In test tube #1, you will add 2.0 mL of 0.20 M K2S208, and 2.0 mL of 0.010 M Na2S203, alongwith the other reactants and spectator ions specified in Table 6.1.7)molsRecalling that moles = M × V =answer the following. Show all work and units.(a) Calculate the number of moles of persulfate ion (S20g²) ion initially present in test tube 1(b) Calculate the number of moles of thiosulfate ion (S203²) initially present in test tube 1

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Answered: In test tube #1, you will add 2.0 mL of…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 35QRT

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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.
Graphite is burned in oxygen to give carbon monoxide and carbon dioxide. If the product mixture is 33% CO and 67% CO2 by mass, what is the heat from the combustion of 1.00 g of graphite?
A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. 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 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.
A possible practical way to eliminate oxides of nitrogen(such as NO2 ) from automobile exhaust gases uses cyanuricacid, C3N3(OH)3 . When heated to the relatively lowtemperature of 625°F, cyanuric acid converts to gaseousisocyanic acid (HNCO). Isocyanic acid reacts with NO2 inthe exhaust to form nitrogen, carbon dioxide, and water,all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, howmuch cyanuric acid (in kilograms) would be requiredto absorb the 1.71010kgNO2 generated annuallyin auto exhaust in the United States?
If the density of both and solutions is 1.0 g/mL, what is the total mass of the solutions added to the insulated container? given information: concentration: 1.0 M molecular reaction: HCl (aq) + NaOH (aq) ---> NaCl (aq) + H2O (aq) d H = -56 kJ/mol liters of sodium hydroxide used: .2 L liters of hydrochloric acid used: .2 L moles NaOH reacted: .2 mol moles HCl reacted: .2 mol moles of water formed: .2 mol
In a combustion reaction, one of the reactants is always
Industrial production of nitric acid, which is used in many products including fertilizers and explosives, approaches 10 billion kg per year worldwide. The first step in its production is the exothermic oxidation of ammonia, represented by the following equation. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) ΔH⁰rxn = −902.0 kJ If this reaction is carried out using 7.007 ✕ 103 g NH3 as the limiting reactant, what is the change in enthalpy?
Calculate the amount (mol) of sucrose that reacted.Molar mass of sucrose = 342.3 g/molDelta*T = 2.14 deg * Cq_water = 5.37 kJq_cal = 0.899 kJ
Why is it important to give the physical states of the reactants and productswhen giving an equation ofΔH?
Suppose you had used 4.00 grams of NaOH(s) in Reaction 1. What would have been the number of Joules released in the reaction? What effect would this have on the value of X1?
22. A recipe for 1 cup of hollandaise sauce calls for ½ cup of butter, ¼ cup of hot water, 4 egg yolks, and the juice of a medium-sized lemon. How many cups of this sauce can be made from a pound (2 cups) of butter, a dozen eggs, 4 medium lemons, and an unlimited supply of hot water? Write an equation for making sauce, then use dimensional analysis and the process used in class for dealing with limiting reagents. How much of each ingredient are in excess?
Phosphoric acid, which is commonly used as rust inhibitor, food additive and etching agent for dental and orthopedic use, can be synthesized using a two-step thermal process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P4 (l) + 5O2 (g) → 2P2O5 (g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P2O5 (g) + 3H2O (l) → 2H3PO4 (l) Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation is balanced

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