O Mass-Mass Stoich-$1 doc Scurses/216161/files/236134137wrap31Met-GUY, KLE L on> Files > Mass-Mass Stoich -s-1.doc-Mass Stoich -s-1.docd Mass-Mass Stoich -s-1.doc (31 KB)700M3.BALANCE the following equation:KCIO3-------> KCl + O,gramsmole of KCIO,?a) How many grams of KCl are produced from 250b) How many grams of KCIO, are needed to produce 15 grams mole of O;?

rom 702 3. BALANCE the following equation: KCIO3 -------> KCI + O, a) How many grams of KCl are produced from 250 grams mole of KCIO;? b) How many grams of KCIO; are needed to produce 15 grams mole of O,?

rom 702 3. BALANCE the following equation: KCIO3 -------> KCI + O, a) How many grams of KCl are produced from 250 grams mole of KCIO;? b) How many grams of KCIO; are needed to produce 15 grams mole of O,?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter11: Solving Equilibrium Problems For Complex Systems

Section: Chapter Questions

Problem 11.3QAP

See similar textbooks

Related questions

Q: Which chemical equation below is balanced? EQUATION A: 2H2(g) + O2(g) ----> 2H2O(g) EQUATION…

A: In a chemical equation, reactants are present on left side and products are present on right side of…

Q: f, in the above reaction 5.0 gram of N2 is reacted with 1.0 gram of H2, which reagent is limiting?…

A: Limiting reagent: The limiting reagent in a chemical reaction is a reactant that is totally consumed…

Q: The reaction between A (one large red sphere) and B (one small blue sphere) to produce AB, is shown…

A: Limiting reactant reactant that completely consumed during reaction.

Q: when burned MgCO3 give MgO and CO2, If 16 g of a mixture of MgCO3 and MgO was completely burned, the…

A: Given : mass of mixture = 16 gm Mass of remaining solid = 11.6 gm

Q: Identify 2 things that could happen during an experiment to cause tthe actual yeild to be lower than…

A: Theoretical yield is the maximum amount of product which can be formed in a reaction. Actual yield…

Q: & When 15.00 g of KCIO: is heated it decomposes. Give the percentage yield 3.09 g of Ois produced at…

A: Mass of KClO3 = 15.00 g Actual yield of O2 = 3.69 g Molar mass of KClO3 = 122.55 g/mol

Q: How many grams of O2 can be prepared from the thermal de composition of 4.27 kg of HgO? Name and…

A: Balance chemical equation: 2 HgO (s) --------> 2 Hg (l) + O2 (g) Moles of HgO = given…

Q: Give a clear handwritten answer....?

Q: 2 KČIO, 2 KCI + 3 02 Calculate how many grams of 0,(g) can be produced from heating 81.9 g KC1O,(s).

Q: If 5.6 moles CU are reacted with 7.2 moles of AgNO3 according to the balanced equation below. Cu(s)…

Q: A sample of nickel ore, which has nickel as the only metal present, is treated with an excessnof…

A: a) Please find below the balanced reaction Ni + H2SO4 ----> NiSO4 + H2

Q: Is each of the following statements true or false? Correctany that are false:(a) A mole of one…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Aluminum oxidizes according to the following equation: Al + O2 -----> Al2O3 a. Powdered Al…

Q: How many grams of sodium sulfide are formed if 1.80 g of hydrogen sulfide is bubbled into a solution…

A: A numerical problem based on mole concept, which is to be accomplished.

Q: A 39.59 sample Of copper B heated in the presence of excess Oxygen and is converted to copper l11)…

A: Given, mass of copper sample = 39.5 g Mass of copper (II) oxide formed = 45.5 g Molar mass of Copper…

Q: 5. Calculate the mass of Fe(OH)3 that can be produced by the reaction of 35 g NaOH with FeCl: (used…

Q: elow is a balanced equation of a combustion reaction: C;Hg + 502 - 3CO2 + 4H20 1 mol H,0 4 mol C,H,…

A: Mole ratio is the ratio is the ratio between the amounts in moles of any two compounds involved in a…

Q: n the reaction of 10.00 mL of FeCl3{aq) and 12.4 g of <½C2O4laq). you calculate that 9.58 g of…

A: Volume of FeCl3 = 10.00 mL Mass of K2C2O4 : 12.4 g Mass of K3FeC2O43H2O = 9.58 g

Q: For the following reaction, 4.74 grams of butane (C,H10) are allowed xygen gas. putane (C,H10)(g) +…

Q: 3. Balance the equation below then use it to answer the following questions. a. Balance the…

A: a) In the Balance chemical equation, the no of elements of each type on reactant and product side…

Q: How to calculate theoretical and percent yield. My values are: .152 g magnesium turnings, 1.10 g of…

A: First we find mass of main reactant 1. Bromobenzene: 157.01g/mol (Main reactant) 2. Benzoic acid:…

Q: ??(??)3+?2??4⟶?Al(OH)3+H2SO4⟶? How many grams of Al(OH)3 are required to completely convert 29.552…

A: Given that mass of H2SO4 = 29.552 g The molar mass of H2SO4 is 98.08 g/mol The incomplete equation…

Q: How much methanol (CH3OH, in grams) can be formed from 60.2 kg of hydrogen? Assume excess CO.…

Q: Balance the following reaction: _____??2?3 + _____?? → _____?? + _____??2?3 Using the balanced…

A: The balanced reaction taking place is given as, => Fe2O3 + 2 Al → 2 Fe + Al2O3 Given: Mass of Al…

Q: Consider titanium. It is a metal with the same strength as steel but it is 45% lighter. It is also…

A: Mole is the amount of the substance that contains the same number of particles or atoms or…

Q: Balance the following equation KCIO3----> KCI+O2 a) how many grams of KCI are produced from 250…

Q: Consider the follarina unbalanced equation: Caz POA),S)+H, SO4 @e>CaSO45)+H; PO4 @c) What masses of…

A: The given unbalanced equation is: Ca3(PO4)2 + H2SO4 -----> CaSO4(s) + H3PO4 Balancing the…

Q: Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and…

A: The reaction taking place is given as, => CaF2 + H2SO4 --------> CaSO4 + HF Given : Mass of…

Q: or the combustion reaction of the moled 2H2 that produces carbon dioxide and vater? O C2H4 + O2 →…

A: The question is based on the concept of chemical reactions. we have to identify the correct reaction…

Q: When reacting Na with Cl, we calculated that the theoretical yield should be 12.5 grams. Our actual…

A: Theoretical Yield = 12.5 g Actual Yield = 9.3 g THEORETICAL YIELD It is the calculated mass of the…

Q: 9. Aluminum chloride AICIB is on ieerpunsive reagent used in many industrial processes It by…

A: According to the question, Aluminium metal reacts with chlorine gas to produce AlCl3 (Aluminium…

Q: C10H8 O2 _CO2 H2O. + -- How many grams of H20 is produced from the reaction of 61.49 g C10H8 ? Hint:…

Q: In the reaction, A + B→C + D, if element B is in excess, then: O both A & B are limiting reactants.…

A: A+B→C+Dit means 1 mole of A require 1mole of B

Q: c) Acetylene, C,H, is the fuel used for welding. i) Write the skeleton equation for the combustion…

A: 1) C2H2(g) + O2(g) =CO2(g) +H2O(g) 2)C2H2(g) + 5/2O2(g) =2uCO2(g) +H2O(g)

Q: Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum…

A: The reaction between MnO2 and Al –metal is shown as: Here, MnO2 and Al react in 3:4 ratio. Given…

Q: Glucose CH2O reacts with oxygen to give CO, and H,0. What mass of the oxygen (in grams) is required…

Q: * 00 0.0 When glucose (C 6H1206) reacts with molecular oxygen, Gaseous carbon dioxide and liquid…

A: Given, The combustion of glucose(C6H12O6) with molecular oxygen to form gaseous carbon dioxide and…

Q: In an experiment, 0.50 g C,H4 (molar mass: 28 g/mol) reacts with 2.30 g O2 (molar mass: 32 g/mol)…

A: Given :- Mass of C2H4 = 0.50 g Mass of O2 = 2.30 g Mass of CO2 = 1.25 g (actual yield) To be…

Q: nagnesium.s)+ hydrochloric acid, ant o maghesium chloridecant Mgrss + 2HCI, aa MgClz Cas) m-0.24g -…

A: We have to predict the limiting reactant, excess reactant and mass of gas Produced.

Q: Determine the limiting reactant for the reaction. no limting reactant O AB2 O B2 O A,

Q: emical stoichiometry, determine the number of moles of carbonic acid that can be p 主 ponie acid: he…

A: Balanced chemical reaction NaHCO3 + HCl ---> NaCl + H2CO3 limiting reagent = NaHCO3 moles of…

Q: 7. For the reaction C5H12+ O2 → H20 + CO2, if one starts w a) moles g and mass g of CsH12 b) moles g…

Q: The balanced equation for combustion C2H5OH(I) + 302(g) ----- 2CO2(g) + 3H2O(g) How many g of…

A: Balance equation: C2H5OH(I) + 3O2(g) -----> 2CO2(g) + 3H2O(g) Mass = Number of moles x molar…

Q: If 5.0 moles of Pb(NO3)2 is reacted with 8.0 moles of KCl in the reaction Pb(NO3)2 + 2KCl…

Q: Consider this react 3Mg+2H POy > Mg(PO4)2+3Hz * how many maaneSiUM grams of onate should 3.

Q: produces carbon dioxide and water. After 4.64 mL of ethanol (density = 0.789 g/ml) was allowed to…

Q: 3. When baking soda (sodium bicarbonate or sodium hydrogen carbonate, NaHCO,) is heated, it releases…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: HEN POTASSIUM CHLORATE KCLO3 IS HEATED STRONGLY, IT BREAKS DOWN RELEASING OXYGEN GAS AND LEAVING…

A: Given data: Potassium chlorate = KClO3 Oxygen gas = O2 Potassium chloride = KCl On heating KClO3,…

Q: 2. If 24.5 grams of cobalt (II) oxide reacts with 2.58 grams of oxygen gas to form cobalt (III)…

Q: I just need a step-by-step explanation for this problem I forgot how to Calculate percent yield

A: The percentage yield of the substance can be described as the ratio of actual yield of the substance…

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

O Mass-Mass Stoich-$1 doc Sc
urses/216161/files/236134137wrap31
Met-GUY, KLE L on
> Files > Mass-Mass Stoich -s-1.doc
-Mass Stoich -s-1.doc
d Mass-Mass Stoich -s-1.doc (31 KB)
700M
3.
BALANCE the following equation:
KCIO3
-------> KCl + O,
grams
mole of KCIO,?
a) How many grams of KCl are produced from 250
b) How many grams of KCIO, are needed to produce 15 grams mole of O;?

Expert Solution

Balancing the decomposition reaction of KClO3:

Potassium chlorate decomposes to give potassium chloride and oxygen gas:

2 KClO₃ $\to 2 K C l_{(s)} + 3 O_{2_{(g)}}$

Note: The unit gram mole means molar mass of molecule/atom/ions etc in grams.

1 gram mole = mass of one mole of molecule in grams.

Calculating the mole ratio of KClO₃ and KCl

Since, 2 mol of KClO₃ gives 2 mol of KCl,

hence, mole ratio of KClO₃ : KCl = 2 : 1

Calculating the mole ratio of KClO₃ to O₂ gas:

Since, 2 mol of KClO₃ gives 3 mol of O₂ _,

hence, mole ratio of KClO₃ : O₂ = 2 : 3

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

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.
Given Active Ingredient: precipitated sulfur (ointment) Raw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g precipitated sulfur Formulation: 250 mg per jar Dosage form: Ointment packaging:100 jars per box Synthesis and Packaging (Need answer)- Balanced Chemical Equation:- % composition by mass of each compound:- Mass to Mass Stoichiometry Calculation:- Limiting Reagent:- Excess Reagent:- Amount (g) in excess: % Yield:- Number of dosage form and packaging that can be produced from stoichiometric solution:
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
Mass of Na2CO3.H2O (g) = 2.12g (g) Mass of the CaCl2.2H2O (g) = 1.98g Mass of the top funnel + filter paper (g) = 15.85g Mass of top funnel + filter paper + CaCO3 collected (g) = 17.81g CaCl2 + Na2CO3 ==== CaCo3 + 2NaCl Theoretical yield in moles and grams? Moles of reagent in excess left unreacted? Mass of precipitate? Experimental yield? Percent yield?
Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.
Magnesium +Acetic Acid --> C2HG5+ O2 ---> Iron (III) carbonate -->
Balance, what is he coefficient in front H2SO4?
Write the empirical formula for the hydrated KAl(SO4)2, based on moles of anhydrous KSI(SO4)2= 0.046 mol molar mass of H2O= 18g/ mol moles of H2O= 0.0444mol ratio pf moles H20 to moles of anhydrous KAI(SO4)2= 9.65/1 . Show all work including units. Hint: if the ratio of moles of H2O to moles of anhydrous KAl(SO4)2 was 4, then the empirical formula would be: KAl(SO4)2•4H2O.
Mass of empty beaker=16.26Volume of CuSO4 5H2O=30mLMolarity of CuSO4 5H2O used=0.542Moles of CuSO4 5H2O=0.016Mass of aluminum foil used=0.26gMass of beaker and copper product=52.12gMass of copper metal product=35.86gMoles of Al used = 0.009636 molMoles of CuSO4 5H2O used=0.016mol Find the moles of copper product based on moles of Al.Find the moles of copper product based on moles of CuSO4 5H2OFind the limiting reactant in grams
Assume that 1.00 mL (1.02 g) of crude product mixture is obtained from the reactionbefore the washing steps, and the distribution constant of the product mixture in brine isK = (Cmixture/Cbrine) = 50.0. Assuming that after mixing the product mixture volume isstill 1.00 mL (i.e., the volume lost is small), and the volume of the first brine wash layeris 2.00 mL. What mass (grams) of product mixture is lost (dissolves) in the first brinewash? (See Technique 13.2, p 53.) Show work.
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 + 2KNO3
Pure CO2 may be prepared by treating limestone with sulfuric acid. The limestone used in the process contains CaCO3, MgCO3 and inert. The acid used contains 12% H2SO4 by weight The residue from the process had the following composition. CaSO4 – 8.56%; MgSO4 – 5.23%; H2SO4 – 1.05%; Inert – 0.53%; CO2 – 0.12%; H2O – 84.51%; During the process, the mass was warmed where CO2 and H2O were removed. Calculate the following.a) The analysis of lime stone and b) The % excess acid used.