2. Pure iron reacts with sulfuric acid, H2SO4(9), to form a solutíon of iron sulfate, Fe2(SOs, in water and gaseous hydrogen gas. 3. During photosynthesis in plants, carbon dioxide and water are converted into glucose, CSH1206, and oxygen gas, O,. 4. Acid rain, a solution of sulfurous acid, H.PO(ag), forms when sulfur dioxie Messanger reacts with water. Adrian Cenc

2. Pure iron reacts with sulfuric acid, H2SO4(9), to form a solutíon of iron sulfate, Fe2(SOs, in water and gaseous hydrogen gas. 3. During photosynthesis in plants, carbon dioxide and water are converted into glucose, CSH1206, and oxygen gas, O,. 4. Acid rain, a solution of sulfurous acid, H.PO(ag), forms when sulfur dioxie Messanger reacts with water. Adrian Cenc

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.57PAE

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4.3 Explain the difference between complete and incomplete combustion.
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Please find the CO2 amount and show the calculation: Air composition (apprx) = 80% N2 and 20% O2 (mol basis only)Average molecular weight of Air = (0.8 x 28 + 0.2 x 32) = 29 g/mol (apprx) Math Sample:2kg pure charcoal (12C) is to be burnt completely with air. Find the air, CO2 andN2 amount in kg’s.Solution:C + O2 = CO2 (you must use a balanced equation)Therefore from the mole ratio of the reaction we write,C : O2 : CO2 = 1:1:1and from air composition we gotO2 : N2 : Air = 1:4:5 Given, 2 kg C = 2000 g/ (12 g/mol) = 166.67 mole CTherefore, similar mole of O2 required. So equivalent Air supposed to be 5times than the mole amount of O2 and released N2 will be 4 times than therequired O2. Therefore, Air amount = 5 x 166.67 moles= 833.34 moles= (833.33x29/1000) kg= 24.17 kg air Similarly N2 released amount will be = (166.67 x 4 x 28/1000) kg = 18.67 kgFind CO2 amount by yourself! (Isn’t it 7.34 kg?)
The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO3s + O2g + 2MnO2s -> 2CO2g In the second step, manganese(IV) oxide and aluminum react to form manganese and aluminum oxidide: 3MnO2s + 4Als + 3Mns -> 2Al2O3s Suppose the yield of the first step is 74.% and the yield of the second step is 96.% . Calculate the mass of manganese(II) carbonate required to make 8.0kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
Give the product of the given reactants, balance the equation, and identify the type of chemical reaction involved in the chemical process. KNO3+ H2O----> ____________
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.5 Balance the reaction: ___ C6H14 (l) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (g) Then give the coefficient of oxygen gas.
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