1. A laboratory method of preparing O2(g) involvesthe decomposition of KCIO3(s).2KCIO3(s) 2KCI(s) + 302(g)(a) How many moles of O2(g) Ccan be produced bythe decomposition of 34.6 g KCIO3?(b) How many grams of KCIO3 must decompose toproduce 45.5 g O2?(c) How many grams of KCI are formed, togetherwith 27.5 g O2, in the decomposition of KCIO3?

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Answered: 1. A laboratory method of preparing…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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6.24 Ethanol, used in alcoholic beverages, can be produced by the fermentation of sucrose, which is found in sugar cane and other plants. The balanced equation for the fermentation process is C12H„0,(s) + H,0(1) – (a) What mass of ethanol, C,H,OH, would be produced when 2.50 g sucrose reacts by this process? (b) What mass of CO, would also be produced? 4C,H,OH() + 4CO,(g)
In a reaction to produce NaF, 3.50 g of HF and 1.26 of Na2SiO3 are reacted according to the following: Na2SiO3 (s) + HF (aq) →H2SiF6 (aq) + NaF (aq) + H2O (l) (a) Balance the equation. (b) Calculate the theoretical yield of NaF. (c) If 0.792 g of NaF is formed, calculate the percent yield.
How many grams of C are required to react with 44.3 g Fe2O3?Given Fe2O3(s)+3C(s)→2Fe(s)+3CO(g)?
2. In the laboratory, O2(g) can be obtained from the following thermal decomposition reaction of potassium chlorate (KCIO3) with the aid of catalyst: A, MnO2 (catalyst) 2KC1O;(s) > 2KCI(s) + 302(g) To determine the composition of the mixture of KCIO3 and potassium chloride (KCI), 0.612 g KCIO3/KCl mixture is taken into a test tube and heated in the presence of sufficient catalyst, MnO2. The total mass of the test tube after heating decreased by 0.096 g. According to this result, what is the percentage of the KCIO3 in the mixture? (K: 39.0 g/mol, Cl: 35.5 g/mol, O: 16.0 g/mol)
The mineral galena is composed of lead(II) sulfide and hasan average density of 7.46 g/cm³. (a) How many moles oflead(II) sulfide are in 1.00 ft³of galena? (b) How many leadatoms are in 1.00 dm³of galena?
The molecular formula of allicin, the compound responsible for the characteristic smell of garlic, is CgH10OS2. (a) What is the molar mass of allicin? g/mol (b) How many moles of allicin are present in 4.60 mg of this substance? mol (c) How many molecules of allicin are in 4.60 mg of this substance? allicin molecules (d) How many O atoms are present in 4.60 mg of allicin? O atoms
0 3.76 Consider the mixture of propane, C,Hg, and O2 shown below. (a) Write a balanced equation for the combustion reaction that Occurs between propane and oxygen. (b) Which reactant is the limiting reactant? (c) How many molecules of CO, H2O, C;Hs, and O, will be present if the reaction goes to completion?
For the equation:4 Fe(CrO2)2 + 8 K2CO3 + 7 O2 ----> 2 Fe2O3 + 8 K2CrO4 + 8 CO2 (a) The number of grams of Fe(CrO2)2 required to produce 4.00 grams of K2CrO4. (b) What is the percent yield of Fe2O3 if 2.90 g of Fe2O3 are formed from reaction of 10.0g of Fe(CrO2)2?
For the following reaction, 3.65 grams of hydrogen gas are mixed with excess nitrogen gas. The reaction yields 16.8 grams of ammonia. N2 (g) + 3H2 - 2NH3 (g) (1) What is the theoretical yield of ammonia?| grams (2) What is the percent yield for this reaction?
Complete combustion of propane (C3H8) produces carbon dioxide and water as products. C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(g) Incomplete combustion produces some carbon monoxide (CO) in place of carbon dioxide (CO2). What is the limiting reactant for incomplete combustion? (A) There is no way to tell (B) Water (C) Propane (D) Oxygen
Ammonium phosphate fertilizer is prepared by the following reaction:3 NH3(g) + H3PO4(aq) ->(NH4)3PO4(s)(a) How many grams of ammonia and phosphoric acid, respectively, are required to produce 1.00 kg of ammonium phosphate, (NH4)3PO4, if the reaction has 100% yield?(b) How many grams of ammonia and phosphoric acid, respectively, are required to produce 1.00 kg of ammonium phosphate, (NH4)3PO4, if the reaction has 85.0% yield?
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