How many grams of KCIO, are needed to form 20.5 g of O2?2 KC103(3) 2KCI(s) + 30,(g)Step 1: Sbow the strategy for solving this problem.grams O, -- grams KCIO,Answer Bankgrams KCIO,males KCIO3grams KCIImoles Ongrams Omoles KCIStep 2: Show the conversions required to solve this problem and calculate the grams of KCIO3.20.5 g 02X= 8 KC10,Answer Bank122.55 g KCIO,I mole KCIO32 moles KCI0,32.00 g O2I mole O,3 males O274.55 g KCII mole KCI2 moles KCIgrams of KCIO3:g KCIO, How many grams of Ni are formed from 59.7 g of Ni-O,?2 NiOz(s) 4Ni(s) + 30-(g)Step 1: Sbow the strategy for solving this problem.grams NiO3 -grams NiAnswer Bankgrams Nimoles Nimoles Niz03males O2grams Niz03grams O,Step 2: Sbow the conversions required to solve this problem and calculate the grams of Ni.59.7 g Niz03 X= g NiAnswer Bank165.38 g NiO31 mole NiO2 males Ni,0332.00 g O21 mole O23 moles On58.69 g Ni1 mole Ni4 males Nigrams of Nig Ni

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Answered: How many grams of KCIO, are needed to…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter11: Stoichiometry

Section: Chapter Questions

Problem 50A

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Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
or each of the following reactions, give the balanced chemical equation for the reaction and state the meaning of the equation in terms of individual molecules and in terms of moles of molecules. msp;MnO2(s)+Al(s)Mn(s)+Al2O3(s) msp;B2O3(s)+CaF2(s)BF3(g)+CaO(s) msp;NO2(g)+H2O(l)HNO3(aq)+NO(g) msp;C6H2(g)+H2C6(g)H12(g)
For each of the following unbalanced reactions, suppose exactly 5.00 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will remain after the limiting reactant is consumed. Na2B4O7(s) + H2SO4(o H3BOj(j) + Na2SO4(u CaC,(s) + H2O(/) Ca(OH)2(s) + C2H2(g) NaCl(s) + H2SO4(/> HCl(g) + Na2SO4(s) SiO2(s) + C(x) —> Si(/) + CO(g)
For each of the following balanced equations, indicate how many moles of the product could be produced by complete reaction of 1.00 g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. msp;NH3(g)+HCl(g)NH4Cl(s) msp;CaO(s)+CO2(g)CaCO3(s) msp;4Na(s)+O2(g)2Na2O(s) msp;2P(s)+3Cl2(g)2PCl3(l)
Air Pollution Nitrogen monoxide, which is present in urban air pollution, immediately Converts to nitrogen dioxide as it reacts with oxygen. a. Write the balanced chemical equation for the formation of nitrogen dioxide from nitrogen monoxide. b. What mole ratio would you use to convert from moles of nitrogen monoxide to moles of nitrogen dioxide?
A 0.20 mol sample of magnesium burns in air to form 0.20 mol of solid MgO. What amount (moles) of oxygen (O2) is required for a complete reaction?
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
Consider the following generic reaction: Y2+2XY2XY2 In a limiting reactant problem, a certain quantity of each reactant is given and you are usually asked to calculate the mass of product formed. If 10.0 g of Y2 is reacted with 10.0 g of XY, outline two methods you could use to determine which reactant is limiting (runs out first) and thus determines the mass of product formed.
When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?

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