguisher is used at a temperature of 63 ∘C, if Vand n are constant?

P=

What are the rules for net ionic equations? I know you must follow the solubility chart, but I'm confused about the other aspects. When the compound is solid, gas or liquid, I don't break apart the compound right? Unless the compound is a strong acid and base? I already know the steps of finding the net ionic equation. I'm just not sure about the rules. So if you could provide an example for the different reactions, can you also include the differences when using the rules?

In the williamson ether synthesis of n-butyl methyl ether from 1-bromobutane, sodium, and ethanol, how could the purity as well as the percent yield of the product be improved?

Consider the following reaction:

CO(g)+2H2(g)⇌CH3OH(g)CO(g)+2H2(g)⇌CH3OH(g)

The reaction between COCO and H2H2 is carried out at a specific temperature with initial concentrations of COCO = 0.32  M M and H2H2 = 0.52  M M. At equilibrium, the concentration of CH3OHCH3OH is 0.15  M M.

Find the equilibrium constant at this temperature.

Express your answer using two significant figures.

Please answer and exaplain ALL 4 parts! Thank you!

A 3.00 mL aliquot of 0.001 M NaSCN is diluted to 25.0 mL with 0.2 M Fe(NO3)3 and 0.1 M HNO3.

1. How many moles of SCN- are present?

2. If all of the SCN- is complexed with Fe3+ to form FeNCS2+, what is the molar concentration of FeNCS2+?

3. For preparing a set of standard solutions of FeNCS2+, the equilibrium molar concentration of FeNCS2+ is assumed to equal the initial molar concentration of the SCN- in the reaction mixture. Why is this assumption valid?

4. The blank solution used to calibrate a spectrophotometer is 10.0 mL of 0.2 M Fe(NO3)3 diluted to 25.0 mL with 0.1 M HNO3. Why is this solution preferred to simply using de-ionized water for the calibration?

What is the concentration of a solution created by mixing 25g of C₃H₆O_(L) (D = 0.774 g/mL) with 25g of CH₄O_(L) (D = 0.890 g/mL)?

Which of the following has the highest boiling point? Please provide an explanation on how to solve this!

a. CH₃OH                b. CH₃Cl                  c. CH₃SH                 d. CH₃CH₃                       e. CH₃F

HClO is a weak acid (Ka=4.0×10^−8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.037 M in NaClO at 25 °C?

A 27.7 mL sample of 0.314 M ethylamine, C2H5NH2, is titrated with 0.325 M nitric acid. The pH before the addition of any nitric acid is .

Use the Tables link in the References for any equilibrium constants that are required.