1. When 5.45 grams of aluminum chlorate (Al(CIO;); decompose, 1.57 liters of oxygen gas are given off. What is the percent yield? Al(CIO;); AICI; + O2
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A: • The given unbalanced chemical equation is, Mg + HCl → MgCl2 + H2
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A: Calculation of number of moles of the two reactants given is shown below.
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A: Percent yield = (Practical yield/theoretical yield)×100
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A: number of moles = mass/molar mass mass = moles × molar mass percent yield ={actual…
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A: Given: The thickness of Al foil=0.550 mm 1 cm =10 mm 0.550 mm ×1 cm10 mm =0.055 cm Volume =1.00 cm2…
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A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…
Q: Methanol (CH3OH) is a liquid at room temperature with a density of 7.91 *10² kg/m³. In a certain…
A: Methanol has a variety of uses as a fuel, laboratory reagent, solvent, etc. In the given reaction,…
Q: Methanol (CH3OH) is a liquid at room temperature with a density of 7.91 x102 kg/m³. In a certain…
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Q: by the reaction of hydrochloric acid with manganese(IV) oxide. HCl(aq) + MnO,(s) - MnCl, (aq) + 2…
A: 4HCl (aq) + MnO2(s) ----> MnCl2(aq) + 2H2O (l) + Cl2(g) Mass of HCl = 44.1 g Mass of MnO2 = 43.7…
Q: Methanol (CH3OH) is a liquid at room temperature with a density of 7.91 x102 kg/m³. In a certain…
A: The type of chemical reaction that occurs between methanol and oxygen is a combustion reaction in…
Q: In a combination reaction, 2.22 g of magnesium is heatedwith 3.75 g of nitrogen. (a) Which reactant…
A: Given : Mass of magnesium taken = 2.22 g And mass of nitrogen taken = 3.75 g Atomic mass of…
Q: Methanol (CH3OH) is a liquid at room temperature with a density of 7.91 ×10² kg/m³. In a certain…
A: (a) It is a combustion reaction. (b) Micropipette can be used to measure the volume of methanol.
Q: How many grams of fluorine (F,) are required to produce 264.0 g of CoF,?
A: Since you have posted multiple questions, we are entitled to answer the first only. Please repost…
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A: Hey since you have posted a sub-part question we would answer first three sub-parts only. If you…
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A: Given Mass of Ca(OH)2 = 0.65 gram Molar mass of Ca(OH)2 = 40 + ( 2×17 ) gm/mole…
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A: Given that - Moles of aluminum, Al = 3 mole Volume of KOH used K=39, Al-27, S-32, H=1= 25 mL…
Q: A sample weighing 3.056 g is a mixture of Fe, O, (molar mass = 159.69 g/mol) and Al, O, (molar mass…
A:
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A: A+B→C+Dit means 1 mole of A require 1mole of B
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A: 1) C2H2(g) + O2(g) =CO2(g) +H2O(g) 2)C2H2(g) + 5/2O2(g) =2uCO2(g) +H2O(g)
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A: The given data contains, Moles of C5H12 = 6.58 moles.
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- Souring of wine occurs when ethanol is converted to acetic acid by oxygen: C2H5OH(l) +O2(g)--->CH3COOH(g)+H2O(l). A 1.00 L bottle of wine labeled as 7.00% (%v/v) ethanol, is found to have a defective seal. Analysis of 1.00 mL showed that there were 0.0274 g acetic acid in that 1.00 mL. The density of ethanol is 0.816 g/mL. (a) What mass of oxygen must leaked into the bottle in pounds(lb) (b) What is the percent yield for the conversion of ethanol to acetic acid, if oxygen is in excess7. Consider a1Msolution ofNa3AsO4. Write the charge and mass balance equations for this system. (please type answer not write by hend)A weight of 0.50 g was taken impure container containing sodium carbonate and bicarbonate. Dissolved in water and then crushed with hydrochloric acid (0.1 N), the burette reading game was at the endpoint of phenolphthalein of 10.5 ml and at the end point of the orange methylation point 30.1 ml. The percentage of sodium carbonate was in ................. knowing that the weights are: Na: 23, C: 12, O: 16
- Use your balanced chemical reaction from the above problem. How many kilograms of the barium product can be produced at 100% yield from the double replacement reaction, made in industry at a larger scale of 675.00 pounds of barium nitrate that is then dissolved in water and mixed with an excess of the potassium sulfate solution. The product is collected by gravimetric filtration and dried. Use 453.592 g = 1 lb. Ba(NO3)2 + K2SO4 ---> BaSO4 + 2KNO3A chemist dissolved 0.08346g of SrCl2 (FW 158.53) and treated it with excess AgNO3 (FW 169.87) to precipitate 0.143g of AgCl (FW 143.32). In his time, the atomic mass of Ag was known to be 107.8 and that of Cl was 35.4 From these values, find the atoimic mass of Sr that the chemist would have calculated.Give typed full explanation After heating 1.1929g CaCO3 and MgCO3 for some minutes the mass of the mixture decreased to 0.8015. The %comp of CaCO3 turned out to be 54.29% and MgCO3 %comp is 45.71%. Calculate the percent error/percent yield.
- In the synthesis of benzoic acid, 3.5 mL of toluene were used and mixed with potassium permanganate solution. In making the potassium permanganate solution, 7 grams of the powder were dissolved in 150 mL of water. The resulting crystals were purified and the yield 1.53 grams. Identify the limiting reagent and compute for the number of moles that it consumed. What is the theoretical yield? What is the percentage yield? MW toluene = 94.14, density=0.87 g/mL , MW KMnO4 = 158, density = 2.7 g/mL , MW Benzoic acid = 122, density = 1.27 g/mLA (3.6500 g) of impure ammonium aluminium sulfate (NH4Al(SO4)2)) was treated with ammonia (NH3(aq)) producing hydrous alumina Al2O3.xH2O. The collected precipitate was filtered, washed, and ignited at 1000 °C to give 0.4935 g Al2O3 (Mw 101.9635 g/mol). Determine: a. % Al2O3 b. %Al c. Express concentration of Al in ppm.Mo in a 0.2711g sample was precipitated giving 1.1682g of (NH4)2PO4.12 MoO3. Find the percentage Mo , P (at wt = 30.97), N=14,Mo=95.9,H=1,O=16
- Use the following atomic masses (in g/mol):Mg = 24.31; O = 16; Ca = 40.08; C = 12.01; Na = 23; H = 1; N = 14.01; S = 32.06; Cl = 35.45; 2.) Limestone consists chiefly of mineral calcite (CaCO3). The carbonate content of 0.5413g of powdered limestone was measured by suspending the powder in water, adding 10mL of 1.392M HCl and heating to dissolve the solid and expel CO2. The excess acid required 39.96mL of 0.1004M NaOH for complete titration to a phenolphthalein end point. Find the % wt of calcite in limestone.An impure sample of Na3PO3 weighing 0.1 g is dissolved in 35 mL of water. A solution containing 45 mL of 3% w/v HgCl2, 30 mL of 10% w/v sodium acetate, and 10 mL of glacial acetic acid is then prepared. After digesting, filtering, and rinsing the precipitate, 0.2857 g of Hg2Cl2 is obtained. Report the purity of the original sample as % w/w Na3PO3.The water in Fell city also contains 30 μg/L of chloroform (formed in the water treatment plant), 5 μg/L of chlorpyriphos (a persticide), and 10 μg/L of chromium VI. Given the reference doses below, calculate the total hazard quotient. State which compound is the total HQ is acceptable. References doses (all mg/kg.d): 0.01 for chloroform, 0.0003 for chlorpyiphos, and 0.003 for chromium VI. Answer: 0.66