In 1897 the Swedish explorer Andreé tried to reach the North Pole in a balloon. The balloon was filled with hydrogen gas. The hydrogen gas was prepared from iron splints and diluted sulfuric acid. The reaction is Fe(s) + H2SO4(aq) → FeSO4(ag) + H2 (g) The volume of the balloon was 4800 m³ and the loss of hydrogen gas during filling was estimated at 10.%. What mass of iron splints and 98% (by mass) H2SO4 were needed to ensure the complete filling of the balloon? Assume a temperature of 0°C, a pressure of 1.0 atm during filling, and 100% yield. Mass of Fe = Mass of H2SO4 = g

In 1897 the Swedish explorer Andreé tried to reach the North Pole in a balloon. The balloon was filled with hydrogen gas. The hydrogen gas was prepared from iron splints and diluted sulfuric acid. The reaction is Fe(s) + H2SO4(aq) → FeSO4(ag) + H2 (g) The volume of the balloon was 4800 m³ and the loss of hydrogen gas during filling was estimated at 10.%. What mass of iron splints and 98% (by mass) H2SO4 were needed to ensure the complete filling of the balloon? Assume a temperature of 0°C, a pressure of 1.0 atm during filling, and 100% yield. Mass of Fe = Mass of H2SO4 = g

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

5) Consider the reaction below. Co(g) + 2H¿(g) → CH,OH(g) 1.5 L of hydrogen gas and 3.5 L of carbon monoxide gas, both at 45 °C and 1.28 atm are in separate containers separated by a value. When the value is opened the two gases mix and react, according to the above reaction. a) Please determine the limiting reagent and the theoretical yield. b) If the percent yield is 67.3%, what is the concentration of the product in the final reaction mixture? c) What is the partial pressure of the product in the final reaction mixture?
The human body burns glucose (C6H12O6) for energy according to this chemical reaction: C6H12O6+6O2→ 6CO2+6H2O The products of the reaction are carbon dioxide CO2 and water H2O Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500.mL of air, which is typically enriched to 4% CO2 and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 0.50kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO2 is 2.0 kg/m^3 .
a 2.802g sample of an unknown pure metal (M) is added to a 0.2 L solution of 2 mol/L H2SO4(aq). The metal reacts with the acid until the metal is completely gone to form M3+(aq) ion in the solution and produces hydrogen gas that is collected. The hydrogen gas that is collected over water that is isolated from the reaction has a volume of 0.82 L at 25 degrees Celsius and a total pressure of 704.0 mmHg. How many moles of H2(g) are produced? Write a balanced equation for the reaction of M with H2SO4(aq). What is the identity of metal M?
A gas phase reaction occurs in a syringe at constant temperature and pressure. If the initial volume in the syringe is 12.3 mL and the final volume is 4.1 mL, which of the following general reactions could have occurred? a) A(g) + B(g) → AB(g) b) 2A(g) + B(g) → A2B(g) c) 2AB(g) → A2(g) + 2B(g) d) 2AB (g) → A2(g) + B2(g) e) 2A2(g) + 4B(g) → 4AB(g) a e
Three bulbs are connected by tubing, and the tubing is evacuated. The volume of the tubing is 49.0 mL The first bulb has a volume of 58.0 ml and contains 6.07 atm of argon, the second bulb has a volume of 250 ml. and contains 1.62 atm of neon, and the third bulb has a volume of 27.0 ml. and contains 7.72 atm of hydrogen. If the stopcocks (valves) that isolate all three bulbs are opened, what is the final pressure of the whole system in atm? Answer:
12. A piece of sodium (Na) metal reacts completely with water to produce NaOH(aq) and H₂(g). The H₂(g) generated is collected over water at 25.0°C. (Vapor pressure of water at 25°C is 0.0313 atm) The volume of the gas is 246 mL measured at normal atmospheric pressure. Calculate the mass (in grams) of Na (MM = 22.99) used in the reaction. 13. Ammonia (NH₁) burns in oxygen gas to form nitric oxide (NO) and water vapor. How many liters of oxygen will react with 8.00 L of ammonia at the same temperature and pressure?
A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.
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…
Nitesh
73. A 500.-mL sample of O2 gas at 24 °C was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2 O2, in the presence of a small amount of manganese catalyst by the reaction 2H2 O2 (aq) → 2H2O (g) + The oxygen thus prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2 in the mixture? How many moles of O2 are in the mixture? (The vapor pressure of water at 24 °C is 23 mm Hg.)
The concentration of an old solution of hydrogen peroxide is being tested because hydrogen peroxide decomposes over time. The following reaction is catalyzed by potassium iodide and used to determine the concentration. If 3.0 ml of the peroxide solution is tested and produces 55 ml of O2(g) at 750 mm Hg and 23˚C, how many grams of hydrogen peroxide were in the solution? 2 H2O2(aq) à 2 H2O(l) + O2(g)
Hydrogen gas can be prepared by the reaction of zinc metal with dilute aqueous hydrochloric acid: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) How many moles of hydrogen would be produced in the reaction if 7.90 g of zinc reacts? What volume of H2 would be produced in this reaction under standard conditions (25°C and 1.013 x 105 Pa)?