Answered: 2 KMnO4 + 5 H2C2O4 + 3 H2SO4 --> 2…

2 KMnO4 + 5 H2C2O4 + 3 H2SO4 --> 2 MnSO4 + 10 CO2 + 8 H2O + K2SO4 If 6.78 g of KMnO4 (MW = 158.03 g/mol) react completely, how many grams of potassium sulfate (MW = 174.26 g/mol) will be produced?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 62QAP: Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker...

See similar textbooks

Related questions

Q: NaCl+H2SO4-> Na2SO4+2HCl a. when there is 35.0 g NaCl and 33.0 g H2SO4 are mixed and react…

Q: For the following reaction: 2H2O + N2O5 —> 2NHO3 What is the theoretical yield of nitric acid (HNO3)…

Q: 4 Fe(CrO2)2 + 8 K2CO3 + 7 02 ----> 2 Fe203 +8 K2CrO4 + 8 CO2 Calculate the percent yield of Fe203…

A: To solve this problem first we calculate the theoretical yield of Fe2O3 . Then percentage yield will…

Q: A reaction has a percent yield 25.6 %. What is the theoretical yield of this reaction if 150.5…

A: Percentage yield is obtained by grams of your actual yield by the grams of theoretical yield and…

Q: Co(g) reacts with H20(g) to form CO2(g) and H2(g). What is the percent yield if 1.8 g H2(g) gas is…

Q: 2KF + Mg(NO3)2 --> MgF2 + 2KNO3 If 100 g potassium fluoride react with 100 g magnesium nitrate how…

Q: When 0.0916 g P406 were mixed with 0.113 g H2O, a student obtained 0.121g H3PO3. What was the…

Q: In the following reaction, what mass of Na will react exactly with 0.20 moles of water? 2Na(s) +…

A: Given data,Moles of water=0.20molesGiven reaction;2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)

Q: if you have 51.8 grams of chromium that react with exceess oxygen how much chromium (III) oxide will…

A: Given, 4Cr(s) + 3O2(g) --> 2Cr2O3(s) Mass of chromium (Cr) = 51.8 g Oxygen gas (O2) = excess…

Q: KC3H5O4 + 7.5 02--> 8 CO2 + 2 H20 + KOH For the reaction listed above, how many grams of oxygen (as…

A: 1 mole = 6.022×1023 [ Avogadro's number ] The mass of one mole of atoms of an element is called its…

Q: 5) For the following reaction: I2 (g) + H2 (g) → 2HI (g) If the amount consumed from (I2) according…

Q: Consider the following reaction: Mg(OH)2(aq) + 2 HNO3(aq) --> Mg(NO3)2(aq) + 2 H2O(l)…

A: Number of mol = Mass/Molar mass % Yield = 100 x Obtained amount/Calculated amount

Q: 3 Ni(NO3)2•6H2O (s) + 2 Na3PO4 (aq) --> Ni3(PO4)2 (s) + 6 NaNO3 (aq) If 5.226 g…

A: Mass of Ni(NO3)2•6H2O = 5.226 g Molar mass of Ni(NO3)2•6H2O = 290.79 g/mol Number of moles of…

Q: In the reaction of 1.01 g of salicylic acid (MM = 138.122 g/mol) with 2.82 g of acetic anhydride (MM…

A: Solution 1.

Q: A mass of 8.15 g C2H4(g) reacts with excess oxygen. If 16.2 g CO2(g) is collected, what is the…

A: The reaction taking place is given as, => C2H4 (g) + O2 (g) ------> CO2 (g) + H2O (g) Given:…

Q: MNSO4 · H20(aq) + H2C2O4(aq) +2H20() - Starting with 3.84 g of MNSO4 · H2O with an excess of oxalic…

A: Manganese sulfate reacts with oxalic acid to form manganese oxalate and sulfuric acid. The equation…

Q: What mass of iron (III) oxide is produced when 3.88 x 10^25 molecules of oxygen reacts with excess…

A: Given 3.88 x 1025 molecules of oxygen 4fe + 3O2 ---> 2Fe2O3

Q: How many grams of Cl2 can be prepared from the reaction of 16.0 g of MnO2 and 30.0 g of HCl…

A: Reaction is : 4HCI + MnO2 →MnCl₂ + Cl₂ + 2H₂0 moles of H+C1 = mass / molar mass = 3035.45+…

Q: Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be…

Q: Cryolite, Na, AIF, (s), an ore used in the production of aluminum, can be synthesized using aluminum…

A: Since you have asked a question with multiple sub-parts, as per our company guidelines we are…

Q: 6 Na(l) + Al2O3(s) ----------> 2 Al(l) + 3 Na2O(s) When 5.52 g of sodium react with excess…

Q: For the reaction CaCl2 + 2AgNO3 --> 2AgCl + Ca(NO3)2 , if AgNO3 is added in excess, what is the…

Q: How many mL of MNSO4 would be produced in the following reaction if you started with 2.00 g H2C2O4,…

Q: When 0.0916g P4O6 were mixed with 0.113 g H2O, a student obtained 0.121 g H3PO3. What was the…

Q: 4Fe(CrO2)2 + 8 K2CO3 + 7 O2 --> 2Fe2O3 + 8 K2CrO4 +8CO2 Calculate the percent yield of Fe2O3…

A: In this question we want to determine the percent yield of the Fe2O3 How we can determine, you can…

Q: To synthesize titanium (IV) chloride, the reaction below is used. 3TIO2(s) + 4C(s) + 6CI2(g) →…

A: Theoretical yield: The yield which depends upon the stoichiometry of the reactants is called…

Q: If 28.6 g of Fe203 reacts with 14.9 g Al, identify the limiting reactant and calculate the…

A: Welcome to bartleby! Introduction : We have to calculate the limiting reagent and theoretical…

Q: For the reaction CaCl2 + 2AgNO3 --> 2AgCl + Ca(NO3)2 , if AgNO3 is added in excess, what is the…

A: As AgNO3 is in excess, so CaCl2 is limiting reagent. Mass of CaCl2 = 18.7 g Molar mass of CaCl2 =…

Q: A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water. Mg3N2 + 3H2O → 2NH3 + 3MgO The…

Q: Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be…

A: The given chemical reaction is as follows: 5Ca + V2O5 → 5CaO + 2V The given mass of V2O5 = 1.540×103…

Q: Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be…

Q: 2Fe(OH)3(s) + 3H2SO4(aq) Fe2(SO4)3(aq) + 6H2O(l) If 2.4 g Fe(OH)3 and 3.3 g H2SO4 react and make…

Q: If 25 grams of methane, CH 4, and 30 g of ammonia, NH 3, are combined w/ excess oxygen, when the…

Q: How many grams of H2 are required to produce7.50 grams of NH3 N2(g) + 3H2(g)-----> 2NH3(g)

A: Nitrogen reacts with hydrogen to form ammonia. The equation for the balanced chemical reaction is…

Q: Asprin, Cg Hg O4, is synthesized by the reaction of salicylic acid, C7H6 O3, with acetic anhydride,…

A: NOTE: please note the given equation is incorrect. I have corrected it and written proper equation.…

Q: 17. 55.0 g of potassium iodide and 185.5 g of lead(II) nitrate react and 35.0 g of lead(II) iodide…

Q: 6H2O

A: Given, Ethane undergoes combustion in the presence of oxygen to produce carbon dioxide and water.…

Q: 2Fe(OH)3(s) + 3H2SO4(aq) Fe2(SO4)3(aq) + 6H2O(l) If 2.4 g Fe(OH)3 and 3.3 g H2SO4 react and make…

A: The given reactants will react to form products according to their stoichiometry in the given…

Q: Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be…

A: Based on limiting reagent we can calculate percentage of yield moles= weight/molecular weight

Q: Given the equation for the decomposition of hydrogen peroxide, 2 H2O2 --> O2 + 2 H2O, a student sets…

A: Conversion factor are those factor which are used to find relation between the quantity of reactant…

Q: Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be…

A: First, calculate the moles for both reactants and then use the mol to mol ratio to find out the…

Q: H3PO4 + 3NaOH ---> Na3PO4 + 3H2O If you mix 100 ml of 8.5M H3PO4 with 150 ml of 9.0M NaOH, how…

Q: What is the minimum amount of 5.7 M H2SO4 necessary to produce 26.8 g of H2 (g) according to the…

A: Mole: Mole of the substance is calculated as mass divided by molar mass of the substance.…

Q: How many grams of iron metal are formed

A: Given :- mass of Al = 81.0 g To calculate :- mass of Fe (in grams) Number of moles = mass/molar…

Q: How many grams of hydrogen gas are produced by the reaction of 5.0 g of zinc with excess…

A: Welcome to bartleby !

Q: 5. Pyrite (FeS2) reacts with oxygen according to the reaction below: 4 FeS2(s) + 11 O2(g) 2 Fe2O3(s)…

A: Since there are multiple questions, we will answer only the first one, that is, no. 5. If you…

Q: FePO4+ 3 Na2SO4 ---> Fe2(SO4)3+ 2 Na3PO4 If I perform this reaction with 25 g of Iron (III)…

A: In this question, you want to determine the percent yield of the Product ( means Iron (III) sulfate…

Q: Consider the reaction of 132.4 grams of NH3 and 173.5 grams O2 What is the theoretical yield of H20…

A: Given: Mass of NH3 = 132.4 g Mass of O2 = 173.5 g Molar mass of NH3 = 17.03 g/mol Molar mass of O2 =…

Q: What was the percent yield?

Question

2 KMnO₄ + 5 H₂C₂O₄ + 3 H₂SO₄ --> 2 MnSO₄ + 10 CO₂ + 8 H₂O + K₂SO₄

If 6.78 g of KMnO₄ (MW = 158.03 g/mol) react completely, how many grams of potassium sulfate (MW = 174.26 g/mol) will be produced?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

A 100.0-g mixture made up of NaCl03, Na2CO3, NaCl, and NaHCO3 is heated, producing 5.95 g of oxygen, 1.67 g of water, and 14.5 g of carbon dioxide. NaCl does not react under the conditions of the experiment. The equations for the reactions that take place are: 2NaClO3(s)2NaCl(s)+3O2(g)Na2CO3(s)2Na2O(s)+CO2(g)2NaHCO3(s)Na2O(s)+2CO2(g)+H2O Assuming 100% decomposition of NaClO3, Na2CO3, and NaHCO3, what is the composition of the mixture in grams?
Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker containing 20.0 g of NaOH. Not all the NaOH was consumed. How many grams of NaOH were left unreacted? The equation for the reaction is H3PO4(aq)+3OH(aq)3H2O+PO43(aq)
For the reaction: C3H8 + O2 ------> CO2 + H2O , What weight in kg of H2O will be produced if 12.3 moles of C3H8 are used?
silver sulfadiazine burn- treating cream creates a barrier against baterial invasion and realeases antimicrobial agents directly into the wound. if 35.0 g Ag2O is reacted with 70.0g C10H10N4SO2, what mass of silver sulfadiazine, AgC10H9N4SO2, can be produced, assuming 100% yield? Ag2O(s)+2C10H10N4SO2(s) -> 2AgC10H9N4SO2(s)+H2O(L) mass=?
Sulfur can be recovered from the hydrogen sulfide removed from crude oil deposits, a process known as sweetening, by roasting in air and using the sulfur dioxide initially formed to push the reaction to the final product: H2S(g) + O2(g) --> H2O(g) + SO2(g) H2S(g) + SO2(g) --> H2O(g) + S(s) The maximum number of kilograms of sulfur that can be isolated per kilogram of hydrogen sulfide entering the process is __________.
Methanol, CH3OH, can be prepared from carbon monoxide and hydrogen according to the reaction CO (g) + 2 H2 (g) --> CH3OH (l). What mass of hydrogen is required to produce 1.0 L of methanol (density = 0.791 g/mL) if this reaction has a 74% yield under certain conditions?
Consider the reaction 2D2(g)+O2(g)→2D2O(l)2D2(g)+O2(g)→2D2O(l) What is the mass of heavy water, D2O(l)D2O(l), produced when 8.75 gg of O2(g)O2(g) reacts with excess D2(g)D2(g)? Express your answer with the appropriate units.
The fizz produced when an Alka-Seltzer tablet is dissolvedin water is due to the reaction between sodium bicarbonate1NaHCO32 and citric acid 1H3C6H5O72:3 NaHCO31aq2 + H3C6H5O71aq2¡3 CO21g2 + 3H2O1l2 + Na3C6H5O71aq2 In a certain experiment 1.00 g of sodium bicarbonate and1.00 g of citric acid are allowed to react. (a) Which is the limitingreactant? (b) How many grams of carbon dioxide form?(c) How many grams of the excess reactant remain after thelimiting reactant is completely consumed?
3. Consider the nickel salt: (NH4 )2Ni(SO4 )2 ·y H2O (Ammonium Nickel Sulfate Hydrate), where y is the number of coordinated waters. (a) Assuming that the product is anhydrous (y = 0), what is the theoretical yield of ammonium nickel sulfate from 1.500 g of Ni (s)? (b) The actual yield of product was 9.640 g - obviously containing coordinated water. The product was then heated strongly until all the water had been driven off. The resulting anhydrous salt had mass 7.000 g. What is the value of y? (c) Based on the mass of the anhydrous product (7.000 g), what is the % yield of the reaction?
Nitrobenzene C6H5NO2, is an important raw material for the dy industry. It is prepared from benzene C6H6, and nitric acid HNO3. C6H6 (I) + HNO3 (I) ---> C6H5NO2 (1) + H2O (I) When 22.4 g of benzene and an excess of HNO3 are used, what is the theoretical yield of nitrobenzene? If 28.7g of nitrobenzene is recovered, what is the percentage yield?
3.50g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 176./gmol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 5.25g water 1.43g Use this information to find the molecular formula of X
Adipic acid, H2C6H8O4, is used to produce nylon. It is made commercially by a controlled reaction between cyclohexane ( C6H12 ) and O2: 2 C6H12 (l) + 5 O2 (g) → 2 H2C6H8O4 (l) + 2 H2O (g) (Given: Atomic Wts (g/mol): C= 12.01 ; H=1.01 ; O=16.00 ) If 25.0 g of cyclohexane is reacted with 20.0 g of O2, a. Identify the limiting reactant and excess reactant? b. How much in grams of the excess reactant will be left after the reaction? c. What is the theoretical yield in terms of the product adipic acid? d. If the actual yield is 33.5 g, what is the % yield of adipic acid?