How many mL of MnSO4 would be produced in the following reaction if you started with 2.00 gH2C204, 2.00 g KMNO4 and 2.00 g H2SO4? Density of MNSO4 is 2.66 g/mL.H2C2O4(aq) + KMNO4(aq) + H2SO4(aq)CO2(g) + MnSO4(aq) + K2SO4(aq) + H2O)

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How many mL of MNSO4 would be produced in the following reaction if you started with 2.00 g H2C2O4, 2.00 g KMNO4 and 2.00 g H2SO4? Density of MNSO4 is 2.66 g/mL. H2C2O4(aq) + KMNO4(aq) + H2SO4(aq) CO2G) + MnS04(aq) + K2SO4(aq) + H2O0)

How many mL of MNSO4 would be produced in the following reaction if you started with 2.00 g H2C2O4, 2.00 g KMNO4 and 2.00 g H2SO4? Density of MNSO4 is 2.66 g/mL. H2C2O4(aq) + KMNO4(aq) + H2SO4(aq) CO2G) + MnS04(aq) + K2SO4(aq) + H2O0)

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

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section: Chapter Questions

Problem 90GQ: A Menthol, from oil of mint, has a characteristic odor. The compound contains only C, H, and O. If...

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An industrial-scale process for making acetylene consists of the following sequence of operations: CaCO3 → CaO + CO2limestone lime carbon dioxideCaO + 3 C → CaC2 + CO calcium carbide carbon monoxideCaC2 + 2 H2O → Ca(OH)2 + C2H2 calcium acetylene hydroxide What is the percentage yield of the overall process if 2.32 metric tons C2H2 is produced from 10.0 metric tons limestone (1 metric ton 5 1000 kg)?
One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III) hydroxide from a solution containing rhodium(III) sulfate according to the following balanced chemical equation: Rh2(SO4)3(aq) + 6NaOH(aq) → 2Rh(OH)3(s) + 3Na2SO4(aq) What is the theoretical yield of rhodium(III) hydroxide from the reaction of 0.500 g of rhodium(III) sulfate with 1.100 g of sodium hydroxide?
Aspirin (acetylsalicylic acid, C9H8O4) is made by reacting salicylic acid (C7H6O3) with acetic anhydride [(CH3CO)2O]: C7H6O3(s)+ (CH3CO)2O(l) → C9H8O4(s) + CH3COOH(l) In one preparation, 3.077 g of salicylic acid and 5.50 mL of acetic anhydride react to form 3.281 g of aspirin. (a) Which is the limiting reactant (d of acetic anhydride = 1.080 g/mL)? (b) What is the percent yield of this reaction? (c) What is the percent atom economy of this reaction?
50 mL of a 0.9 Ca3(PO4)2 solution is added to a beaker. How many moles of Ca3(PO4)2 were added? How many grams oF Ca3(PO4)2 were added?
1- Consider the reaction at room temperature of 6.7 g of a pure sample of bismuth (III) sulfide, which is reacted with 75 mL of 2.5 M nitric acid solution, forming elemental sulfur, nitrogen monoxide, nitrate bismuth(III) and water. Indicate which statement is correct: Alternatives: A. The limiting reagent is nitric acid, and 0.56 g of nitrogen monoxide is formed. B. The limiting reagent is bismuth(III) sulfide, and 0.29 L of nitrogen monoxide is formed under standard conditions of pressure and temperature. C. 0.39 g of nitrogen monoxide is formed and the excess reactant is nitric acid. D. The reactant in excess is nitric acid and 0.58 L of nitrogen monoxide is formed under standard conditions of pressure and temperature. E. The limiting reagent is bismuth(III) sulfide and 0.29 L of water is formed.
A mixture of BaO and CaO weighing 2.2120g is transformed into mixed sulfates, BaSO4 and CaSO4 weighing 5.0230g. Calculate the number of grams CaO and BaO in the mixture. What weight of limestone should be taken so that 1/20 the number of mg of CaSO4 obtained will represent the percentage of CaO in the numeral?
A Menthol, from oil of mint, has a characteristic odor. The compound contains only C, H, and O. If 95.6 mg of menthol burns completely in O2, and gives 269 mg of CO2 and 111 mg of H2O, what is the empirical formula of menthol?
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
A chemical plant uses electrical energy to decompose aqueous solutions of NaClNaCl to give Cl2Cl2, H2H2, and NaOHNaOH: 2NaCl(aq)+2H2O(l)→2NaOH(aq)+H2(g)+Cl2(g)2NaCl(��)+2H2O(�)→2NaOH(��)+H2(�)+Cl2(�) Part A If the plant produces 1.9×106 kg1.9×106 kg (1900 metric tons) of Cl2Cl2 daily, estimate the quantities of H2H2 produced. Express your answer using two significant figures.
After the experiment, a student decides to dispose of their excess Mg safely by reacting it with acetic acid. If the student had 0.60 g of excess Mg metal, how many mL of 0.83 M acetic acid (HC2H3O2)are required to fully react with the metal? Assume the reaction proceeds as below, and give your answer to 2 decimal places. Mg (s) + 2HC2H3O2 (aq) -> H2 (g) + Mg(C2H3O2)2 (aq)
One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III) hydroxide from a solution containing rhodium(III) sulfate according to the following unbalanced chemical equation: Rh2(SO4)3(aq) + NaOH(aq) → Rh(OH)3(s) + Na2SO4(aq) If 3.10 g of rhodium(III) sulfate reacts with 5.90g of sodium hydroxide a. Determine the limiting reactant. b. Determine the excess reactant. c. What mass of rhodium (III) Hydroxide may be produced d. Calculate the percent yield if 1.3 g of rhodium (III) Hydroxideare actually obtained. MM of Rh2(SO4)3(aq) = 494g/mol MM of NaOH = 40g/mol) MM of Rh(OH)3(s) = 153.93g/mol
Cryolite (Na3AlF6) is used in the commercial production of aluminum from ore. Cryolite itself is produced by the following reaction: 6 NaOH + Al2O3 + 12 HF → 2 Na3AlF6 + 9 H2O A mixture containing 420.0 kg of NaOH, 128.4 kg of Al2O3, and 600.0 kg of HF is heated to 950 °C until it reacts to completion. What is the maximum mass of Na3AlF6 formed? ________kg Na3AlF6

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