A student collected 20.31 mL of H2 over water at 30.00°C. The water level inside the collection apparatus was 8.1 cm higher than tl water level outside. The barometric pressure was 702 torr. How many grams of zinc had to react with HCl(ag) to produce the H2 that was collected? You may need the data in the table to solve this problem.

A student collected 20.31 mL of H2 over water at 30.00°C. The water level inside the collection apparatus was 8.1 cm higher than tl water level outside. The barometric pressure was 702 torr. How many grams of zinc had to react with HCl(ag) to produce the H2 that was collected? You may need the data in the table to solve this problem.

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...

See similar textbooks

Similar questions

A student collects 69.2 mL of hydrogen gas from the reaction of 0.082 grams of magnesium solid with excess hydrochloric acid. The actual volume of hydrogen collected corrected to STP conditions is 62.5 mL. What would be the percent yield of hydrogen gas collected in this reaction. (HINT: you need to find the theoretical yield of hydrogen first.) The mole ratio of magnesium to hydrogen is 1:1.
Hydrogen gas generated from the reaction of aluminum with hydrochloric acid was collected over water at 20°C. If 26.5 mL of gas was collected at an atmospheric pressure of 0.875 atm, how many mmol (millimoles) of hydrogen were collected? The vapor pressure of water at 20°C is 17.55 torr. Give your answer to 3 sig figs. 2 Al(s) + 6 HCl(aq) -> 2 AlCl3(aq) + 3 H2 (g)
A student collected 500. mL of nitrogen at a temperature of 20.°C. The next day the student found that the volume had changed to 525 mL. What was the new temperature of the gas?
A student collected 17.14 ml of H₂ over water at 25.00 °C. The water level inside the collection apparatus was 9.5 cm higher than the water level outside. The barometric pressure was 736 torr. How many grams of zinc had to react with HCl(aq) to produce the H₂ that was collected? You may need the data in the table to solve this problem. mass= gZn Table 10.2 Vapor Pressure of Water at Various Temperatures Temperature Vapor Pressure Temperature Vapor Pressure (C) (torr) (C) (torr) 0 4.579 50 92.51 5 6.543 55. 118.04 10. 9.209 60 149.38 15 12.788 65 187.54 20 17.535 70 233.7 25 23.756 75 289.1
A 10.0 L vessel at 298 K contains O2(g) at a pressure of 740. mmHg. What mass of He(g) would be added to increase the total pressure to 1480. mmHg?
A student collected 10.48 mL of H2 over water at 20.00 ºC. The water level inside the collection apparatus was 8.1 cm higher than the water level outside. The barometric pressure was 725 torr. How many grams of zinc had to react with HCl(aq) to produce the H2 that was collected? You may need the data in the table to solve this problem. Temperature (0C) Vapor Pressure 20 17.535 mass= ___g Zn
The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4240 L of hydrogen gas at STP, heat the mixture to run the reaction, then separate the ammonia from the reaction mixture. What volume of reactant, measured at STP, is left over? Assume the reaction goes to completion. N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)
Given the reaction: 2 Al (s) + 6 HCI (ag) --> 2 AICI3 (aq) + 3 H2 (g) A strip of aluminum of unknown mass is reacted with excess hydrochloric acid. When the hydrogen gas is collected over water, it is done so at a temperature of 22.0 °C and fills a flask of volume 32.5 mL. The pressure inside the collection tube is 756.1 mmHg and the water vapor pressure at 22.0 °C is 19.83 torr. Determine the mass of the aluminum strip in milligrams (mg).
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…
A sample of H2(g) was collected over water in a volume of 12.0 mL at 18 °C under atmospheric pressure of 770. Torr. Partial pressure of water is P(H2O, 18 °C) = 16 Torr. Find the mol’s of H2(g) in the sample
@
A sample of 328.1 mL of wet nitrogen gas was collected over water at a total pressure of 761 torr and a temperature of 21.0 °C. (The vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH2SO3, with 404.3 mL of a solution of sodium nitrite according to the following equation. NANO2 + HNH2SO3¬ N2 + NaHSO4 + H2O Calculate what must have been the molar concentration of the sodium nitrite.