A mixture of KCIO3 and KCl with a mass of 0.950 g was heated to produce 02. After heating, the mass of residue was 0.840 g. Assuming all the KCIO3 decomposed to KCl and O₂, calculate the mass percent of KCIO3 in the original mixture. % KC103 M W 7 3 e d C % Sin $ 4 I 5 t D.O 6 hp y Ili & 7 h u 8 j 9 k

A mixture of KCIO3 and KCl with a mass of 0.950 g was heated to produce 02. After heating, the mass of residue was 0.840 g. Assuming all the KCIO3 decomposed to KCl and O₂, calculate the mass percent of KCIO3 in the original mixture. % KC103 M W 7 3 e d C % Sin $ 4 I 5 t D.O 6 hp y Ili & 7 h u 8 j 9 k

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter3: Equation, The Mole, And Chemical Formulas

Section: Chapter Questions

Problem 3.85QE: A chemist prepared a compound that she thought had the formula FeI3. When the compound was analyzed,...

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A chemist prepared a compound that she thought had the formula FeI3. When the compound was analyzed, it contained 18.0% Fe and 82.0% I. Calculate the mass percentage composition expected for FeI3 and compare the result with that found in the analysis. Is this the correct formula of the compound?
The phosphorus in a 0.2091-g sample was precipitated as the slightly soluble (NH4)3PO4 • 12 MoO3. This precipitate was filtered, washed, and then redissolved in acid. Treatment of the resulting solution with an excess of Pb2+ resulted in the formation of 0.2922 g of PbMoO4. Express the results of this analysis in terms of percent P2O5.
In the common process for the manufacture of nitric acid, sodium nitrate is treated with aq. sulphuric acid containing 95% H2SO4. In order that the resulting "niter cake" may be fluid; it is desirable to use sufficient acid so that there will be 34% H2SO4 by wt in the final cake. This excess H2SO4 will actually be in combination with the Na2SO4 in the cake, forming NaHSO4, although for purposes of computation it may be assumed to be free acid. The cake will contain 1.5% water and the reaction will go to completion, but 2% of the HNO3 formed will remain in the cake. Assume that the NaNO3 used is dry and pure. Calculate per 100 kg of NaNO3 charged: (a) wt and % composition of the niter cake (b) wt of aqueous acid to be used (c) wt of water vapor and nitric acid distilled from the niter cake.
The mercury in a 1.1113-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5Hg2+ + 2H5IO6 → Hg5(IO6)2 + 10H+ The precipitate was filtered, washed free of precipitating agent, dried, and weighed, and 0.4733 g was recovered. Calculate the percentage of Hg2Cl2 in the sample. _______%
43. In the preparation of Rochelle salt (MW = 282.83 g/mol), 7.2 grams of monohydrated Sodium carbonate (MW = 124.01 g/mol) dissolved in 80 mL water was made to react with 20g of Potassium bitartrate (MW = 188.10 g/mol). What is the amount of Rochelle salt obtained from Monohydrated Sodium carbonate? Rochelle's Salt:2 KHC4H4O6 + Na2CO3.H2O + 6 H2O -> 2 KNaC4H4O6.4H2O + CO2 ↑ a 38.77 g b 28.74 g c 36.48 g d 32.84 g
The aluminum in a 2.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous ‍‍Al2O3⋅xH2O. The precipitate was filtered and ignited at 1000°C to give anhydrous Al2O3, which weighed 0.3006 g. Express the result of this analysis in terms of a. %NH4Al(SO4)2 b. %Al2O3 c. %Al
another question The aluminum in a 1.200g sample of impure ammonium aluminum sulfate was precipitatedwith aqueous ammonia as the hydrous Al2O3 · XH2O. The precipitate was filtered and ignitedat 100°C to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysisin terms of % Al.
The phosphorus in a 0.2222-g sample was precipitated as the slightly soluble (NH4)3PO4 • 12Mo O3. This precipitate was filtered, washed, and then redissolved in acid, Treatment of the resulting solution with an excess of Pb2+ resulted in the formation of 0.2922 g of PbMo O4. Express the results of this analysis in terms of percent P₂O5. _______ %
A 0.6447 g portion of manganese dioxide was added to an acidic solution in which 1.1402 g of a chloride containing sample was dissolved. Evolution of chlorine took place as a consequence of the following reaction: MnO2(s) + 2Cl- + 4H+ ® Mn2+ + Cl2(g) + 2H2O After the reaction was complete, the excess MnO2 was collected by filtration, washed, and weighed, and 0.3521 g was recovered. Express the results of this analysis in terms of percent aluminum chloride. (Al:27.0 ; Mn:55.0 ; O:16.0 ; Cl:35.5 ; H:1.0 g/mol)
Sample: Saline 0.900% (m/v), in sodium chloride (NaCl). Data: M.A. (g/mol): Na = 22.9898; K = 39.0983; Cr=51.9961; Ag = 107.8682; Cl = 35.453; N=14.0067; O = 15.9994. Material available in the laboratory's warehouse: Reagents: distilled water; standardized solution of silver nitrate (AgNO₃), at a concentration of 0.09980 mols/L; Potassium chromate solution (K₂CrO₄) 1%; ammoniacal ferric alum solution [Fe(NH₄)(SO₄)₂] and; nitrobenzene (or cooking oil, alternatively); 0.1000 mols/L potassium thiocyanate (KSCN) standard solution. Glassware: beakers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyers; 10.00 and 25.00 mL volumetric pipettes; 15.00 mL burette; 30.00, 50.00 and 100.00 mL volumetric flasks Calculate the molarity of saline, in terms of the NaCl concentration (concentration in mols/L). (a) 0.900 mols/L (b) 5.84 mols/L (c) 0.154 mols/L (d) 0.0154 mols/L
A 1.00 g mixture of H2O and D2O was electrolyzed producing H2(g), D2(g) and O2(g). The H2(g) and D2(g) were then completely reacted with Cl2(g) to produce HCl(g) and DCl(g). The HCl(g) and DCl(g) was then dissolved in 1.000 L of water. Then, a 25.00 mL portion of that 1.000 L solution was reacted completely with AgNO3(aq) to give 0.3800 g of AgCl(s). Calculate the mass % (%w/w) of D2O in the original 1.000 g mixture.
A 1.00 g mixture of H2O and D2O was electrolyzed producing H2(g), D2(g) and O2(g). The H2(g) and D2(g) were then completely reacted with Cl2(g) to produce HCl(g) and DCl(g). The HCl(g) and DCl(g) was then dissolved in 1.000 L of water. Then, a 25.00 mL portion of that 1.000 L solution was reacted completely with AgNO3(aq) to give 0.3800 g of AgCl(s). Calculate the mass % (%w/w) of D2O in the original 1.000 g mixture. Atomic Masses (g/mol): H = 1.008, D = 2.014, O = 16.00, Cl = 35.45, Ag = 107.9