When heated, potassium chlorate (KC103) has a melting point of 355 °C and it decomposes in the temperature of 480 °C . Potassium chlorate (KC103(s)) then decomposes to KCI(s) and 02(g) in the presence of MnO2(s) catalyst. MnO2(s) does not participate in the overall chemical process, though. To determine the gas constant, the experiment used 100. mg of MnO2(s) and 1.300 g of pure KCIO3(s), then they were combined together in a test tube and heated over a bunsen burner. The resultant O2(g) product was collected in a 100-mL eudiometer after being bubbled in distilled water at exactly 25 °C (or 298.15 K). The experiment was carried out at a 755 torr barometric pressure. At 25 °c, the water vapor has a vapor pressure of 23.8 mmHg. The heat was removed after a few seconds of reaction, and the contents of the test tube containing the remaining KCI03(s), Mn02(s) catalyst, and the KCl product were weighed to be 1.285 g.The liquid level in the eudiometer is 1.36 cm below the reservoir's water level. The trapped gas is 88.57 mL, according to the eudiometer's graduation. iii) In mmHg, compute the partial pressure of the collected 02 iv.) Compute the experimental value for the ideal gas constant,R. Use the unit L * atm * mol-1 * K

When heated, potassium chlorate (KC103) has a melting point of 355 °C and it decomposes in the temperature of 480 °C . Potassium chlorate (KC103(s)) then decomposes to KCI(s) and 02(g) in the presence of MnO2(s) catalyst. MnO2(s) does not participate in the overall chemical process, though. To determine the gas constant, the experiment used 100. mg of MnO2(s) and 1.300 g of pure KCIO3(s), then they were combined together in a test tube and heated over a bunsen burner. The resultant O2(g) product was collected in a 100-mL eudiometer after being bubbled in distilled water at exactly 25 °C (or 298.15 K). The experiment was carried out at a 755 torr barometric pressure. At 25 °c, the water vapor has a vapor pressure of 23.8 mmHg. The heat was removed after a few seconds of reaction, and the contents of the test tube containing the remaining KCI03(s), Mn02(s) catalyst, and the KCl product were weighed to be 1.285 g.The liquid level in the eudiometer is 1.36 cm below the reservoir's water level. The trapped gas is 88.57 mL, according to the eudiometer's graduation. iii) In mmHg, compute the partial pressure of the collected 02 iv.) Compute the experimental value for the ideal gas constant,R. Use the unit L * atm * mol-1 * K

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

Chapter5: Gases

Section: Chapter Questions

Problem 102E: Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated...

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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.
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400C in a nickel reaction vessel. A 100.0-mL nickel container is filled with xenon and fluorine, giving partial pressures of 1.24 atm and 10.10 atm, respectively, at a temperature of 25C. The reaction vessel is heated to 400C to cause a reaction to occur and then cooled to a temperature at which F2 is a gas and the xenon fluoride compound produced is a nonvolatile solid. The remaining F2 gas is transferred to another 100.0-mL nickel container, where the pressure of F2 at 25C is 7.62 atm. Assuming all of the xenon has reacted, what is the formula of the product?
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 1111g of NH4Cl forms where gaseous NH3 and gaseous HC1 first come into contact. NH3(g)+HCl(g)NH4Cl(s) At approximately what distance from the ammonia moistened plug does this occur? (Hint: Calculate the rates of diffusion for both NH3 and HCI, and find out how much faster NH3 diffuses than HCI.)
A sample of gas in which [H2S] = 5.96 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.
Carbon dioxide gas is collected in a laboratory experiment to determine the molar mass of the compound. At 294 K and 1.01 atm, 1.008 g of CO2 was collected when a 500 mL flask was filled with the evolved CO2. What is the experimental molar mass of CO2?
Provide a particle level explanation for the following: when the temperature of a sealed, rigid (non-flexible) container is decreased, pressure also decreases.
Much to everyone"s surprise. nitrogen monoxide (NO) has been found to act as a neurotransmitter. To prepare to study its effect. a sample was col lected in a container of volume 300.0 cm3 At 14.5 oc its pressure is found to be34.5 kPa. What amount (in moles) of NO has been col lected?
2. A sample of vapor weighing 0.368 g filled a Florence flask when heated in a water bath at 95.0°C. The actual volume of the flask was 128.4 mL and the barometric pressure was 747 torr. Calculate (a) the volume of the vapor at STP and (b) the molar mass of the volatile liquid. (Use the approach applied in the Introduction and on the data sheet.)
A 2.00 L reaction container at 25.0 °C contains CO2 (g) and O2 (g). The total pressure of the gases in the container was 656 torr and the mole fraction of CO2 is 0.245. A)Calculate the partial pressure of oxygen gas in the mixture. B)Calculate the mass of oxygen gas in the mixture (in g). C)Which gas will rise to the top of the container? Explain your answer.
A container of volume 100.0 dm3 is divided into two (unequal) compartments. In the left compartment there are 2.0 mol of N2 at 1.0 atm and 25 degrees C; in the right compartment there are 3.0 mol of O2 at the same T and p. What are deltaG, deltaS and deltaH for the process occurring when the partition is removed. Assume that the gases are perfect.
What is the partial pressure (in atm) of CO2 at 468.2 K in a 25.0 L fuel combustion vessel if it contains 64.0 grams CO2, 82.1 g H₂O, and 7.30 mol vaporized, yet uncombusted fuel?