If a solution containing 106.70 g of mercury(II) nitrate is allowed to react completely with a solution containing 17.796 g of sodium sulfide, how many grams of solid precipitate will form? precipitate: How many grams of the reactant in excess will remain after the reaction? excess reactant: g

If a solution containing 106.70 g of mercury(II) nitrate is allowed to react completely with a solution containing 17.796 g of sodium sulfide, how many grams of solid precipitate will form? precipitate: How many grams of the reactant in excess will remain after the reaction? excess reactant: g

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter5: Chemical Reactions

Section: Chapter Questions

Problem 5.60E

See similar textbooks

Related questions

Q: Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution…

A: Pb(CH3COO)2 + H2SO4 ----- PbSO4 + 2CH3COOH Molar mass of Lead Acetate = 325.29 gm/mol Number of…

Q: For the following reaction, 4.41 grams of carbon (graphite) are allowed to react with 15.8 grams of…

A: To calculate the amount of carbon dioxide that can be formed we need to know its molecular mass and…

Q: For the following reaction, 28.9 grams of sulfur dioxide are allowed to react with 6.29 grams of…

Q: If a solution containing 59.943 g of mercury(II) nitrate is allowed to react completely with a…

Q: for the following reaction: FeCl3+MgO --> Fe2O3+MgCl2 If 0.1297Mol of FeCl3 is added, how much…

A: We have reaction of FeCl3 with MgO , we have added 0.1297 mol of FeCl3 , we have to calculate the…

Q: For the following reaction, 21.0 grams of sulfur dioxide are allowed to react with 8.42 grams of…

A: Balanced chemical equation: SO2 (g) + O2 (g) -------> SO3 (g) This equation suggests that:…

Q: For the following reaction, 4.36 grams of butane (C4H10) are allowed to react with 20.5 grams of…

A: Number of moles is calculated by dividing the given mass with molecular mass.

Q: For the following reaction, 9.91 grams of glucose (C6H12O6) are allowed to react with 14.1 grams of…

Q: For the following reaction, 8.20 grams of carbon (graphite) are allowed to react with 10.3 grams of…

Q: For the following reaction, 5.64 grams of chlorine gas are mixed with excess carbon disulfide. The…

A: The balanced chemical equation for the reaction of carbon disulfide ( CS2 ) and chlorine gas (Cl2)…

Q: An aqueous solution containing 8.66 g of lead(II) nitrate is added to an aqueous solution containing…

A: In a reaction there are substrate molecule and product molecule both are present. Balanced are those…

Q: For the following reaction, 3.48 grams of iron are mixed with excess oxygen gas . The reaction…

A: The reaction given is, => Fe (s) + O2 (g) → FeO (s) Given: Mass of Fe reacting = 3.48 g. And mass…

Q: For the following reaction, 3.64 grams of hydrogen gas are allowed to react with 48.9 grams of…

A: given, mass of hydrogen gas = 3.64 g mass of iodine = 48.9 g we need to calculate mass of…

Q: For the following reaction, 21.9 grams of iron are allowed to react with 33.9 grams of chlorine gas.…

A: Given, mass of iron = 51.9 grams mass of chlorine = 33.9 grams

Q: For the following reaction, 3.88 grams of oxygen gas are mixed with excess carbon (graphite). The…

Q: If a solution containing 109.90 g of mercury(II) nitrate is allowed to react completely with a…

A: Here, we have to find the mass of the precipitate that will be formed when 109.90 g of mercury(II)…

Q: When a solution containing 15.0g of lead(ii)nitrate and a solution containing 15.0g of potassium…

A: Lead (II) nitrate reacts with potassium iodide to form an aqueous solution of potassium nitrate and…

Q: According to the following reaction, how many grams of calcium oxide will be formed upon the…

A: First write a balanced equation: CaCO3 → CaO + CO2 1mol CaCO3 will produce 1 mol CaO Molar…

Q: Copper(II) carbonate was used by artists as a pigment due to its bright green-blue colour. It can be…

Q: For the following reaction, 4.52 grams of hydrogen gas are mixed with excess iodine. The reaction…

A: Given :- hydrogen(g) + Iodine(s) → Hydrogen iodide (g) mass of Hydrogen = 4.52 g actual yield of…

Q: For the following reaction, 8.39 grams of carbon (graphite) are allowed to react with 12.6 grams of…

A: Given: Mass of Carbon= 8.39 g Mass of Oxygen gas= 12.6 g To calculate: a) Maximum amount of CO2…

Q: For the following reaction, 6.64 grams of oxygen gas are mixed with excess carbon (graphite). The…

Q: For the following reaction, 5.18 grams of chlorine gas are mixed with excess iron. The reaction…

A: In the first reaction, limiting reagent chlorine will give the theoretical yield of ferric chloride…

Q: For the following reaction, 5.71 grams of oxygen gas are mixed with excess carbon (graphite) . The…

A: The reaction taking place is given as, => Carbon (graphite) (s) + oxygen (g) -----> Carbon…

Q: For the following reaction, 66.5 grams of iron(III) oxide are allowed to react with 20.9 grams of…

A: The reaction taking place is - Fe2O3 + 2Al → Al2O3 + 2Fe Given mass of Fe2O3 = 66.5 g Molar mass of…

Q: For the following reaction, 6.18 grams of nitrogen gas are mixed with excess hydrogen gas . The…

A: To solve this problem first we have to write the balanced chemical equation then according to the…

Q: According to the following reaction, how many grams of zinc hydroxide will be formed upon the…

Q: For the following reaction, 4.40 grams of ethylene (C,H4) are mixed with excess hydrogen gas . The…

A: For the reaction: C2H4(g) + H2(g) →C2H6(g) Hydrogen gas behaves as the excess reactant as it is…

Q: A sample of 6.64 g of liquid 1-propanol, C,HO, is combusted with 44.9 g of oxygen gas. Carbon…

A: Given, Mass of liquid 1-Propanol(C3H8O) = 6.64 g Mass of oxygen gas(O2) = 44.9 g Physical state of…

Q: For the following reaction, 4.91 grams of iron are mixed with excess oxygen gas. The reaction yields…

Q: If a solution containing 61.28 g of lead(II) chlorate is allowed to react completely with a solution…

A: The chemical reaction between lead chlorate and sodium sulfide is shown below;…

Q: If a solution containing 108.65 g of mercury(II) acetate is allowed to react completely with a…

Q: If a solution containing 127.23 g of silver chlorate is allowed to react completely with a solution…

Q: For the following reaction, 3.77 grams of chlorine gas are mixed with excess iron. The reaction…

Q: For the following reaction, 10.8 grams of glucose (C,H1206) are allowed to react with 16.3 grams of…

A: We first calculated the moles of each reactant. Then using the balanced chemical equation we take…

Q: For the following reaction, 4.50 grams of water are mixed with excess diphosphorus pentoxide. The…

A: The reaction taking place is given as, => diphosphorus pentoxide(s) + water(l) → phosphoric…

Q: For the following reaction, 4.36 grams of sulfur are mixed with excess carbon monoxide. The reaction…

A: Sulfur reacts with carbon monoxide to form sulfur dioxide and carbon. The equation for the balanced…

Q: For the following reaction, 4.81 grams of iron are mixed with excess hydrochloric acid. The reaction…

Q: For the following reaction, 36.4 grams of aluminum oxide are allowed to react with with 132 grams of…

A: Solution stoichiometry involves the calculation of concentration of solutions in the given…

Q: For the following reaction, 56.7 grams of iron(III) oxide are allowed to react with 17.8 grams of…

Q: If a solution containing 23.09 g of mercury(II) nitrate is allowed to react completely with a…

Q: For the following reaction, 6.52 grams of sulfuric acid are mixed with excess barium hydroxide. The…

A: Given :- amount of sulfuric acid = 6.52 g actual yield of barium sulfate = 11.7 g To be…

Q: According to the following reaction, how many grams of calcium oxide will be formed upon the…

Q: An aqueous solution containing 9.55 g9.55 g of lead(II) nitrate is added to an aqueous solution…

A: Given that : The mass of lead (II) nitrate = 9.55 g The mass of potassium chloride = 5.77 g The…

Q: For the following reaction, 17.1 grams of iron are allowed to react with 36.2 grams of chlorine gas…

Q: For the following reaction, 6.42 grams of oxygen gas are mixed with excess hydrogen sulfide. The…

A: The limiting reagent gives the smallest yield of product calculated from the reagents (reactants)…

Q: According to the following reaction, how many grams of hydrochloric acid will be formed upon the…

A: By the help of stoichiometric coefficient we can find the amount of unknown substance by the help of…

Q: For the following reaction, 33.5 grams of iron are allowed to react with 18.8 grams of oxygen gas.…

A: 4Fe + 3O2 → 2 Fe2O3Molecular weight of…

Q: For the following reaction, 4.59 grams of water are mixed with excess carbon monoxide. The reaction…

Q: When silver nitrate and sodium sulfate react, a precipitate forms. What mass of the precipitate is…

A: A)

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

100%

If a solution containing 106.70 g of mercury(II) nitrate is allowed to react completely with a solution containing 17.796 g of
sodium sulfide, how many grams of solid precipitate will form?
precipitate:
g
How many grams of the reactant in excess will remain after the reaction?
excess reactant:

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 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 3 images

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

Citric acid, C6H5CH3, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger . The equation representing this reaction is C12H22O11+H2O+3O22C6H8O7+4H2O What mass of citric acid is produced from exactly 1 metric ton (1.000103kg) of sucrose if the yield is 92.30%?
At high temperatures, silicon dioxide reacts with carbon to produce silicon carbide, SiC, also known as carborundum, an important industrial abrasive. If the reaction is run with 100. g of each reactant: (a) Determine the limiting reactant; and (b) Calculate the mass of excess reactant remaining after the reaction is over.
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?
Sulfur dioxide gas reacts with sodium hydroxide to form sodium sulfite and water. The unbalanced chemical equation for this reaction is given below: SO2(g)+NaOH(s)Na2SO3(s)+H2O(l) Assuming you react 38.3 g sulfur dioxide with 32.8 g sodium hydroxide and assuming that the reaction goes to completion, calculate the mass of each product formed.
Although many sulfate salts are soluble in water, calcium sulfate is not (Table 7. 1). Therefore, a solution of calcium chloride will react with sodium sulfate solution to produce a precipitate of calcium sulfate. The balanced equation is :math>CaCl2(aq)+Na2SO4(aq)CaSO4(s)+2NaCl(aq) a solution containing 5.21 g of calcium chloride is combined with a solution containing 4.95 g of sodium sulfate, which is the limiting reactant? Which reactant is present in excess?
For each of the following balanced chemical equations, calculate how many grams of the product(s) would be produced by complete reaction of 0.125 mole of the first reactant. msp;AgNO3(aq)+LiOH(aq)AgOH(s)+LiNO3(aq) msp;Al2(SO4)3(aq)+3CaCl2(aq)2AlCl3(aq)+3CaSO4(s) msp;CaCO3(s)+2HCl(aq)CaCl2(aq)+CO2(g)+H2O(l) msp;2C4H10(g)+13O2(g)8CO2(g)+10H2O(g)
Lead(II) carbonate, also called “white lead,” was formerly used as a pigment in white paints. However, because of its toxicity, lead can no longer he used in paints intended for residential homes. Lead(II) carbonate is prepared industrially by reaction of aqueous lead(II) acetate with carbon dioxide gas. The unbalanced equation is :math>Pb(C2H3O2)2(aq)+H2O(l)+CO2(g)PbCO3(s)+HC2H3O2(aq) ppose an aqueous solution containing 1.25 g of lead(II) acetate is treated with 5.95 g of carbon dioxide. Calculate the theoretical yield of lead carbonate.
Thionyl chloride, SOCl2, is used as a very powerful drying agent in many synthetic chemistry experiments in which the presence of even small amounts of water would be detrimental. The unbalanced chemical equation is :math>SOCl2(l)+H2O(l)SO2(g)+HCl(g) lculate the mass of water consumed by complete reaction of 35.0 g of SOCl2.
When small quantities of elemental hydrogen gas are needed for laboratory work, the hydrogen is often generated by chemical reaction of a metal with acid. For example, tine reacts with hydrochloric acid, releasing gaseous elemental hydrogen: :math>Zn(s)+2HCI(aq)ZnCl2(aq)+H2(g) at mass of hydrogen gas is produced when 2.50 g of zinc is reacted with excess aqueous hydrochloride acid?
Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide al high temperatures. mg src=Images/HTML_99425-9-66QAP_image001.jpg alt="" align="top"/> e other products of the reaction are nitrogen gas and water Vapor. The balanced equation for this reaction is: :math>2NH3(g)+3CuO(s)N2(g)+3Cu(s)+3H2O(g) at is the theoretical yield of solid copper that should form when 18.1 g of NH3, is reacted with 90.4 g of CuO? If only 45.3 g of copper is actually collected, what is the percent yield? mg src=Images/HTML_99425-9-66QAP_image002.jpg alt="" align="top"/>
A yield of 3.00gKClO4 is obtained from the (unbalanced)reaction KClO3KClO4+KCl when 4.00 g of the reactant is used. What is the percentageyield of the reaction?
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)