molecules by the action of the solvent. For example: HCI>H*(aq) + Cl'(aq) Hydrochloric acid (HCI) is an ionic compound that is broken down into two ions: Hydrogen (H*) and Chlorine (Cl). An ionic compound contains a cation with a positive charge (H*) and an anion with a negative charge (Cl). For a compound to go through ionization (be broken down into ions), it must be an ionic compound. Note that molecular compounds to not go through ionization. 1. What two classes of elements make up molecular compounds? 2. What classes of elements make up ionic compounds?

molecules by the action of the solvent. For example: HCI>H(aq) + Cl'(aq) Hydrochloric acid (HCI) is an ionic compound that is broken down into two ions: Hydrogen (H) and Chlorine (Cl). An ionic compound contains a cation with a positive charge (H*) and an anion with a negative charge (Cl). For a compound to go through ionization (be broken down into ions), it must be an ionic compound. Note that molecular compounds to not go through ionization. 1. What two classes of elements make up molecular compounds? 2. What classes of elements make up ionic compounds?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.101QE: In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is...

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In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
The reaction of solid calcium fluoride and sulfuric acid produces calcium sulfate solids and gaseous HF. The gas product is dissolved in water to form hydrofluoric acid. Fluorite ore, a source of calcium fluoride, contains 95%wt CaF2 and 5%wt SiO2. In a certain process, the ore is reacted with 93%wt aqueous sulfuric acid, supplied 15% in excess. From this, 95% of the ore dissolves in the acid. Some of the HF formed reacts with the dissolved silica in the reaction: HF reacts with SiO2 to produce H2SiF6 and liquid water. If 60%wt of hydrofluoric acid was formed when hydrogen fluoride (which exits the reactor) is dissolved in water, determine the amount of ore needed to produce one metric ton of acid. Report your answers to one decimal place only.
The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. a.) What is qH2O? b.) What is qrxn c.) What is ΔHrxn? d.) Is the reaction endothermic or exothermic?
Magnesium +Acetic Acid --> C2HG5+ O2 ---> Iron (III) carbonate -->
The manufacture of nitrogen trifluoride is a growing industry, due to its use as a plasma etchant in the semiconductor industry. Nitrogen trifluoride can be synthesized by passing a currentthrough a high-temperature mixture of ammonium fluoride and hydrogen fluoride, withhydrogen gas as a byproduct. In one synthesis, 1.20x103g ammonium fluoride is reacted with1.20x103g hydrogen fluoride to produce 5.00x102g nitrogen trifluoride. What is the limitingeactant, excess reactant, theoretical yield of nitrogen trifluoride, percent yield, and mass ofxcess reactant remaining after the reaction?
1. One of the first families of rockets used by the American space program was the Redstonefamily of rockets. The first Redstone rockets (in the 1950s) used B10H14 (often called decaborane)as a rocket fuel that reacts violently with liquid di-oxygen to make diboron trioxide and steam.When used as a rocket fuel, scientists carefully calculated the amount necessary so that bothcomponents ran out at the same time. (Excess fuel would be excess weight for the rocket tocarry.) If the total mass of both reactants put together is 12.0  104 kg, what was the volume ofliquid di-oxygen carried by the rockets? (Liquid di-oxygen has a density of 1.141 g/mL.)
Coal-fired power plants emit CO2, which is one of the gases that is of concern with regard to global warming. A technique that power plants can adopt to keep most of the CO2 from entering the air is called CO2 capture and storage (CCS). If the incremental cost of the sequestration process is $0.019 per kilowatt-hour, what is the present worth of the extra cost over a 3-year period to a manufacturing plant that uses 100,000 kWh of power per month? The interest rate is 12% per year compounded quarterly.
Use the following atomic masses (in g/mol): K = 39.1; Mn = 54.94; O = 16; H = 1; P = 30.97; C = 12.01; Na = 23; Mg = 24.31; S = 32.06; Zn = 65.38; Cu = 63.55 In the standardization of Hydrochloric Acid against pure anhydrous Sodium Carbonate, 1mL was found to be equivalent to 0.05g of the primary standard. Compute for the normality of the acid.
The last calculation we need to do is find the %acetic acid (a.k.a the "acidity"). We can average all of the acetic acid masses from the completely reacted samples in the previous step. For now, let's assume we ended up with a final average mass of 2.37 g acetic acid consumed. If the initial volume of acetic acid used was 50.0 mL, what's the %m/v of acetic acid?
When two cotton plugs, one moistened with ammonia and the other with hydrochloric acid, are simultaneously inserted into opposite ends of a glass tube that is 87.0 cm long, a white ring of NH4Cl forms where gaseous NH3 and gaseous HCl first come into contact.NH3(g) + HCl(g) ⟶ NH4 Cl(s)At approximately what distance from the ammonia moistened plug does this occur?
When 25 g of ethanol (MW 46.07 g/mol) is mixed with 25 g of water (MW 18.02 g/mol) at 25 C, the total volume of the ethanol/water solution is 50 mL. Given that the partial molar volume of water in the solution is 17.4 mL / m ol, what is the partial molar volume of the ethanol?
A student measured qrxn for the reaction of 0.492 g of a metal, X(s)(molar mass = 81.72), with HCl(aq) to be -874 J. Assuming this metal reacts in the same manner as magnesium, what is the ΔH°f (in kJ/mol) for this metal's cation in solution, i.e., X2+(aq)? Report your answer to the correct number of significant figures and only include the numerical answer

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