Thehormone estrogen is produced in the ovaries of females and elsewhere in the body in men and post-
menopausal women, and it is also administered in estrogen replacement therapy, a common treatment
for women who have undergone a hysterectomy. Unfortunately, it also binds to estrogen receptors in
breast tissue and can activate cells to become cancerous. Tamoxifen is a drug that also binds to estrogen
receptors but does not activate cells, in effect blocking the receptors from access to estrogen and
inhibiting the growth of breast-cancer cells.
Tamoxifen is administered in tablet form. In the manufacturing process, a finely ground powder
contains tamoxifen (tam) and two inactive fillers—lactose monohydrate (lac) and corn starch (cs). The
powder is mixed with a second stream containing water and suspended solid particles of polyvinylpyrro-
lidone (pvp) binder, which keeps the tablets from easily crumbling. The slurry leaving the mixer goes to a
dryer,inwhich94.2%ofthewaterfedtotheprocessisvaporized.Thewetpowderleavingthedryercontains
8.80wt% tam, 66.8% lac, 21.4% cs, 2.00% pvp, and 1.00% water. After some additional processing, the
powder is molded into tablets. To produce a hundred thousand tablets, 17.13kg of wet powder is required.
(a) Taking a basis of 100,000 tablets produced, draw and label a process flowchart, labeling masses of
individual components rather than total masses and component mass fractions. It is unnecessary to
label the stream between the mixer and the dryer. Carry out a degree-of-freedom analysis of the
overall two-unit process.
(b) Calculate the masses and compositions of the streams that must enter the mixer to make 100,000
tablets.
(c) Why was it unnecessary to label the stream between the mixer and the dryer? Under what
circumstances would it have been necessary?
(d) Go back to the flowchart ofPart (a). Without using the mass of the wet powder (17.13kg) or any of
the results from Part (b) in your calculations, determine the mass fractions of the stream
components in the powder fed to the mixer and verify that they match your solution to Part (b).
(Hint: Take a basis of 100kg of wet powder.)
(e) Suppose a student does Part (d) before Part (b), and re-labels the powder feed to the mixer on the
flowchart of Part (a) with an unknown total mass (m1) and the three now known mole fractions.
(Sketch the resulting flowchart.) The student then does a degree-of-freedom analysis, counts
four unknowns (the masses of the powder, pvp, and water fed to the mixer, and the mass of
water evaporated in the dryer), and six equations (five material balances for five species and the
percentage evaporation), for a net of 2 degrees of freedom. Since there are more equations than
unknowns, it should not be possible to get a unique solution for the four unknowns. Never-
theless, the student writes four equations, solves for the four unknowns, and verifies that all of the balance equations are satisfied. There must have been a mistake in the degree-of-freedom
calculation. What was it?

Hello. I am attempting to test kidney stone solubility by using titration methods. I want to set up an experiment that incorporates lemon juice and EDTA solution to dissolve an artificial kidney stone. I need to find a procedure that includes: lemon juice, kidney stone(calcium oxalate), EDTA, and titration methods. Please be as detailed as possible with step-by-step instructions. Thank you.

a) Calculate the pH during the titration of 30.00 mL of 0.1000 M trimethylamine, (CH₃)₃N(aq), with 0.1000 M HCl(aq) after 24 mL of the acid have been added. K_b of trimethylamine = 6.5 x 10^-5.

b)Calculate the pH during the titration of 20.00 mL of 0.1000 M methylamine, CH₃NH₂(aq), with 0.1000 M HNO₃(aq) after 19.9 mL of the acid have been added. K_b of methylamine = 3.6 x 10^-4.

A canister contains butane at a pressure of 760 torr and a temprature of 25C. All of contents of the canister are allowed to react with excess oxygen to produce carbon dioxide and water.

2 (C4H10) + 13O2 -------> 8CO2+ 10(H2O)

Equation is balanced and butane is completely consumed in the reaction, and 46.5g grams of CO2 are produced. What is the volume, in liters, of the canister that contained the butane??

Answer is 6.46L but can anyone please show work for this question?? I just can't get the right answer or near even near it. Please teach me how to approach this problem. Thank You!

I need to know the following values in the table below. All the info you need should be listed.

1. Write the balanced equation for the reaction between solid zinc and aqueous hydrochloric acid. Be sure to include physical states.

Consider the reaction below and select the appropriate response for each mixture of reactants that follows. RESPONSES: LR = limiting reactant, XSR = excess reactant or stoichiometric quantities

2Ag + S → Ag₂S

a) 100 g Ag + 100 g S
b) 4.0 mol Ag + 2.0 mol S
c) 400 g Ag + 50 g S
d)15 atoms Ag + 10 atoms S

1. What mass of water is produced from the complete combustion of 3.10×10−3 g of methane?

2. What mass of oxygen is needed for the complete combustion of 3.10×10⁻³ g of methane?

3. Set up two algebraic equations, one expressing the mass of carbon dioxide produced in terms of each reagent and the other expressing the mass of sample burned in terms of each reagent.

What is the mass of methyl alcohol (CH3OH) in the sample?

The SN2 Reaction can be described as chemospecicific; define the terms "chemoselectivity" and "chemospecificity", and explain the origin of the observed chemospecifity in the williamson ether synthesis

Questions regarding the lab: Spectrophotometric Determination of Caffeine in a Soft Drink

1)How are the absorption spectra of atoms and molecules the same, and how are they different?

2)Beer’s law, A=e b c forms the basis of a calibration curve. It clearly shows that there is a theoretically linear relationship between absorbance and concentration under constant conditions of analyte absorptivity (e) and path length (b). However, it is important for an analyst to be aware that there are limitations analyte concentration range under which there truly is a linear relationship between absorbance and concentration. Under what conditions of concentration does the linear relationship break down?

3)Caffeine is not fluorescent. However, just for argument’s sake imagine that it was fluorescent. Would the wavelength of maximum fluorescence be shorter, longer, or equal to the wavelength of maximum absorbance? Why?

4)Why was it necessary to remove CO2 before the analysis?

Determine the percent composition of air in the lungs from the following composition in partial pressures: PN2=565mmHg, PO2=108mmHg, PCO2=37mmHg, PH2O=50mmHg; all at 37∘C and 1atm pressure.

A % N2

B % O2

C %CO2

D % H2O

Two common ways for a chemist to increase the yield of a reactiom are described below. Explain why they increase the yield.
a. Add more of one of the reactants
b. Remove one of the products as it is being made.

QUESTION 1

Compute the typical thermal energy of a water molecule at normal conditions: (k_B T) and compare it to the answer to an earlier problem, where you computed the work needed to lift a molecule by a certain distance. Based on this comparison, the thickness of the Earth's atmosphere is about

QUESTION 2

How much energy is released after an Argon atom moving with speed 3.00 km/sec hits a brick wall and get adsorbed?

QUESTION 3

In the previous problem, what is the value of the collision energy in terms of k_BT, assuming the temperature was 95 ^oF at the time?

QUESTION 4

In equilibrium, the number of molecules moving in one direction is equal, on average, to the number of molecules moving in the opposite direction.

True

False

QUESTION 5

In equilibrium, all directions in space are equivalent in that the speeds of molecules moving in any given direction have the same distribution.

True

False

a) Determine the rate law.

b) Calculate the rate constant. Specify units.

c) Calculate the rate of reaction for experiment 5.

d) How is the rate of appearance of D related to the disappearance of B?

e) In experiment 3, what is the rate of disappearance of B?

9. The decomposition of N₂O₅is first order with a rate constant of 4.80 x 10^-4 s^-1at 45 ºC. If the initial concentration is

1.65 x 10^-2 M, what is the concentration after 825 s? What is the half life? How long would it take for the concentration of N₂O₅ to decrease to 1.00 x 10^-2 M from its initial value?

10. The following reaction has a K_c = 3.92 at 1200 Kelvin:     CO(g) + 3H₂(g) ⇌ CH₄(g) + H₂O(g)

At equilibrium, the reaction vessel contains 0.30 M CO , 0.10 M H₂ , and 0.020 M H₂O

Write the equilibrium constant expression. What is the [CH₄] at equilibrium? Calculate the K_p (for atm).

answers:

9. 0.0111 M, 24.1 min, 17.4 min

10. K_c = [CH₄][H₂O]         [CH₄] = 0.059 M     K_p = 4.04 x 10^-4

               [CO][H₂]