EQRYPfabASDFGHJKLcaps lockshiftCVNMoltfncontroloptioncommandMODULEScience 7in your notebook.Smulov csolution that is 2% boric acid?Im 02She sulVosmuloVnoulo2Given: Velu23.75 mLAsid:Jortoals Ivils im 0T aniein0o noulozailaloe io-guovamuloV2. What is the percent by volume of a 90mL solution that contains 25 mLMea to amulnmethanol?Jm 02 xIm 08 XLET'S PRACTICE!PRACTICE 1:C_1. Alcohol as disinfectant is normally sold as a solution of 70% ethyl orisopropyl alcohol. How much alcohol is present in a 100 mL solution?A. 30 mLB. 60 mL2. A beverage contains 3% alcohol which means thatC. 70 mLD. 75 mLA. The solution contains 30 mL of alcohol.B. The solution contains 30 mL water in 70 mL of water.C. The solution contains 3 mL of alcohol in 97 mL of water.D. The solution contains 300 mL of alcohol in 700 mL of water.-

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EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter13: Isolation Of Eugenol From Clov

Section: Chapter Questions

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Cocaine(C17H21O4N) is a natural substance found in the leaves of the coca plant, which has been used for centuries as a local anesthetic and stimulant. Illegal cocaine arrives in the USA either as a pure compound or as the hydrochloride salt(C7H21O4NHCl). At 25 degrees celsius, the salt is very soluble in water(2.59kg/L), but pure cocaine is much less so(1.70g/L) a. What is the maximum amount of salt in grams that can dissolve in 50.0mL of water? b. When a 25mL aqueous solution that contains 62.50 g of the salt is treated with NaOH, the salt is converted to pure cocaine. How much water in liters is needed additionally to dissolve the formed pure cocaine,
Would you help me whit this example (6) Thank you.
Write the empirical formula for the hydrated KAl(SO4)2, based on moles of anhydrous KSI(SO4)2= 0.046 mol molar mass of H2O= 18g/ mol moles of H2O= 0.0444mol ratio pf moles H20 to moles of anhydrous KAI(SO4)2= 9.65/1 . Show all work including units. Hint: if the ratio of moles of H2O to moles of anhydrous KAl(SO4)2 was 4, then the empirical formula would be: KAl(SO4)2•4H2O.
How do you cancel the units to get Δ‡S J/K*mol? If A has units of dm3/mol*s and KbT/h leaves me a remaining unit of 1/s
A major component of honey is fructose (C6H12O6) with a molar mass of 180.16 g/mol. A tablespoon (15.0 mL) of honey is considered one serving. How many tablespoons must be eaten to consume 0.1900 moles of fructose? Assume honey is 100% fructose. The density of honey is 1.45 g/mL.
ΔH° f (kJ/mol) SO 2Cl 2( g) + 2 H 2O( l) → 2 HCl( g) + H 2SO4( l) ΔH° rxn = ? SO 2Cl 2( g) -364H 2O( l) -286HCl( g) -192H 2SO 4( l) +314
Carbon dioxide emissions associated with a one-night stay in a hotel room are calculated at 28.98 kg of CO2 per room day for an average hotel. The 250 rooms of your hotel are all occupied for two days during a college football game. How much CO2 did the guests and hotel release into the atmosphere? Round your answer to the nearest whole number. kgs
Calculate ΔH orxnfor the following: CH4(g) + Cl2(g) → CCl4(l) + HCl(g)[unbalanced]ΔH o/f[CH4(g)] = −74.87 kJ/molΔH o/f[CCl4(g)] = −96.0 kJ/molΔH o/f[CCl4(l)] = −139 kJ/molΔH o/f[HCl(g)] = −92.31 kJ/molΔH o/f[HCl(aq)] = −167.46 kJ/molΔH o/f[Cl(g)] = 121.0 kJ/mol
C + 2 H2 ----> 1 CH4 What is molar ratio of C to H2 ?
a hydrated CuSO4 salt was heated and thus dehydrated. Determine the % H2O by weight in the hydrated CuSO4 salt. SHOW WORK TO RECEIVE FULL CREDIT mass of empty dish 43.571 gmass of dish + hydrated salt 44.326 gmass of dish + dehydrated salt 44.054 g 4. Using the data found in question number 3, determine the empirical formula for the hydrated CuSO4salt. What is the chemical name of this dehydrated salt? 5. Suppose that after your second heating, you were impatient and did not wait until your porcelain evaporating dish to cool. Instead, you weighed it while it was still hot. How would this specifically affect the calculated percentage of water in the compound?
3. Molly Cule weighed 8.61g of her hydrate (which is CaSO4*2H2O). After she did her hydrates lab, she found that her anhydrate weighed 6.81g. A) If Molly has not completely dried her samples before weighing her anhydrate, how would her final calculations of mole ratio of water to anhydrate be affected? B) How many moles of water were lost during the lab due to evaporation?
1-Pentanol to 1-bromopentane Chemicals: - 60ml Conc. Sulfuric Acid - 100ml Saturated Sodium bicarbonate - 65ml 1-Pentanol - 78g sodium bromide - Distilled water - 58.42g 1-Bromopentane 1-Pentanol Sodium Bromide Sulfuric Acid 1-Bromopentane Formula C5H12O NaBr H2SO4 C5H11Br MW (g/mol) 88.15 102.894 98.078 151.04 Density (g/mL) 0.811 3.21 1.84 1.218 Boiling point (*C) 138 1,396 337 130 NaBr(aq) + H2SO4(aq) -> NaHSO4(aq) + HBr(aq) CH3(CH2)4OH(aq) + H+ Br- (aq) CH3(CH2)4OH2 (aq) + Br-(aq) CH3(CH2)4OH2 (aq) + Br-(aq)  CH3(CH2)4Br(aq) + H2O(aq) How do I calculate the percent yield and identify the limiting reagent?

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