2) Suppose you are given a mixture of cobalt nitrate, magnesium sulfate, and naphthalene. After separating a 4.599g sample of the mixture you recover 2.535g of cobalt nitrate, 0.444g of magnesium sulfate, and 1.073g of naphthalene. a) What is the percent magnesium sulfate in the original mixture? b) What was your total percent recovery?

2) Suppose you are given a mixture of cobalt nitrate, magnesium sulfate, and naphthalene. After separating a 4.599g sample of the mixture you recover 2.535g of cobalt nitrate, 0.444g of magnesium sulfate, and 1.073g of naphthalene. a) What is the percent magnesium sulfate in the original mixture? b) What was your total percent recovery?

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

Section: Chapter Questions

Problem 40PS

See similar textbooks

Similar questions

Sulfuric acid, H2SO4, can be formed from the chemical reaction 2SO2+O2+H2O--->2H2SO4. Suppose 400g of SO2; 175g of O2, and 125 g H2O are mixed and the reaction proceeds until one of the reactants is used up. How many grams of H2SO4 is produced?A. 612gB. 620gC. 622gD. 630g
Octane, C8H18, can be used as a representative compound for gasoline.a. Is the combustion of octane a source or sink of a GHG? Explain.b. Write and balance the chemical equation for the combustion of octanec. Calculate the mass of carbon dioxide produced from the completecombustion of 1.0 gallon of gasoline, assuming the fuel is only octane.• Things to think about: How will you start this problem? Notice that youare not given grams initially, you are given 1.0 gallon. What conversionwill you use to get between gallons and grams? There are 3.785 litersin a gallon. Use 0.703 g/mL as the density of octane.
10 grams of methane and 10 grams of ethane are burned completely. Which will produce more carbon dioxide? Support your answer with calculations.
Why is the percent recovery of the essential oil less than 100%? State at least two reasons that are inherent to the experiment as performed and are thus unavoidable.
Each week CapeChem, a manufacturer of fine chemicals, uses up 300.kg of Compound A and 900.kg of Compound B in a reaction with only one product, Compound C . What is the maximum theoretical mass of Compound C that CapeChem could ship each week? Round your answer to the nearest kilogram. Suppose on average the percent yield of C in CapeChem's reactors is 93.% . Calculate the average amount of Compound C that CapeChem actually ships each week. Round your answer to the nearest kilogram.
The mystery fuel speedster! (Homework ) For fun, you build an explosive car with your little brother by attaching wheels to an empty windshield washer container. To advance it, you add 1.20 ml ( = 0.7915 g/ml) of a liquid but volatile fuel into the container. You close the cap and shake to evaporate the liquid. Finally, you place the car on its wheels, remove the cap and insert a burning wooden rod into the container. A flame suddenly comes out of the car, which is propelled with good speed in front of your little brother surprised, but all upset by the maneuver. The volatile fuel is composed of 37.5% carbon, 12.6% hydrogen and 49.9% oxygen. Its molar mass is approximately 32.0 g/mol. During the reaction, the fuel (gaseous) burns in the presence of gaseous oxygen, and the products of the reaction are carbon dioxide and water, gaseous too. The volume of the windshield washer container used is 4.00 litres. Useful Info: There is 21.0% gaseous oxygen in the air and initial conditions…
Calculate the percentage recovery and percentage using the data below 1)mass of lavender flower=45.65g 2)mass of the glass vial=15.19g 3)mass of lavender oil and the glass vial=16.61g 4)The theoretical yield of lavender oil from lavender flower =2.5%
Compare: Producing 350g of Al(NO3)3 required a greater amount of Ba(NO3)2 or Al2(SO4)3? How much more was needed?
Jennifer was a pre-pharmacy student and enrolled in general chemistry laboratory. One day the lab instructor asked Jennifer to identify a hydrate on the shelf labeled A, B, C, and D. They were possibly CaSO4 • 2H2O, CaCrO4 • 2H2O, AlCl3 • 6H2O, and ZnSO4 • 7H2O. Jennifer weighed 1.485 g of a hydrate. After heating/weighing three times, she finally obtained 0.820 g of the anhydrous compound. Jennifer concluded the hydrate was ZnSO4 • 7H2O. Was Jennifer’s finding correct? Why?
Butane, C4H10, burns to completion with 110% theoretical air.4.1) What is the actual air-fuel ratio on mass basis.4.2) What is the actual air-fuel ratio on mole basis. 4.3) What is theoretical air-fuel ratio (mass basis)4.4) What is theoretical air-fuel ratio (mole basis) 4.5 Determine the equivalence ratio.
In the synthesis of Hexyl Acetate, a student used 1.552 g of potassium acetate, 1.75 mL of 1-bromohexane, and 2.5 mL of DMF to obtain hexyl acetate. Show all work and include units in your calculations! Determine the theoretical yield for the student's experiment. The reaction is in the attached image.
Show work using conversion factors Answer Key:#37a CaCO3 + 2HCl --> CaCl2 + H2O + CO2 #37b 36.46 g/mol HCl #37c 100.09 g/mol CaCO3 #37d 1.250 moles CO2 #37e 4.92 mole HCl #37f 7.1422 moles HCl ( fixed 10/14/2020) #37g 143 g CO2