For a sample containing both protein and nucleic acid, the absorbance measured at a particular wavelength will be the sum of contributions from both types of molecule. Using the protein and nucleic acid concentrations you calculated in the previous step, calculate how much of the absorbance of the BSA and E.coli extract comes from protein and how much from nucleic acid, at each wavelength. HINT: the values in the table provided, are in essence, extinction coefficients with the units (mg/ml)^-1cm^-1.

There was a question previous to this, and I calculated that my protein concentration is 0.58 mg/ml and that my nucleic acid concentration is 0.04 mg/ml.

this is what I have come up with so far, but I am not sure if it is correct, and am not sure how to use it to determine how much absorbance is from protein or nucleic acid.

A₂₈₀=C_protein280*ε_protein280 + C_{nucleic acid280}*ε_{nucleic acid280}

_and A₂₆₀=C_protein260*ε_protein260 + C_{nucleic acid260}*ε_{nucleic acid260}

A₂₈₀=(0.58 mg/ml)*(0.894cm^-1M^-1) + (0.04 mg/ml)*(10.8cm^-1M^-1)

A₂₈₀=0.51852+0.432

A₂₈₀=0.95052

and A₂₆₀=(0.58mg/ml)(0.512 cm^-1M^-1) + (0.04 mg/ml)*(22.1 cm^-1M^-1)

A₂₆₀=0.29696+0.884

A₂₆₀=1.18

Two aqueous hydrogen bromide solutions containing 12.0 wt% HBr (SG = 1.1377) and 30.0 wt% HBr (SG = 1.2552) are mixed to form a 4.27 molar HBr solution (SG = 1.2340)

1.What feed rate of the 30.0 wt% HBr solution would be required to produce 1150 kg/hr of product?
2. What is the feed ratio of liters of 12.0 wt% HBr solution to liters of 30.0 wt% HBr solution?

In photography, unexposed silver bromide is removed from film by soaking the film in a solution of sodium thiosulfate, Na₂S₂O₃. Silver ion forms a soluble complex with thiosulfate ion, S₂O₃^2-, that has the formula Ag(S₂O₃)₂^3-, and formation of the complex causes the AgBr in the film to dissolve. The Ag(S₂O₃)₂^3- complex has K_form= 2.0 x 10¹³. How many grams of AgBr (K_sp= 5.4 x 10^-13) will dissolve in 126 mL of 1.27 M Na₂S₂O₃ solution?

The entropy of sublimation of a certain compound is 20.7 J K–1 mol–1 at its normal sublimation point of 101 °C. Calculate the vapour pressure (in torr) of the compound at 9 °C. Assume that the enthalpy of sublimation is constant.

A 50.0-mL solution containing Ni2+ and Zn2+ was treated with 25.0 mL of 0.0452 M EDTA to bind all the metal. The excess unreated EDTA required 12.4 mL of 0.0123 M Mg2+ for complete reaction. An excess of the reagent 2,3-dimercapto-1-propanol was then added to displace the EDTA from zinc. Another 29.2 mL of Mg2+ was required for reaction with the liberated EDTA. Calculate the molarity of Ni2+ and Zn2+ in the original solution

Choose all that apply. Solids, liquids, and gases can be distinguished by their?

A. Molecular Level

B. Shape

C.Temperature

D. Kinetic Energy

E. Mass

F. Density

- (a) What factors determine whether a collision between two molecules will lead to a chemical reaction?

(b) According to the collision model, why does temperature affect the value of the rate constant? (c) Does the rate constant for a reaction generally increase or decrease with an increase in reaction temperature?

Free chlorine in water distributes between HOCl and OCL^- species according to the following reaction:

HOCl <--> H^+ + OCl^-

K=[H^+][OCl^-]/[HOCl] = 10^-7.6 @ 25 degrees C

A water has a pH of 7.8, temperature of 25 degrees C, and the total free chlorine (HOCl + OCl^-) = 1.2*10^-4 mole/L. Calculate the concentration of the HOCl species in mg/L.

For a particular redox reaction BrO– is oxidized to BrO3– and Ag is reduced to Ag. Complete and balance the equation for this reaction in basic solution. Phases are optional.

Ethyl chloride (C2H5Cl) boils at 12∘C. When liquid C2H5Cl under pressure is sprayed on a room-temperature (25∘C) surface in air, the surface is cooled considerably.Assume that the heat lost by the surface is gained by ethyl chloride. What enthalpies must you consider if you were to calculate the final temperature of the surface?

Check all that apply.

The specific heat of the solid surface

The enthalpy of vaporization of C2H5Cl(l)

The specific heat of C2H5Cl(l)

The specific heat of C2H5Cl(g)

suppose 1.00 mol of ice at -30.0c is heated at ... Question Suppose 1.00 mol of ice at -30.0C is heated at atmospheric pressure until it is converted to steam at 140.C. Calculated Q, W, ΔH, and ΔU for this process. For ice, water, and steam, Cpm = 38.0, 75.0, and 36.0 J/mol K, respectively, and can be taken to be approximately independent of temperature. ΔHfus for ice is 6.007 kJ mol , and ΔHvap for water is 40.66 kJ mol . Use the ideal gas law for steam, and assume that the volume of ice or water is negligible relative to that of 1 mol of steam.

Please select ONE of the questions below to answer. Use GCU style (no first-person, no contractions, no quotes). Support your response with references from course articles or text readings. Every student’s response is expected to have examples and demonstrate understanding of chemistry.

DQ1

1. Pressure changes are utilized in many common items, internal combustion engines, vacuum cleaners, etc. Describe a unique example of a commonly exploited pressure change and how it is works.

2. Provide a unique and common example of diffusion. Your answer should include the molecules involved and the types of factors that might affect the diffusions of said molecules.

3. The ideal gas law encompasses many other laws. Provide a unique example that follows the ideal gas law and specify how it is applied.

use 100 words or more, include a source, don not copy and paste

Suppose that 200.0mL of a 0.1220 M HCL solution was added to a full antacid tabet containing CaCO3. The HCl fully reacted with the CO3^2- and the excess HCL was then back titrated with a 0.1050 M NaOH solution. The back titratin required 32.20 mL based on this data, calculate the moles of CaCO3 in the balet and the weight of CaCo3 IN THE TABLET (the molecular weight of CaCO3 is 100.09 g/mol)

What would these calculations look like?

a mixture of 0.2 mol of NO, 0.1 mol of H2 and 0.2 mol of H2O is placed in 2.0 L at 300 K. At equal [NO] = 0.062. Calculate K