4S + 30, + 2H,0 2H,SO, Sulfuric acid is a very important chemical and an indicator of a nation's industrial strength. World production in 2004 was about 180 million tons. Most of this amount (~60%) is consumed for fertilizers, particularly superphosphates, ammonium phosphate (NH,),PO, and ammonium sulfates (NH,),SO,. Sulfuric acid is needed to dissolve insoluble phosphate ores. If you start with 15.0g of sulfur and 20.0g of O,, How much sulfuric acid (H,SO) can you theoretically produce? very

4S + 30, + 2H,0 2H,SO, Sulfuric acid is a very important chemical and an indicator of a nation's industrial strength. World production in 2004 was about 180 million tons. Most of this amount (~60%) is consumed for fertilizers, particularly superphosphates, ammonium phosphate (NH,),PO, and ammonium sulfates (NH,),SO,. Sulfuric acid is needed to dissolve insoluble phosphate ores. If you start with 15.0g of sulfur and 20.0g of O,, How much sulfuric acid (H,SO) can you theoretically produce? very

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter1: Introduction To Chemistry

Section: Chapter Questions

Problem 1.6PAE: Use the web to determine the differences in the amounts of aluminum recycled in states where there...

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The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
Use the web to determine the differences in the amounts of aluminum recycled in states where there are deposits on aluminum cans versus states where recycling is voluntary. What is the most reliable way to estimate this value? mat uncertainty is there in the estimate?
The burning of iron pyrites (FeS.) in air may be expressed by the following reaction: Fes2 + 02 -> Fe203 + SO2 а. What mass of iron pyrite must be burned in air to produce 400.0g of ferric oxide? (8) b. What mass of oxygen will be consumed? ( C. How many molecules of sulfur dioxide will be produced ?
(2) 8. Write the balanced equation for the neutralization reaction between HI and Ba(OH)2 in aqueous solution. Include phases (physical states) in your equation. Use the arrow, not "=".
3) %23 Combustion of hydrocarbons such as undecane (C,,H) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap II 11 the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid undecane into gaseous carbon dioxide and gaseous water. olo x10 Ar 2. Suppose 0.490 kg of undecane are burned in air at a pressure of exactly 1 atmn and a temperature of 10.0 °C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits. Explanation Check O 2019 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy 11:16 PM 99+ 12/3/2019 O Type here to search hp Ba end ins prt sc home f10 f12 delete f8 f5 f6 esc num & %24 backspace lock 8 3
Urea (CH,N,0) is a common fertilizer that is synthesized by the reaction of ammonia (NH3) with carbon dioxide: 2 NH3(aq) + CO2(ag)– CH,N;O(ag) + H,0(1) In an industrial synthesis of urea, a chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.
The active ingredient in baking soda is sodium bicarbonate (NaHCO3). The active ingredient in vinegar is acetic acid (CH3CO2H). When mixed, they react as follows. This is balanced as written: NaHCO3(5) + CH3CO2H(aq) NaCH3CO2(aq) CO2(g) + H2O) + --> One of the products is gas; it is carbon dioxide (CO2). Based on this reaction, for every ONE molecule of sodium bicarbonate (NaHCO3) that reacts, how many molecules of GAS will form?
The reaction between potassium chlorate and red phosphorus takes place when you strike a match on a matchbox. If you were to react 52.9 g of potassium chlorate (KCIO,) with excess red phosphorus, what mass of tetraphosphorus decaoxide (P,O10) would be produced? KC1O:(5) + P4(s) - P,O0(5) + KCI(s) (unbalanced)
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N2(9)+3 H,(9)→2NH;(g) In the second step, ammonia and oxygen react to form nitric acid and water: NH3(9)+2O,(9)→HNO,(9)+H,O(9) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced.
1. A common way to produce oxygen in the laboratory is through the decomposition of potassium chlorate. (a) Balance the reaction and include states. KCIO, ( ) > O2() +KCI ( ) (b) How many grams of potassium chlorate (molar mass = 122.5492) must react to produce 425.00 mg of KCI (molar mass 74.5510).
The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina (Al,0,) and water: 2Al(OH), (s) Al,0; (s) + 3 H,0 (g) - In the second step, alumina (Al,0,) and carbon react to form aluminum and carbon dioxide: 2Al,0; (s) + 3C(s) → 4Al(s) + 3 CO, (g) Suppose the yield of the first step is 82.% and the yield of the second step is 69.%. Calculate the mass of aluminum hydroxide required to make 10.0 kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. x10
The 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 O-0 decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 58.0 mL of dioxygen gas are produced by this reaction, at a temperature of 60.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Round your answer to 3 significant digits.

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