Consider the reaction between sodium sulfide and copper(Il) sulfide: NazS (aq) + Cuso4 (aq) -> NazSO4(aq) + CuS (s) A chemist allows 16.7 g of Na,S and 35.0 g of CuSO, to react. Determine the theoretical yield of NazSO4 for the reaction. 31.1 20.5 30.4 O 21.0

Consider the reaction between sodium sulfide and copper(Il) sulfide: NazS (aq) + Cuso4 (aq) -> NazSO4(aq) + CuS (s) A chemist allows 16.7 g of Na,S and 35.0 g of CuSO, to react. Determine the theoretical yield of NazSO4 for the reaction. 31.1 20.5 30.4 O 21.0

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

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 7RQ: Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation?...

See similar textbooks

Related questions

Q: 4. Consider the reaction between sulfur trioxide and water: SO3 (g) + H2O (1) → H2SO4 (aq) A chemist…

A: 4) Given, SO3(g) + H2O(l) ➝ H2SO4(aq) mass of SO3 react = 61.5 g mass of H2O react = 11.2 Actual…

Q: Consider the following fictitious reaction. If the reaction begins with 0.362 mol of A and the…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: Consider the following reaction between sulfur trioxide and water: SO3(g)+H2O(l)→H2SO4(aq) A…

Q: Consider the balanced chemical reaction below. What is the maximum amount of grams of Fe that can be…

A: • Number of moles = Given massMolar Mass• Mass = No.of moles x molar mass• Molar mass of Fe2O3 = 2 x…

Q: 10.0 grams of methane is burned in an excess of oxygen and the reaction forms 19.8 grams of water in…

A: The percentage yield of a product in a reaction is the percentage of that product obtained compared…

Q: What is the percent yield of a reaction if the product recovered is 21.2 g and the theoretical yield…

A: The correct options are as follows:

Q: A student performed the synthesis of aspirin and started with 3.96 g of salicylic acid. The…

Q: 1. Write the balanced equation for the formation of lithium nitride from pure lithium metal and…

A: Limiting reactant :- A reactant which is present in lesser number of moles than required as per…

Q: When 11.5 g of C reacts with 114.5 g of Cu2O, 87.4 g of Cu are obtained. Determine the limiting…

A: Given, Amount of C = 11.5 g Amount of Cu2O = 114.5 g Cu obtained from reaction or actual yield of…

Q: Consider the balanced equation for the combustion of benzene, CóH6 - 2 C,H6 + 15 O2 → 12 CO2 + 6 H2O…

A: The number of moles required of a particular species to react with other species to yield a given…

Q: Consider the reaction between sulfur trioxide and water:SO3( g) + H2O(l) → H2SO4(aq)A chemist allows…

A: Given information, Mass of SO3 = 61.5 g Mass of H2O =11.2 g Mass of H2SO4 = 54.9 g

Q: Titanium can be obtained from its oxide by the reaction shown here. When 42.0 g of TiO, react with…

A: Given: mass of TiO2 = 42.0 g mass of C = 11.5 g mass of Ti obtained, =18.7 g

Q: . Consider the reaction between NiS2 and O2:2 NiS2(s) + 5 O2( g) → 2 NiO(s) + 4 SO2( g)When 11.2 g…

A: Given data Reaction : 2 NiS2(s) + 5 O2( g) → 2 NiO(s) + 4 SO2( g) mass of NiS2 reacts = 11.2 g mass…

Q: Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced…

A: In order to find the theoretical yield and percent yield we first write down the given data: Mass of…

Q: An aqueous solution containing 3.89 g of sodium phosphate was mixed with an aqueous solution…

A: The question is based on the concept of Reaction Stoichiometry. We have to identify the limiting…

Q: Using the mass of sodium bicarbonate used for runs 1 and 2, calculate the theoretical yield of solid…

Q: 5. Consider the reaction between HCI and O2: 4 HCI (9) + 02 (9) → 2 H2O (1) + 2 Cl2 (g) When 63.1 g…

Q: Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with…

A: The given reaction is, 4HCl(aq)+MnO2(s)⟶MnCl2(aq)+2H2O(l)+Cl2(g) Clearly, from…

Q: Consider the following chemical reaction: AgNO3 (aq) + K2CrO4 (aq) -----------> Ag2CrO4(s) +…

Q: Consider the balanced chemical reaction below. If 24.3 g of iron is produced when 50.0 g of…

A: The amount of substance is usually defined in terms of mole. The mole is the SI unit of the quantity…

Q: Iron reacts with oxygen at high temperatures to form iron(III) oxide.…

A: The given reaction is, Number of moles of reactants is calculated.

Q: 1) How many grams of N2(g) can be made from 9.05 g of NH; reacting with 45.2 g CuO? 2 NH:(g) + 3…

Q: Consider the combination reaction: 2 Al(s) + 3 Br2(1) 2 AIBr3(s) ----> Suppose the actual yield of…

A: We have to predict the theoretical yield.

Q: If the reaction below produces 3.82 gram of barium sulfate and the theoretical yield is 4.15 grams,…

A: Given Chemical Reaction :: Ba(NO3)2 (aq) + CuSO4 (aq) --> Cu(NO3)2 (aq) + BaSO4 (s)

Q: Consider the following reaction Ca(s) + 2HCI(aq) --> CaCl2(aq) + H2(8) If the theoretical yield of…

A: given, theoretical yield = 0.736 g actual yield = 0.720 g

Q: Chemistry Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide…

A: Given, Gaseous methane (CH4) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide…

Q: Consider the reaction: 4A + 3B - 3C + 4D A student in our chemistry laboratory mixes 6.4 mol…

A: The limiting reagent in a reaction is a reactant that is totally consumed when the reaction is…

Q: In mining, roasting is the oxidation of metal sulfides to produce metal oxides and sulfur dioxide, a…

Q: 6. Magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. The…

A: The balance chemical reaction : 2Mg(s) + O2(g) ---> 2MgO(s) Mass of Mg = 10.1 g Mass of O2 =…

Q: Calcium carbonate is heated. Calcium oxide and carbon dioxide gas are formed. The equation for the…

A: 225 kg of Calcium carbonate is heated until it decomposes completly to CaO and CO2. Yield of CaO =…

Q: The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O: 4NH3(g) + 7O2(g)…

A: Chemical Reaction Involved: 4NH3(g) + 7O2(g) -------> 4NO2(g) + 6H2O(g)

Q: SO3 (g) + H2O (l) à H2SO4 (aq) A chemist allows 61.5 g of SO3 and 11.2 g of H2O to react. When…

A: The reaction in which the reactant is totally consumed when the reaction is completed is known as…

Q: Magnesium oxide can be made by heating magnesium metal in the presence of oxygen according to the…

Q: Consider the following reaction: 2 K(s) + S(s) + 2 O2(g) --> K2SO4(s) If you start off with…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

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

Q: Consider the balanced chemical reaction below. If 24.3 g of iron is produced when 50.0 g of…

A: Molar mass of Fe2O3 =(56×2+16×3) g/mol = 160 g/molMolar mass…

Q: Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with…

Q: For the reaction shown, compute the theoretical yield of the product (in moles) for each of the…

A: Given:Balanced chemical reaction:

Q: Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with…

A: Given:4HCl(aq)+MnO2(s)⟶MnCl2(aq)+2H2O(l)+Cl2(g)

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

A: Welcome to bartleby !

Q: The ethane gas(C2H6) with chlorine gas produces C2h5Cl as its main product (along with HCl). In…

Q: In preparing a paint pigment of chrome yellow, PbCrO4, student used 6.94 of Pb(NO 3 ) 2 and K 2 CrO…

A: The chemical reaction between lead nitrate and K2CrO4 is shown below and the theoretical yield for…

Q: Consider the balanced chemical reaction below. If 24.3 g of iron is produced when 50.0 g of…

A: The amount of iron(III) oxide made to react with 50.0 g of carbon monoxide is 50.0 g. The amount of…

Q: Consider the reaction: 2 SO2(g) + O2(g) → 2 SO3(g) If 6.940 g SO2 is mixed with 17.41 g O2,…

A: The reaction given is 2 SO2(g) + O2(g) → 2 SO3(g) Hence from the above reaction, we can say that 2…

Q: Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with…

A: 1) First we will determine the limiting reactant : a) moles of MnO2 = ( Mass / Molar mass) moles…

Q: Methyl salicylate (oil of wintergreen) is prepared by heating salicylic acid, C, He Os, with…

A: Given that: Mass of salicylic acid = 1.40 g Mass of methanol = 13.1 g Actual yield of methyl…

Q: A chemist goes into the lab and performs an experiment in which a mixture of 8.47 grams of Zn and…

A: When two reactive compounds are mixed, then they react according to the stoichiometry of the…

Q: 100 g manganese dioxide reacts with 300g hydrochloric acid in the reaction shown bellow. MnO2 + 4…

A: A limiting reactant is the compound on the reactant side, which consumed completely during the…

Q: Use only 1 decimal point for atomic masses. Determine the yield (amount of product) of HCI(g) if 2.6…

A: The yield depends on the amount of limiting reagent. The given balanced chemical equation is: From…

Q: [References] The deep blue compound Cu(NH3)4SO4 is made by the reaction of copper(II) sulfate and…

A: Given, Mass of CuSO4 = 48.0 g

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

Consider the reaction between sodium sulfide and copper(Il) sulfide:
NazS (aq) + CuS04 (aq) -> Na2SO4(aq) + CuS (s)
A chemist allows 16.7 g of Na,S and 35.0 g of CUSO, to react. Determine the theoretical yield of
NazSO4 for the reaction.
31.1
20.5
30.4
O 21.0

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 2 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

A natural brine found in Arkansas has a bromide ion concentration of 5.00 × 10−3 M. If 210. g Cl2 were added to 1.00 × 103 L of the brine, determine the limiting reactant. calculate the theoretical yield of Br2 (d = 3.12 g/mL).
The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Small quantities of oxygen gas can be generated in the laboratory by the decomposition of hydrogen peroxide. The unbalanced equation for the reaction is H2O2(uz/)-? H2O(/) + O2(g) Calculate the mass of oxygen produced when 10.00 g of hydrogen peroxide decomposes.
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.
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.
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
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?
Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation? lf 2.50 moles of A2 are reacted with excess AB, what amount (moles) of product will form? If the mass of AB is 30.0 u and the mass of A2 are 40.0 u, what is the mass of the product? If 15.0 g of AB is reacted, what mass of A2 is required to react with all of the AB, and what mass of product is formed?
4.43 Magnesium nitride forms in a side reaction when magnesium metal burns in air. This reaction may also be carried out in pure nitrogen. 3Mg(s)+N2(g)Mg3N2(s) If 18.4 g of Mg3N2forms from the reaction of 20.0 g of magnesium with excess nitrogen, what is the percentage yield?
High cost and limited availability of a reactant often dictate which reactant is limiting in a particular process. Identify the limiting reactant when the reactions below are run, and come up with a reason to support your decision. a. Burning charcoal on a grill: C(s)+O2(g)CO2(g) b. Burning a chunk of Mg in water: Mg(s)+2H2O(l)Mg(OH)2(aq)+H2(g) c. The Haber process of ammonia production: 3H2(g)+N2(g)2NH3(g)
4.21 Ammonium nitrate, NH4NO3, will decompose explosively to form N2, O2, and H2O, a fact that has been exploited in terrorist bombings. What mass of nitrogen is formed by the decomposition of 2.6 kg of ammonium nitrate?