hyrw 2o nsn hyapsn semSt.) Calcium oxide is sometimes very challenging to etare n theOumistry labrortory.This compound reacts with moisture in theair and is converted to calcium hydcokide. If a bottle ofcalcium oxide i8 left on the ehelf too long, it groduallyabsorbs moisture from the humidity in the laboratory.Eventually th bottle cracks and spills the colcium hydrokidethat hus been produced. WrHhe the unbalancaed chemical equaherfor this process.33.) The clement tin often occurs in nature as the oxide, Snb produce pure tin metal from this sort of tin oe, the oreGtmol rom theusually is heated with coal Carbon) This produies pure

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31.) Calcium oxide is sometimes very.challenging to etore in the hemistry labroctory.This compound rtacts with moisture in the air and is converted to calcium hydcokide. If a bottle ot calcium oxide is left on the shelf too long, t grodually absorbs moisture from the humidity i8 the laboratory. bventually th bottle cracks and spills the colciun hydrokide that hus bèen producod. WrAhe the unbalancad chemical equaher for this process. 33.) The elemnt tin often occurs in nature as He oxide, Sn0z. b produce pure tin metal from this sort of tin ore, the ore usually io heated with coal Carbon) This produces pure from the

31.) Calcium oxide is sometimes very.challenging to etore in the hemistry labroctory.This compound rtacts with moisture in the air and is converted to calcium hydcokide. If a bottle ot calcium oxide is left on the shelf too long, t grodually absorbs moisture from the humidity i8 the laboratory. bventually th bottle cracks and spills the colciun hydrokide that hus bèen producod. WrAhe the unbalancad chemical equaher for this process. 33.) The elemnt tin often occurs in nature as He oxide, Sn0z. b produce pure tin metal from this sort of tin ore, the ore usually io heated with coal Carbon) This produces pure from the

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter13: Gases

Section: Chapter Questions

Problem 136AP

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62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?
A 0.580 g sample of calsium(Ca) is allowed to burn in 2.530 g of oxygen gas(O2). The sole product is calsium oxide(CaO)oxide is produced?
Cinnabar, (or Cinnabarite) HgSHgS is the common ore of mercury. Because of its mercury content, cinnabar can be tpxoc to human beings; however, because of its red color, it has also been used since ancient times as a pigment. Alchemists produced elemental mercury by roasting cinnabar ore in air: HgS(s)+O2(g) → Hg(l) + SO2(g) The votality and toxicity of mercury make this a hazardous procedure, which likely shortened the life span of many alchemists. Given 100g of cinnabar, a. How much elemtal mercury can be produced from this reaction? b. How much oxygen is required to completely react with the given amount of cinnabar?
To obtain pure lead, lead (II) sulfide is burned in an atmosphere of pure oxygen. The products of thereaction are lead and sulfur trioxide (SO3). Write a balanced chemical equation for this process.
Limestone rocks are composed mainly of calcium carbonate (CaCO3) that reacts easily with an acid, releasing carbon dioxide gas.
The source of oxygen that drives the internal combustionengine in an automobile is air. Air is a mixture of gases, principallyN2(∼79%) and O2(∼20%). In the cylinder of an automobileengine, nitrogen can react with oxygen to producenitric oxide gas, NO. As NO is emitted from the tailpipe ofthe car, it can react with more oxygen to produce nitrogendioxide gas. (a) Write balanced chemical equations for bothreactions. (b) Both nitric oxide and nitrogen dioxide are pollutantsthat can lead to acid rain and global warming; collectively,they are called “NOx” gases. In 2009, the United Statesemitted an estimated 19 million tons of nitrogen dioxideinto the atmosphere. How many grams of nitrogen dioxide isthis? (c) The production of NOx gases is an unwanted side reactionof the main engine combustion process that turns octane,C8H18, into CO2 and water. If 85% of the oxygen in an engine isused to combust octane and the remainder used to produce nitrogendioxide, calculate how many grams of nitrogen…
Cocaine (C17H21O4N) is a natural substance found in the leaves of the coca plant, which has been used for centuries as a local anesthetic and stimulant. Illegal cocaine arrives in the USA either as a pure compound or as the hydrochloride salt (C17H21O4NHCl). At 25oC, the salt is very soluble in water (2.50 kg/L), but pure cocaine is much less so (1.70 g/L). What is the maximum amount of salt (in gram) that can dissolve in 50.0 mL of water? [1 mark.] When a 25 mL aqueous solution that contains 62.50 g of the salt is treated with NaOH, the salt is converted to pure cocaine. How much water (in liters) is needed additionally to dissolve the formed pure cocaine? Round your final answer off to two decimal points. C17H21O4NHCl(aq) + NaOH(aq) → C17H21O4N(aq) + H2O(l) + NaCl(aq)
Write the Qc for this Solid molybdenum(VI) oxide reacts with gaseous xenon difluoride to form liquid molybdenum(VI) fluoride, xenon gas, and oxygen gas.
Although we tend to make less use of mercury these days because of the environmental problems created by its improper disposal, mercury is still an important metal because of its unusual property of existing as a liquid at room temperature. One process by which mercury is produced industrially is through the heating of its common ore cinnabar (mercuric sulfide, HgS) with lime (calcium oxide, CaO). 4 HgS(s) + 4 CaO(s) → 4 Hg(l) + 3 CaS(s) + CaSO4(s) What mass of mercury would be produced by complete reaction of 10.7 kg of HgS? kg
Magnesium nitrate and barium nitrate decompose similarly on heating and the reaction can be represented as follow: M(NO3)2 (s) --› MO (s) + 2NO2 (g) + ½O2 (g), where M = Mg or Ba (a) When Group 1 nitrates (with the exception of lithium nitrate) are strongly heated, the corresponding nitrite was formed along with a colorless gas which relights a glowing splint. (i) Write a balanced equation for the thermal decomposition of potassium nitrate. (ii) Unlike other Group 1 nitrates, lithium nitrate decomposes on heating in the same way as Group 2 nitrates. Suggest a reason for the difference in behaviour, and give an equation for its decomposition. (b) Zinc carbonate and magnesium carbonate decompose when heated to give similar products. (i) Suggest an equation for the thermal decomposition of magnesium carbonate. (ii) The radius of Zn2+ cation is 0.074 nm. Use the Data Booklet to deduce whether zinc carbonate will decompose at a higher or lower temperature than magnesium carbonate. Explain…