Hydrogen chloride molar mass

Eleven elements are gases under normal conditions (Fig. 4.2). So are many compounds with low molar masses, such as carbon dioxide, hydrogen chloride, and organic compounds such as the methane, CH4, of natural gas and the... 

FIGURE 4.22 The plug on the left is soaked in hydrochloric acid and that on the right in aqueous ammonia. Formation of ammonium chloride occurs where gaseous hydrogen chloride and ammonia meet. The reaction occurs closer to the HC1 plug because HC1 has the greater molar mass and thus its molecules diffuse more slowly. 

Ammonia has a molar mass of 17.0 g/mol hydrogen chloride has a molar mass of 36.5 g/mol. What is the ratio of their diffusion rates ... 

You are given the molar masses for ammonia and hydrogen chloride. To find the ratio of the diffusion rates for ammonia and hydrogen chloride, use the equation for Graham s law of effusion. 

Ammonia molecules diffuse about 1.5 times as fast as hydrogen chloride molecules. This ratio is logical because molecules of ammonia are about half as massive as molecules of hydrogen chloride. Because the molar masses have three significant figures, the answer does, too. 

Intermolecular reactions between carbon-centred radicals on adjacent chains will produce crosslinking, which will compete with the chain-scission and intramolecular reactions. The effect on the molar-mass distribution will depend on the competition between these reactions. For example the poly(acrylates) will preferentially crosslink rather than degrade and the recovery of monomer from these polymers is less than 1%, compared with close to 100% for poly(methacrylates). Poly(vinyl chloride) (PVC) is also a polymer that undergoes crosslinking in preference to scission, but the major observation of importance is the rapid elimination of hydrogen chloride by an auto-catalysed reaction as shown in Scheme 1.53. This is discussed in more detail later. 

The density of a gas depends on temperature, pressure, and the molar mass of the substance. When two gases are at the same pressure and temperature, the ratio of their densities should be the same as the ratio of their molar masses. The molar mass of ammonium chloride is 53.5 g/mol, and the ratio of this to the molar mass of molecular hydrogen (2.02 g/mol) is 26.8. The experimental value of 14.5 is roughly half this amount. Snch results usually indicate breakup or dissociation into smaller molecules in the gas phase (note the temperatnre). The measured molar mass is the average of all the molecules in equihbrinm. 

Stream Information. Directed arcs that represent the streams, with flow direction from left to right wherever possible, are numbered for reference. By convention, when streamlines cross, the horizontal line is shown as a continuous arc, with the vertical line broken. Each stream is labeled on the PFD by a numbered diamond. Furthermore, the feed and product streams are identified by name. Thus, streams 1 and 2 in Rgure 3.19 are labeled as the ethylene and chlorine feed streams, while streams 11 and 14 are labeled as the hydrogen chloride and vinyl-chloride product streams. Mass flow rates, pressures, and tempera-mres may appear on the PFD directly, but more often are placed in the stream table instead, for clarity. The latter has a column for each stream and can appear at the bottom of the PFD or as a separate table. Here, because of formatting limitations in this text, the stream table for the vinyl-chloride process is presented separately in Table 3.6. At least the following entries are presented for each stream label, temperature, pressure, vapor fraction, total and component molar flow rates, and total mass flow rate. In addition, stream properties such as the enthalpy, density, heat capacity, viscosity, and entropy, may be displayed. Stream tables are often completed using a process simulator. In Table 3.6, the conversion in the direct chlorination reactor is assumed to be 100%, while that in the pyrolysis reactor is only 60%. Furthermore, both towers are assumed to carry out perfect separations, with the overhead and bottoms temperatures computed based on dew- and bubble-point temperatures, respectively. 

EXERCISE 3.73 hi an industrial process, hydrogen chloride, HCl, is prepared by burning hydrogen gas, H2, in an atmosphere of chlorine, CI2. Write the chemical equation for the reaction. Below the equation, give the molecular, molar, and mass intepretations. 

The relative masses of the reactants and products of a chemical reaction can be determined from the reaction s coefficients. Recall that an amount of an element or compound in moles can be converted to a mass in grams by multiplying by the appropriate molar mass. We know that 1 mol of hydrogen reacts with 1 mol of chlorine to yield 2 mol of hydrogen chloride. The relative masses of the reactants and products are calculated as follows. 

At the end of the 1930s, the cationic polymerization as well has been attempted by Schlack, who discovered that anhydrous hydrogen chloride was capable of initiating the polymerization of CL. However, for reasons unknown at that time, the acid-initiated reartion did not yield high-quality PA6 and was therefore considered to be of no interest for commercial purposes. As a matter of fact, the cationic mechanism of lactam polymerization has always found very limited applications, if any, not only because of the low conversions and the low molar masses of the resultant polyamides but also for the extensive occurring of side reactions. 

Figure 5.9 Relation of molecular speed to molar mass. When ammonia gas, which is injected into the left arm of the tube, comes in contact with hydrogen chloride, which is injected into the right arm of the tube, they react to form solid ammonium chloride NHsCg) + HCI(g) — NH4CI(s). Because NH3 (MM = 17 g/mol) moves faster than HCI (MM = 36.5 g/mol), the ammonium chloride forms closer to the HCI end of the tube.

Hydrochloric acid oxidizes zinc metal in a reaction that produces hydrogen gas and chloride ions. A piece of zinc metal of mass 8.5 g is dropped into an apparatus containing 800.0 mL of 0.500 M HCl(aq). If the initial temperature of the hydrochloric acid solution is 25°C, what is the final temperature of this solution Assume that the density and molar heat capacity of the hydrochloric acid solution are the same as those of water and that all the heat is used to raise the temperature of the solution. 

PRACTICE EXAMPLE B Zinc metal and aqueous hydrochloric acid, HCl(aq), react to give hydrogen gas, Hjfg), and aqueous zinc chloride, ZnCl2(aq). A 0.4000 g sample of impure zinc reacts completely when added to 750.0 mL of 0.0179 M HCl. After the reaction, the molarity of the HCl solution is determined to be 0.00403 M. What is the percent by mass of zinc in the sample ... 

---