NH₂ImbruvicaABBVIE WINSPHARMACYCLICSPHARMACEUTICALS: $21 billiondeal helps firm become a leaderin treating blood cancersUST MONTHS AFTER abandoning its $54 bil-lion bid for specialty drug maker Shire, AbbVieis shelling out $21 billion for Sunnyvale, Calif.based Pharmacyclics. The purchase furthers AbbVie'sambitions in the field of hematological cancer and re-duces its reliance on one major product.The hefty price tag is the result of heated competi-tion. "I've been through a lot of these, and I'd say this isone of the most competitive ones I've seen." AbbVie'sCEO Richard A. Gonzalez said on a March 5 call withinvestors. Three companies were bidding against eachother until the bitter end, he said. Indeed, just hoursbefore the deal was announced, some media outlets reported that Johnson & Johnson had won out.Pharmacyclics's key asset is Imbruvica, a BTK inhibi-tor acquired in 2006 from Celera Genomics for just6$2 million and some equity. FDA approved Imbravicain late 2013 to treat mantle cell leukemia, and the drughas since won the agency's nod in three other bloodcancers. It is expected to bring in $1 billion in sales thisyear for Pharmacyclics and its marketing partner J&J.Imbruvica represents "a pipeline in a molecule,much like Humira did," Gonzalez said. AbbVie's Humi-ra is the world's top-selling drug, bringing in $12.5 bil-lion in sales last year across a range of inflammatorydiseases, but its patent is set to expire in late 2016.AbbVie believes its portion of peak sales for Imbruvicacould exceed $7 billion per year.The deal also advances AbbVie's goal of becom-ing a powerhouse in treating hematological cancer, amarket worth $24 billion in 2014. AbbVie sees syner-gies between Imbruvica and two small molecules in itspipeline: ABT-199, which blocks Bel-a and is in PhaseIl studies to treat acute myelogenous leukemia andduvelisib, a PI3K inhibitor in Phase II studies to treatseveral blood cancers.Last October, AbbVie walked away from the Shiredeal after a change in U.S. tax law. Gonzalez said thetwo deals are strategically "very different." Shire wasviewed as an avenue to lowering AbbVie's tax base,whereas Pharmacyclics complements its oncologyportfolio LISA JARVIS A) For what condition did the FDA approve this drug?B) How many aromatic rings does this drug contain?C) How many "true" lone pairs does this drug contain?D) How many aromatic pi electrons does this drug contain?

A ring is considered to be an aromatic if it is cyclic, planar, have delocalised pi electrons and…

A) For what condition did the FDA approve this drug? B) How many aromatic rings does this drug contain? C) How many "true" lone pairs does this drug contain? D) How many aromatic pi electrons does this drug contain?

A) For what condition did the FDA approve this drug? B) How many aromatic rings does this drug contain? C) How many "true" lone pairs does this drug contain? D) How many aromatic pi electrons does this drug contain?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 52E: Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00...

See similar textbooks

Similar questions

The reaction of solid calcium fluoride and sulfuric acid produces calcium sulfate solids and gaseous HF. The gas product is dissolved in water to form hydrofluoric acid. Fluorite ore, a source of calcium fluoride, contains 95%wt CaF2 and 5%wt SiO2. In a certain process, the ore is reacted with 93%wt aqueous sulfuric acid, supplied 15% in excess. From this, 95% of the ore dissolves in the acid. Some of the HF formed reacts with the dissolved silica in the reaction: HF reacts with SiO2 to produce H2SiF6 and liquid water. If 60%wt of hydrofluoric acid was formed when hydrogen fluoride (which exits the reactor) is dissolved in water, determine the amount of ore needed to produce one metric ton of acid. Report your answers to one decimal place only.
An aqueous solution of sucrose (C12H22O11) is prepared by dissolving 7.4045 g in sufficient deionized water to form a 100.00 mL solution. Calculate the molarity of the solution. Do you mind showing work? I would assume that (given) gram weight (times moles present/divided by mole(s) of compound) then divided - again by compound weight will give a percentage, then divded by the .....that's where I'm a little lost. thanks
What is the Molecular weight of a certain volatile liquid which is placed in 225 g flask which has total capacity volume of 252.17 mL. After the liquid was heated to 96.7 oC the gass volatilized and the weight of the flask measure 227.33g. What is the could be the MW of the volatile sample?
underecfectsol
One litre of a saturated aqueous solution of Ag2SO4 (MW = 311.79 g mol- 1) at 25 °C is evaporated to dryness. 4.844 g of Ag2SO4 residue was produced. What is the solubility product (Ksp)?
Magnesium +Acetic Acid --> C2HG5+ O2 ---> Iron (III) carbonate -->
The goal is to convince an investor to invest in your company so that you can build a factory to make ester compounds. For example, you could make hexyl pentanoate, and sell it for use in perfumes and make the investor money. You must come up with a compound that you can make and sell. You can use your textbooks and theinternet as resources. You can also access the link: https://jameskennedymonash.wordpress.com/2013/12/13/infographic-table-of-estersand-their-smells/ to look at an infographic of the ester compounds responsible for the smell of different fruits, perfumes and flowers. At the end of your research, you must have the compound table filled out
Acetaminophen, a popular drug taken as pain reliever and fever reducer, is produced together with acetic acid from the reaction of 3.05 g 4-aminophenol and 4.1 ml of acetic anhydride. Acetaminophen was extracted at 60% yield. Density of acetic anhydride at 20 C, 1.08 g/ml. Calculate the actual no. of grams of acetaminophen produced. [Determine L.R., E.R.]
(a) A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas City (MCI) to Baltimore (BWI) burned 11,800 lb (about 1700 gallons) of Jet A fuel en route. Jet A fuel is kerosine based, consisting primarily of CnH2n+2 hydrocarbons, with n =6 to 16, so the carbon:hydrogen ratio is close to 1:2. During this flight, how much CO2 was released into the atmosphere? Assume the combustion of the fuel was complete, so all the fuel was burned to form CO2 and H2O. Give both the mass of CO2 produced (in kg and in lbs) and the volume it would occupy at 298 K, 1 atm.(b) How much CO2 would be released into the atmosphere if those passengers and crew made the trip instead, in pairs, in hybrid cars at 40 miles per gallon. Assume the density of the gasoline is 0.75 kg L-1 and that carbon and hydrogen dominate the composition in a ratio of 1:2. The road trip is 1082 miles.
A pipet is used to transfer 5.00 mL of a 1.25 M stock solution in flask “S” to a 25.00-mL volumetric flask “A,” which is then diluted with DI H2O to the calibration mark. The solution is thoroughly mixed. Next, 2.00 mL of the solution in volumetric flask “A” is transferred by pipet to a 50.00-mL volumetric flask “B” and then diluted with DI H2O to the calibration mark. Calculate the molarity of the solution in volumetric flask “B.”
A 0.2500-g of dry CaCO3 was completely dissolved into a solution of 5-mL conc. HCl and 50-mL distilled water in an erlemeyer flask. The resulting solution was boiled for 5 minutes to expel CO2 from the reaction, and then it was cooled to room temperature and the solution was transferred in a 500-mL volumetric flask filled to volume by rinsing the erlenmeyer flask and combining all the washings to fill the mark. A 5.0-mL aliquot of the CaCl2 solution was taken from the orignal solution and was transferred into an erlenmeyer flask with 10-mL NH3 buffer, 20-mL distilled water, and 5 gtts of EBT. The solution consumed 4.96 mL of an EDTA solution. MW: CaCO3 = 100.1 Compute for the N EDTA solution. 0.0053 N 0.0531 N 0.5313 N None of the choices
Oceanic uptake of carbon dioxide is thus described:CO2 (g) + H2O ⇔ H2CO3, K = [H2CO3]/PCO2 = 3 x 10-2 M atm-1 H2CO3 ⇔ HCO3- + H+, K = [HCO3-][H+]/[H2CO3] = 9 x 10-7 moles/LHCO3- ⇔ CO32 - + H+, K = [CO32 -][H+]/[HCO3-] = 7 x 10-10 moles/LCharge balance equation:[H+] = [OH-] + [HCO3-] + 2[CO32 ] If the CO2 concentration in the atmosphere is 300 ppm, what is the pH of the ocean?