3. Kinetics study on the decomposition of phosphine at 950 K was done by injecting PH3 gas into a reaction vessel. Then, the total pressure at constant volume was measured. Given the balanced chemical reaction and data obtained in the study, 4 PH3 (g) - P4 (g) + 6 H₂ (g) PTotal (Torr) 100 150 167 172 Time (s) 0 40 80 120 a. Show the kinetic plots from zero- to second-order and select which order the reaction appears to obey using Linear Regression Analysis (R²) b. What is the rate law that describes this reaction?

3. Kinetics study on the decomposition of phosphine at 950 K was done by injecting PH3 gas into a reaction vessel. Then, the total pressure at constant volume was measured. Given the balanced chemical reaction and data obtained in the study, 4 PH3 (g) - P4 (g) + 6 H₂ (g) PTotal (Torr) 100 150 167 172 Time (s) 0 40 80 120 a. Show the kinetic plots from zero- to second-order and select which order the reaction appears to obey using Linear Regression Analysis (R²) b. What is the rate law that describes this reaction?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter5: Gases

Section: Chapter Questions

Problem 5.105PAE: 105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so...

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One of the chemical controversies of the nineteenth century concerned the element beryllium (Be). Berzelius originally claimed that beryllium was a trivalent element (forming Be3+ ions) and that it gave an oxide with the formula Be2O3. This resulted in a calculated atomic mass of 13.5 for beryllium. In formulating his periodic table, Mendeleev proposed that beryllium was divalent (forming Be2+ ions) and that it gave an oxide with the formula Be2O3. This assumption gives an atomic mass of 9.0. In 1894, A. Combes (Comptes Rendus 1894, p. 1221) reacted beryllium with the anion C5H7O2and measured the density of the gaseous product. Combess data for two different experiments are as follows: I II Mass 0.2022 g 0.2224 g Volume 22.6 cm3 26.0 cm3 Temperature 13C 17C Pressure 765.2 mm Hg 764.6 mm If beryllium is a divalent metal, the molecular formula of the product will be Be(C5H7O2)2; if it is trivalent, the formula will be Be(C5H7O2)3. Show how Combess data help to confirm that beryllium is a divalent metal.
Starting with the definition of rate of effusion and Graham’s finding relating rate and molar mass, show how to derive the Graham’s law equation, relating the relative rates of effusion for two gases to their molecular masses.
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
During the discussion of gaseous diffusion for enriching uranium, it was claimed that 235UF6 diffuses 0.4% faster than 238UF6. Show the calculation that supports this value. The molar mass of 235UF6=235.043930+618.998403=349.034348 g/mol, and the molar mass of 238UF6=238.050788+618.998403=352.241206 g/mol.
A sample of a smoke stack emission was collected into a 1.25-L tank at 752 mm Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass. What is the partial pressure exerted by each gas?
Consider a gas mixture containing equal concentrations of argon and helium. Without performing any calculations, determine which is higher: the number of collisions between helium and helium, the number of collisions between argon and argon, or the number of collisions between helium and argon?
5-56 The three main components of dry air and the percentage of each are nitrogen (78.08%), oxygen (20.95%), and argon (0.93%). (a) Calculate the partial pressure of each gas in a sample of dry air at 760 mm Hg. (b) Calculate the total pressure exerted by these three gases combined.
105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so unusual the process was once used in fireworks displays. There are actually several reactions that take place when the solid Hg(SCN)2 is ignited: 2Hg(SCN)2(s)2HgS(s)+CS2(s)+C3N4(s)CS2(s)+3O2(g)CO2(g)+2SO2(g)2C3N4(s)3(CN)2(g)+N2(g)HgS(s)+O2(g)Hg(l)+SO2(g) A 42.4-g sample of Hg(SCN)2 is placed into a 2.4-L vessel at 21°C. The vessel also contains air at a pressure of 758 torr. The container is sealed and the mixture is ignited, causing the reaction sequence above to occur. Once the reaction is complete, the container is cooled back to the original temperature of 21°C. (a) Without doing numerical calculations, predict whether the final pressure in the vessel will be greater than, less than, or equal to the initial pressure. Explain your answer. (b) Calculate the final pressure and compare your result with your prediction. (Assume that the mole fraction of O2 in air is 0.21.)
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
Given that 1.00 mol of neon and 1.00 mol of hydrogen chloride gas are in separate containers at the same temperature and pressure, calculate each of the following ratios. (a) volume Ne/volume HCI (b) density Ne/density HCI (c) average translational energy Ne/average translational energy HCI (d) number of Ne atoms/number of HCl molecules
Sulfur-containing compounds give skunks their potent smell. One of the principal smelly compounds in skunk spray is (E)-2-butene-1-thiol, C4H7S. a What is the root-mean-square (rms) molecular speed of a gas molecule of this compound at 25C? b Using the value from part a, calculate how long it would take a molecule of C4H7S to reach your nose if you were 150 m from the skunk. c Does the calculation that you performed in part b provide an accurate estimate for the length of time it would take for the molecule to travel 150 m, or is there something that was overlooked in performing the calculation?