Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Chapter 5, Problem 33QAP
Dichlorine oxide is used as bactericide to purify water. It is produced by the chlorination of sulfur dioxide gas.
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2. Given the following equation:3 NO2 (g)+ H2O(l)2 HNO3 (aq)+ NO(g)Assume STPa. What mass of water is required to react with 15.5 L of Nitrogen dioxide?b. What volume of Nitrogen monoxide would be produced from 100.0 g of water?c. If 42.0 L of NO(g)is produced, what volume of NO2 (g)reacted?d. How many water atoms would be required to react with an excess ofNitrogen dioxide to produce 46.0 L of Nitrogen monoxide?
Consider the following equation, which represents the combustion of hydrogen sulfide.2H2S(g)+3O2(g)→2SO2(g)+2H2O(g)
a) What volume, in liters, of SO2 is formed when 137 L of H2S(g) is burned? Assume that both gases are measured under the same conditions.
b) What volume, in liters, of O2(g) is required to form 28 L of H2O(g)? Assume that both gases are measured under the same conditions.
Q2a. Sulfur dioxide (SO2), a gas that plays a central role in the formation of acid rain, is found in the exhaust of automobiles and power plants. Consider a 1.53L sample of gaseous SO2 at a pressure of 5.6 x 103 Pa. If the pressure is changed to 1.5 x 104Pa at a constant temperature, what will be the new volume of the gas?
b.If one molecule with the empirical formula C3H7 has a mass of 1.428 x 10-22 g, determine the molecular formula of the compound
Chapter 5 Solutions
Chemistry: Principles and Reactions
Ch. 5 - Prob. 1QAPCh. 5 - A 6.00-ft cylinder has a radius of 26 in. It...Ch. 5 - Prob. 3QAPCh. 5 - Prob. 4QAPCh. 5 - A cylinder with a movable piston records a volume...Ch. 5 - A tank is filled with gas to a pressure of 875 mm...Ch. 5 - A sample of CO2 gas at 22C and 1.00 atm has a...Ch. 5 - A sample of nitrogen gas has a pressure of 1.22...Ch. 5 - Prob. 9QAPCh. 5 - A tire is inflated to a gauge pressure of 28.0 psi...
Ch. 5 - Prob. 11QAPCh. 5 - A sealed tank at room temperature, 25C, has 22.0 g...Ch. 5 - A balloon filled with helium hasa volume of...Ch. 5 - Prob. 14QAPCh. 5 - Prob. 15QAPCh. 5 - Prob. 16QAPCh. 5 - A piece of dry ice (CO2(s)) has a mass of 22.50 g....Ch. 5 - A four-liter tank is filled with propane gas,...Ch. 5 - Prob. 19QAPCh. 5 - Prob. 20QAPCh. 5 - Calculate the densities (in g/L) of the following...Ch. 5 - Calculate the densities (in grams per liter) of...Ch. 5 - Helium-filled balloons rise in the air because the...Ch. 5 - Space probes to Mars have shown that its...Ch. 5 - Cyclopropane mixed in the proper ratio with oxygen...Ch. 5 - Phosgene is a highly toxic gas made up of carbon,...Ch. 5 - The gas in the discharge cell of a laser contains...Ch. 5 - Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2,...Ch. 5 - A 1.58-g sample of C2H3X3(g) has a volume of 297...Ch. 5 - A 0.750-g sample of the gas PX3 is in a sealed...Ch. 5 - Nitrogen oxide is a pollutant commonly found in...Ch. 5 - Nitrogen trifluoride gas reacts with steam to...Ch. 5 - Dichlorine oxide is used as bactericide to purify...Ch. 5 - Titanium(III) chloride is used in the manufacture...Ch. 5 - Nitric acid can be prepared by bubbling dinitrogen...Ch. 5 - Potassium peroxide is used to absorb the CO2...Ch. 5 - Hydrogen cyanide (HCN) is a poisonous gas. It can...Ch. 5 - When hydrogen peroxide decomposes, oxygen is...Ch. 5 - Ammonium nitrate can be used as an effective...Ch. 5 - Acetone peroxide, C9H18O6(s), is a powerful but...Ch. 5 - Prob. 41QAPCh. 5 - A certain laser uses a gas mixture consisting of...Ch. 5 - A sample of a smoke stack emission was collected...Ch. 5 - Prob. 44QAPCh. 5 - Prob. 45QAPCh. 5 - Prob. 46QAPCh. 5 - Prob. 47QAPCh. 5 - Follow the instructions of Problem 47 for the...Ch. 5 - When acetylene, C2H2, is burned in oxygen, carbon...Ch. 5 - When ammonium nitrate decomposes at 722C,...Ch. 5 - Prob. 51QAPCh. 5 - Nitrogen gas can be obtained by decomposing...Ch. 5 - Prob. 53QAPCh. 5 - Prob. 54QAPCh. 5 - Prob. 55QAPCh. 5 - Prob. 56QAPCh. 5 - A gas effuses 1.55 times faster than propane...Ch. 5 - A gas effuses through an opening one-fifth as fast...Ch. 5 - Prob. 59QAPCh. 5 - Prob. 60QAPCh. 5 - At what temperature will a molecule of uranium...Ch. 5 - Calculate the average speed of a (a) chlorine...Ch. 5 - Prob. 63QAPCh. 5 - Prob. 64QAPCh. 5 - Prob. 65QAPCh. 5 - Prob. 66QAPCh. 5 - Prob. 67QAPCh. 5 - Prob. 68QAPCh. 5 - Prob. 69QAPCh. 5 - Given that 1.00 mol of neon and 1.00 mol of...Ch. 5 - An intermediate reaction used in the production of...Ch. 5 - Prob. 72QAPCh. 5 - Prob. 73QAPCh. 5 - Glycine is an amino acid made up of carbon,...Ch. 5 - Prob. 75QAPCh. 5 - The Lamborghini Aventador engine has a 12-cylinder...Ch. 5 - Prob. 77QAPCh. 5 - Prob. 78QAPCh. 5 - Prob. 79QAPCh. 5 - Prob. 80QAPCh. 5 - Prob. 81QAPCh. 5 - Prob. 82QAPCh. 5 - Prob. 83QAPCh. 5 - The graph below shows the distribution of...Ch. 5 - Consider the following sketch. Each square in bulb...Ch. 5 - The following figure shows three 1.00-L bulbs...Ch. 5 - Prob. 87QAPCh. 5 - Prob. 88QAPCh. 5 - Prob. 89QAPCh. 5 - Prob. 90QAPCh. 5 - Prob. 91QAPCh. 5 - A 0.2500-g sample of an Al-Zn alloy reacts with...Ch. 5 - Prob. 93QAPCh. 5 - A mixture in which the mole ratio of hydrogen to...
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- 8. Calcium oxide is used to remove sulfur dioxide generated in coal-burning power plants according to the following reaction.2CaO(s)+2SO2(g)+O2(g)→2CaSO4(sWhat mass of calcium oxide is required to react completely with 1.4×103 L of sulfur dioxide?arrow_forwardThe great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 53.0mL of dioxygen gas are produced by this reaction, at a temperature of 50.0°C and pressure of exactly 1atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.arrow_forwardThe 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)arrow_forward
- . In the first step of the industrial process for making nitric acid, ammonia reacts with oxygen in the presence of a suitable catalyst to form nitric oxide and water vapor: 4NH3(g) + 5O2(g)→ 4NO(g) + 6H2O(g) How many liters of NH3(g) at 850 °C and 506.6 kPa are required to react with 1.00 mol of O2(g) in this reaction?arrow_forwardConsider the general chemical equation 2A+3B→5C+D. Part A. How many moles of C are produced from 2 mol of A? Express your answer as an integer and include the appropriate units. Part B. How many liters of gas B must react to give 1 L of gas D at the same temperature and pressure? Express your answer as an integer and include the appropriate units.arrow_forwardWhat volume of oxygen will react with 25 mL of ethanol, assuming the gases are present at the same temperature and pressure? Express the answer in mL, and write only the numerical value of the answer with the correct number of significant figures in the box. 2 CH3CH2OH(g) + 6 O2(g) → 4 CO2(g) + 6 H2O(g)arrow_forward
- An organic chemist isolates a colorless liquid from a petroleum sample. She places the liquid in a pre-weighed flask and puts the flask in boiling water, which vaporizes the liquid and fills the flask with gas. She closes the flask and reweighs it. She obtains the following data: Volume (V) of flask = 196 ml T = 99.1°C P= 751 mmHg mass of flask + gas = 81.5 g mass of flask = 78.3 g Calculate the molar mass (in g/mol) of the liquid.arrow_forward6.The combustion of propane gas produces carbon dioxide and water vapor.C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)What volume of oxygen is required to completely combust 0.650L of propane? What volume of carbon dioxide is produced in the reaction? (molar volume ratio is treated similarly like molar ratio)arrow_forwardConcrete is prepared by roasting the mineral calcium carbonate, CaCO3, to drive off CO2 and produce calcium oxide, CaO. The chemical equation for this reaction is: CaCO3 ==> CaO + CO2 The Grand Coulee Dam on the Columbia River in Washington State was built using a volume of concrete of approximately 1.0 x 107 m3. If concrete has a density of 2.4 x 103 kg/m3, and assuming concrete is 100% by volume CaO, how much CO2 was released producing the concrete used to build the dam?arrow_forward
- SO2 is a product of coal combustion. It may combine with O2 and H2O in the atmosphere to form sulfuric acid, a component of acid rain. One way to reduce the formation of acid rain involves trapping the SO2 by passing smokestack gases through a spray of calcium oxide and O2. The product of this reaction is calcium sulfate. a) Write a balanced chemical equation describing this reaction by writing the product and adding coefficients. __SO2+__CaO+__O2=__CaSO4 b) How many metric tons of calcium sulfate would be produced from each metric ton of SO2 that is trapped?arrow_forwardChlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g) How much MnO2(s) should be added to excess HCl(aq) to obtain 335 mL Cl2(g) at 25 °C and 1.00×102 kPa ? mass: ______g MnO2arrow_forwardNitric acid can be produced by the reaction of gaseous nitrogen dioxide with water. 3NO2(g)+H 2O(l)=2HNO3(l)+NO(g) If 829 L of NO2 gas react with water,what volume of NO gas will be produced ? Assume the gases are measured under the same conditions . Answer in units of Larrow_forward
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