The reaction 2KCIO3 (s) 2KCI (s) + 302 (g) represents a common laboratory procedure for producing small quantities of pure oxygen. A 0.250-L flask is filled with O2 that has been collected over water at an atmospheric pressure of 729 torr. The temperature of the water and the gas is 14 °C. Calculate the molar volume of oxygen at 0 °C and 760 torr. Note: The vapor pressure of H2O at 14.0 °C is 12.0 torr. Hint: "molar volume" is expressed as L/mol

The reaction 2KCIO3 (s) 2KCI (s) + 302 (g) represents a common laboratory procedure for producing small quantities of pure oxygen. A 0.250-L flask is filled with O2 that has been collected over water at an atmospheric pressure of 729 torr. The temperature of the water and the gas is 14 °C. Calculate the molar volume of oxygen at 0 °C and 760 torr. Note: The vapor pressure of H2O at 14.0 °C is 12.0 torr. Hint: "molar volume" is expressed as L/mol

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Some commercial drain cleaners use a mixture of sodium hydroxide and aluminum powder. When the solid mixture is poured into the drain and dissolves, a reaction ensues that produces hydrogen gas : 2NaOH(aq)+2Al(s)+6H 2 O(l) 2NaAl(OH) 4 (aq)+3H 2 (g) Determine the pressure (in kPa) of hydrogen gas produced when 19.08 g of aluminum reacts with excess sodium hydroxide and water if the temperature is 28.22 C and the volume is 26.52 L. Provide your answer with TWO decimals.
A mixture of He and CO2 is placed in a 7.5L flask at 22C. The partial pressure of the He is 2.2 atm and the partial pressure of the CO2 is 1.9 atm. What is the mole fraction of He?
1) Calculate the volume of 1.62g of Helium gas at 25.670C and 872 mmHg. (R = 0.0821 atm.L/mol.K) 2) Given the following reaction of Ca(s) in HCl(aq): Ca(s) + 2 HCl(aq) --> CaCl2(aq) + H2(g) If 32.7g of calcium solid are placed in this reaction and at the end of the experiment, hydrogen gas is produced at 25.000C and with a pressure of 790. mmHg. Calculate the volume of hydrogen gas produced. 3) An unknown gas with a mass of 1.211g occupies a volume of 677 mL. The temperature is 230C and the air pressure is 0.987 atm. Calculate the molar mass of the gas.
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For the following reaction: C3H8(g) + 3CO₂(g) + 4H₂O(1) 502(g) The change in gaseous moles, An = To maximize the product yield, the volume of the container should ◆ , so that the pressure will be (> →
In an ideal gas experiment performed with some modifications, the students used0.029 g of aluminum foil instead of magnesium ribbon. They prepared the eudiometer by adding 6M HCl andfilling it with water to the brim. Once the setup was complete, they performed theexperiment. Note that the aluminum was completely consumed in the reaction.From the experiment, it was found that the external pressure was 1.05 atm at30.0 °C, and the volume of the air inside the eudiometer was 33.5 mL. The waterlevel inside the eudiometer is 4.15 cm below the surface of the water leveloutside. ● At 30.0 °C, Pvapor = 31.8 mmHg● R = 0.08206 L-atm/mol-K = 62.36 L-torr/mol-K● MWAl = 26.98 g/mol Find the value of the pressure of dry air (PDA) in torr and give the balanced chemical reaction of the aluminum metal with the acid.
Small amounts of oxygen can be generated by the thermal decomposition of KClO 3; 2 KClO 3(s) ↔ 2 KCl(s) + 3 O 2(g) A sample of KClO 3 was decomposed and oxygen collected over water at 26.00 °C (Vapor pressure = 25.21 torr). How many grams of KClO 3 decomposed if 1.032 L of gas were collected at 693.6 torr?
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Q1 (a) 3.2 g of sulphur was produced in a reaction between 6.0 L of hydrogen sulfide gas with excess an amount of sulphur dioxide. With the aid of Table Q1 (a)(i) and Table Q1 (a)(ii), predict the temperature (in °C) of the reaction if it was conducted at 750 torr. Element Actinium Aluminum Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Boron Bromine Cadmium Calcium Californium Carbon Cerium Cesium Chlorine Chromium Cobalt Copper Curiam CY с Ce Cs a Cr Co Ca Cm Dysprosium Dy Einsteinium Es Er Eu Fm F Fr Gd Ga Ge Erbium Europium Fermium Fluorine Francium Gadoliniam Gallium Germaniam Gold Hafnium Helium Holmium Hydrogen Indium Iodine Iridium Iron Krypton Lanthanam Lawrencium Lead Lithiam Lutetium Table Q1 (a)(i): Atomic Number and Atomic Mass of Elements Magnesium Manganese Symbol Ac Al Am Sb As Al Ba Bk Be Bi B Br Ca Hr He Ho H In I Ir Fe Kr La Lr Ph Li Lu Mg Mn Atomic number (2) 89 13 95 51 18 33 85 56 97 4 83 5 35 48 20 98 6 58 55 17 24 27 29 96 66 99 68…
Calculate the molarity of a solution containing 241 grams of NaCI in 1836 ml of solution? (Atomic masses of Na=23 and Cl=35.5) Answer:
A sample of Cl2 with a pressure of 1.84 atm and a volume of 290 mL is allowed to react with excess Br2 at 182 °C. Br2 (g) +Cl2 (g) --> 2BrCl (g) Calculate the pressure of the BrCl produced in the reaction if it is transferred to a 2.16-L flask and cooled to 32 °C