Answered: 301.4 g of SO2(g), 409.3 g of CaCO3(s),…

301.4 g of SO2(g), 409.3 g of CaCO3(s), and 101.7 g of O2(g) react in the following fashion: 2 SO2(g) + 2 CaCO3(s) + O2(g) ---> 2 CaSO4(s) + 2 CO2(g) What mass (in g) of CaSO4(s) is produced?

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...

See similar textbooks

Related questions

Q: The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In…

Q: 7.5 g of Pb(NO3)2 (aq) is reacted with excess KBr (aq) to produce 4.3 g of PbBr2 (s). What is the…

A: Reaction: Pb(NO3)2 (aq) + 2 KBr (aq) → PbBr2(s) + 2 KNO3(aq) 331.2 g…

Q: The chemical equation for the complete combustion of propane, C₂Hg(g), is C₂Hg(g) +5 0₂(g) → 3…

A: The chemical equation given is C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) Mass of propane, C3H8 (g)…

Q: The metals industry was a major source of air pollution years ago. One common process involved…

A: Given the reaction is, 2PbS+3O2---->2PbO+2SO2 Mole of PbS is 9.53mol. We have to calculate mole…

Q: The combustion of propane may be described by the chemical equation C₂H₂(g) +50₂(g)-3C0₂(g) +…

A: Number of moles = mass/molar mass Mass = moles × molar mass Molar mass of O2 = 31.999 g/mol Molar…

Q: If 7.3 grams of sodium carbonate are used in the reaction and the result a 74.0% yield, what is the…

A: The balanced reaction taking place is given as, => Sn3(PO4)4 + 6 Na2CO3 → 3 Sn(CO3)2 + 4 Na3PO4…

Q: 23 In a universe far, far away, there exists an alien world where they have a different periodic…

A: Instead of the conventional periodic table some alien periodic table is given, wherein name of…

Q: The limiting reagent is

Q: Consider the reaction: 2Fe(s) + O₂(g) → 2FeO(s) Given an initial mass of 19.87 g Fe, an excess of…

Q: The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000°C and…

Q: Magnesium hydroxide (Mg(OH) 2), as "Milk of Magnesia" can be used to neutralize excess stomach acid,…

Q: Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) →…

A: Given : Mass of sucrose = 35.4 gram Molar mass of sucrose = 342 gm/mole

Q: When copper(II) sulfate pentahydrate (CuSO4·5 H2O) is heated, it decomposes to the dehydrated form.…

Q: Iron(III) oxide reacts with carbon monoxide according to the equation: Fe,0;(6) + 3 CO(g) – 2 Fe(s)…

A: The given reaction is, Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) Given that: mass of Fe2O3 = 22.55 g…

Q: Acetic acid, sold as vinegar, is produced by the carbonylation of methanol, according to the…

Q: A sample of 1.544moles of methane (CH4) is mixed with 1.273 moles of chlorine. What is the…

A: Given :- number of moles of CH4 = 1.544 mol number of moles of Cl2 = 1.273 mol To be calculated :-…

Q: 18 g of CH4(g) are reacted with 5.2 g of O2(g) by the following reaction CH4(g) + 2O2(g) -->…

A: Given, mass of CH4 (g) = 18 g mass of O2 (g) = 5.2 g Now, the moles of CH4 (g) and O2…

Q: A sample of 1.129moles of methane (CH.) is mixed with 1.754 moles of chlorine. What is the…

A: Given :- number of moles of CH4 =1.129 mol number of moles of Cl2 = 1.754 mol To calculate :- The…

Q: Hydrazine can be synthesized via the following reaction: 2NH3(aq) + Cl2(g) + 2NaOH(aq) → N₂H4(aq) +…

Q: The following equation represents the combustion reaction of octane (C8H18), which is the primary…

A: Given, 2C8H18(l) + 25 O2(g) --> 16CO2(g) + 18H2O(l) Excess reactant - O2 gas molar mass of…

Q: [References] A sample of limestone and other soil materials was heated, and the limestone decomposed…

A: Calcium carbonate decomposes into calcium oxide and carbon dioxide. The equation for the balanced…

Q: The amount of product that can be produced depends only on the amount of the limiting reactant…

Q: In a combustion reaction between 700.0 mL propane, C3H8 with oxygen gas, O2 at 25 °C, an unknown…

A: The chemical equations should be balanced in accordance with the law of conservation of mass.…

Q: Consider the reaction. 2Pb(s)+O2(g)⟶2PbO(s) An excess of oxygen reacts with 451.4 g of lead,…

Q: Consider the reaction: P4(s) + 6Cl₂(g) → 4PC13 (1) Given an initial mass of 15.75 g P4, an excess of…

Q: In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following…

A: The given chemical reaction is PCl5s + 4H2Ol →H3PO4aq + 5HClg. The mass of PCl5 is 12.0 g. The mass…

Q: PCL5(s) + H2O(l) ----> POCl3(l) + 2HCl(aq) When 79.60 g of phosphorus pentachloride reacts with…

Q: When ammonia (NH3) is reacted with an excess of oxygen gas, it produces nitrogen monoxide gas and…

Q: In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following…

A: Limiting reagent of a reaction is the compound which is completely consumed during the reaction. The…

Q: e percentage yield of the

Q: Under certain conditions the formation of ammonia from nitrogen with excess oxygen produces a 38.2%…

A: The given balanced equation is as follows. 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) Molar mass of NH3=17…

Q: A sample of 8.61 g8.61 g of liquid 1‑propanol, C3H8O,C3⁢H8O, is combusted with 64.6 g64.6 g of…

A: It's a multiple part question. Given information, Mass of 1-propanol = 8.61 g Mass of oxygen gas =…

Q: hat are the percentages of carbon, hydrogen, and nitrogen in the compound? What is the empirical…

A: Solution: So this question is from the stoichiometry. We have general knowledge of formulae for…

Q: Lime, CaO, can be produced in two steps as shown in the equations below. If the percentage yield of…

Q: The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O according to the…

A: We have 52.4 g of ammonia, we have to calculate the mass of nitrogen dioxide produced.

Q: Consider the reaction. 2Pb(s)+O2(g)⟶2PbO(s) An excess of oxygen reacts with 451.4 g of lead, forming…

A: First, calculate the theoretical yield of the given reaction,

Q: Consider the reaction of ethylene (C 2H 4) and water to form ethanol (C 2H 6O), which was mentioned…

A: Given: The theoretical yield of ethanol is 23 g. The actual yield of ethanol is 15 g.…

Q: Balance the following chemical equation CB,H.(g) + O₂(g) - > CO₂(g) + H₂O(g)

A: Is an equation in which the number of atoms for each element in the reaction and the total charged…

Q: How many moles of nitrogen are formed when 85.6 g of KNO3 decomposes according to the following…

A: First convert mass into mole by dividing molar mas software KNO3 Then use mole-mole relationship

Q: Consider the reaction: C(s) + O₂(g) → CO₂(g) Given an initial mass of 11.3 g C, an excess of O2, and…

Q: Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) →…

A: Given - Un - Balanced Chemical equation is - C₁₂H₂₂O₁₁(s) + O₂(g) → CO₂(g) + H₂O(l) The balanced…

Q: Lime, CaO, can be produced in two steps as shown in the equations below. If the percentage yield of…

A: The two reactions given are,

Q: You are given the balanced chemical reaction: C4H8(g) + 6 O2(g) 4 CO2(g) + 4H₂O(g). If 0.3218 moles…

Q: NH3 (g) + 5 O2 (g) -> 4NO (g) + 6H2O (g) Part A) What is the theorectical yield of water (in mg)…

A: Welcome to bartleby! We have to calculate theoretical yield of water and limiting reagent also…

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: Silicon tetrachloride (SiCl4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2Cl2(g) ->…

A: Molar mass of Cl2 = 70.9 g/mol

Q: In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following…

A: The given chemical reaction is PCl5s + 4H2Ol →H3PO4aq + 5HClg. The mass of PCl5 is 12.0 g. The mass…

Q: The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is…

A: Given, mass of NO = 9.500 g Mass of O2= 11.99 g Molar mass of NO = 30.0 g/mol Molar mass of O2=…

Q: In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following…

A: ♣ Limiting reactants are those reactants that are consumed completely in a chemical reaction. They…

Q: Alcoholic fermentation converts glucose (C6H12O6) into ethanol (C2H5OH) and carbon dioxide (CO2).…

A: Alcoholic fermentation of Glucose gives Ethanol and Carbon dioxide. It can be written in chemical…

Question

301.4 g of SO₂(g), 409.3 g of CaCO₃(s), and 101.7 g of O₂(g) react in the following fashion:

2 SO₂(g) + 2 CaCO₃(s) + O₂(g) ---> 2 CaSO₄(s) + 2 CO₂(g)

What mass (in g) of CaSO₄(s) is produced?

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

In coal, sulfur typically exists in the form of iron pyrites, FeS₂, or in organic compounds. Burning coal in power plants converts the sulfur to sulfur dioxide according to the following reaction: 4 FeS2(s) + 11 O2(g) --> 2 Fe₂O3(s) + 8 SO2(g) What mass (in grams) of sulfur dioxide is produced when 0.334 mol of oxygen gas reacts?
Worksheet 2: The Mole and Chemical Quantities 1) What is the molar mass of ammonium sulfate? 2) a) How many MOLECULES of nitrogen trifluoride are present in 4.50 moles of this compound? b) How many ATOMS of fluorine are present in 4.50 moles of nitrogen trifluoride? c) How many MOLES of nitrogen trifluoride are present in 1.24 x 10 22 molecules of this compound? d) How many grams of nitrogen trifluoride must be weighed out to get a sample of nitrogen trifluoride that contains 18.7 g of fluorine? e) If a sample of nitrogen trifluoride contains 18.7 g of fluorine, how many grams of nitrogen does it contain? 3) Magnesium hydroxide and ammonia are formed when magnesium nitride is added to water Mg3N2 (s) + 6 H2O (1) → 3 Mg(OH)2 (s) + 2 NH3 (1) a) How many moles of magnesium nitride are needed to produce 2.00 moles of ammonia?
328.8 g SO2(g), 425.3 g CaCO3(s), and 105.7 g 02(g) react as follows:2 SO2(g) + 2 CaCO3 (s) + 02(g) ---> 2 CaSO4(s) + 2 CO2(g)What mass (in g) of CaSO4(s) is produced?
Glucose, C,H,,O6, is used as an energy source by the human body. The overall reaction in the body is described by the equation C,H120,(aq) + 6 0,(g) → 6 CO,(g) + 6 H,O(1) Calculate the number of grams of oxygen required to convert 63.0 g of glucose to CO, and H,O. mass of O2: Calculate the number of grams of CO, produced. g mass of CO,: Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Scienc
A 18.2 g of iron metal reacts with excess oxygen gas to produce 47.9 g of Fe3O4. The reaction between these two substances are written as: ____ Fe(s) + ____ O2(g) → _____ Fe3O4 (s) Balance the chemical equation. Calculate the molar mass of O2 and Fe3O4. If the 43.72 g of Fe3O4 was produced, what is the percent yield of this reaction?
Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation: N2(g) + 3H2(9) → 2NH3(g) 1. What is the maximum mass of ammonia that can be produced from a mixture of 191.3 g of N2 and 46.25 g of H2? 2. Which element would be completely consumed? (enter nitrogen or hydrogen) 3. What mass of the starting material would remain unreacted? Submit Answer Tries 0/10
The formation of potassium chlorate, KClO3, can be represented by the equation (unbalanced): K (s) + Cl2 (g) + O2 (g) = KClO3 (s) The molar masses are; K = 39.1 g/mol; Cl2 = 70.9 g/mol; O2 = 32.0 g/mol If we reacted 100.0 grams of each reagent, which would be the limiting reagent for the reaction? Group of answer choices Cl2 K O2
For the reaction CH4 (g) + Cl2 (9) → CH3 Cl (g) + HCl (g) When 41.6 g of CHĄ and 84.0 g of Cl, reacts completely, what is the mass of HCl that could be produced? Molar mass: CH4 = 16.05 g mol-1; Cl2 = 70.90 g mol-1; HCI = 36.46 g mol-1 O 43.2 g O 94.5 g O 191. g O 18.3 g O 21.4 g
Sodium hypochlorite is the active ingredient in most household bleach products. One method of preparing this compound is as follows: Cl2(g) + 2N2OH(aq) → NaOCI (aq) + NaCl(aq) + H2O(1) In a certain experiment, 50.0 g chlorine was reacted with 50.0 g sodium hydroxide to yield 37.8 g sodium hypochlorite. (a) Calculate the theoretical yield (b) Calculate the percent yield.
SO2(g) + H2O(l) → H2SO3(g) Given an initial mass of 14.12 g SO2, an excess of H2O, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of H2SO3 produced by the reaction.
In one reaction, 41.2 g of Cu(NO3)2 is produced. What amount (in mol) of CuCl2 was consumed? What mass (in grams) of AgCl is produced? mol CuCl2 consumed g AgCl produced
4.529 g of antimony (III) sulfate and 13.98 g of lead (II) chlorate are reacted together. How much of all products and reactants are left after the reaction is complete?