### Combustion Reaction of Hexane**Example Question:**(4.2, Similar to For Practice 4.2) Write a balanced equation for the combustion of hexane ($ \text{C}_6\text{H}_{14} $) in which it combines with gaseous oxygen to form gaseous carbon dioxide and gaseous water. The smallest possible set of whole-number coefficients has been used.**Question:**What is the coefficient of $ \text{C}_6\text{H}_{14} $ when the reaction is balanced?---**Answer Options:**- ○ 3- ○ 4- ○ 1- ○ 2### Detailed Explanation:The balanced chemical equation for the combustion of hexane ($ \text{C}_6\text{H}_{14} $) is as follows:\[ \text{2 C}_6\text{H}_{14} + 19 \text{O}_2 \rightarrow 12 \text{CO}_2 + 14 \text{H}_2\text{O} \]To balance the equation, we follow these steps:1. **Write the unbalanced equation:**\[ \text{C}_6\text{H}_{14} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \]2. **Balance the carbon atoms:** - There are 6 carbon atoms in $ \text{C}_6\text{H}_{14} $, so we need 6 CO₂ molecules on the products side:\[ \text{C}_6\text{H}_{14} + \text{O}_2 \rightarrow 6 \text{CO}_2 + \text{H}_2\text{O} \]3. **Balance the hydrogen atoms:** - There are 14 hydrogen atoms in $ \text{C}_6\text{H}_{14} $, so we need 7 $ \text{H}_2\text{O} $ molecules on the products side:\[ \text{C}_6\text{H}_{14} + \text{O}_2 \rightarrow 6 \text{CO}_2 + 7 \text{H}_2\text{O} \]4. **Balance the oxygen atoms:** -

Answered: Image /qna-images/answer/04903a8f-7d28-4657-8d2f-5bc670dadc74.jpg

(4.2, Similar to For Practice 4.2) Write balanced equation for the combustion of hexane (C6H14) in which it combines with gaseous oxygen to form gaseous carbon dioxide and gaseous water. The smallest possible set of whole-number coefficients has been used. What is the coefficient of C6H14 when the reaction is balanced? O 3 04 0 1 O 2

(4.2, Similar to For Practice 4.2) Write balanced equation for the combustion of hexane (C6H14) in which it combines with gaseous oxygen to form gaseous carbon dioxide and gaseous water. The smallest possible set of whole-number coefficients has been used. What is the coefficient of C6H14 when the reaction is balanced? O 3 04 0 1 O 2

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

Question 3 of 22 Write a balanced chemical equation based on the following description: butane gas and oxygen gas react to produce carbon dioxide gas and water vapor 2 C,H10(g) + 9 O2(g) → 8 CO(g) +10 H20(g) 3c 2- Reset > 1 4 7 8 (s) (1) (g) (aq) C W H. Ва Ox Са x H20 p for additional resources LO
Balance the following chemical equations: 1. The reaction between iron and oxygen in the air produces rust. Fe+0 Fe O 2. Car engine burns fuel. Combustion or burning takes place when methane combines with oxygen in the air to produce carbon dioxide and water vapor. +0. Aco+HO 16 Hyperacidity is observed when the stomach becomes too acidic. Antacids such as calcium hydroxide are used to neutralize the hydrochloric acid inside the stomach. 3. Ca(OH) + HCI CaCl +H.0
6. Consider the reaction: 4Al(s) + 3029) – > 2Al2O3(s) (a) If 9.00 moles of aluminum react with an excess of oxygen, how many moles of aluminum oxide are produced? (b) The production of 0.435 moles of aluminum oxide requires the reaction of moles of aluminum and (c) When 1.730 moles of aluminum reacts, moles of oxygen? moles of oxygen are consumed.
Consider the following unbalanced equation: NH3 + 02 ------> NO2 + H2O The combustion of 28.8 grams of ammonia consumes how many grams of oxygen. Select one: а. 108 b. 54.1 С. 28.8 O d. 94.9 e. 15.3
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Cryolite, Na, AIF,(s), an ore used in the production of aluminum, can be synthesized using aluminum oxide. Balance the equation for the synthesis of cryolite. equation: Al, 0, (s)+NAOH(1)+HF(g) Na, AIF, + H, O(g) If 12.9 kg of Al,0,(s), 56.4 kg of NaOH(1), and 56.4 kg of HF(g) react completely, how many kilograms of cryolite will be produced? mass of cryolite produced: kg Na, AlF, Which reactants will be in excess? NaOH Al, O3 HF What is the total mass of the excess reactants left over after the reaction is complete? total mass of excess reactants: kg Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Science Books
6.38 Use the balanced equation for the combustion of ethane to complete the table. Initially mixed How much reacts Composition of final mixture 2C₂H6(g) + 70₂(g) 10 20 molecules molecules HS 4CO₂(g) + 6H₂O(g) 0 O molecules molecules - (artis
15. Citric acid, C6H807 (aq), is often used as an additive to make candies "sour. a. Draw a flowchart that shows how to caloulate the molar mass of citric acid, b. Verify the steps in your flowchart by calculating the molar mass of citric acid.
Camels store the fat tristearin (C57H110O6) in their hump. As well as being a source of energy, the fat is a source of water, because of the following respiration reaction: 2 C57H110O6 (s) + 163 O2 (g) à 114 CO2 (g) + 110 H2O (l)What mass (g) of water can be made from 1.0 kg of fat?
5. 2Fe(OH);(s) + 3H,SO4(ag) → Fe2(SO4);(ag) + 6H;0(I) classify: If 2.4 g Fe(OH)3 and 3.3 g H2SO4 react and make 4.5 g Fe2(SO4)3, g H20 are made also. Find theoretical yield of Fe2(SO4)3 in a reaction of 24.1 mol Fe(OH)3 and 30.5 mol H2SO4 : The 24.1 mol Fe(OH)3 are enough to form mol Fe2(SO4)3. The 30.5 mol H,SO4 are enough to form mol Fe2(SO4)3. The limiting reagent in the mixture is The theoretical yield of Fe2(SO4)3 is moles If only 8.2 mol Fe2(SO4)3 Was isolated, the percent reaction yield is %
0 3.76 Consider the mixture of propane, C,Hg, and O2 shown below. (a) Write a balanced equation for the combustion reaction that Occurs between propane and oxygen. (b) Which reactant is the limiting reactant? (c) How many molecules of CO, H2O, C;Hs, and O, will be present if the reaction goes to completion?
Methane, CH4, burns in oxygen. What are the products of the reaction? Write the balanced equation for the reaction. What mass of O2, in grams, is required for complete combustion of 25.5 g of methane? What is the total mass of products expected from the combustion of 25.5 g of methane? 2.The metals industry was a major source of air pollution years ago. One common process involved “roasting” metal sulfides in the air: 2 PbS(s) + 3 O2(g) !’"#$%&⎯⎯) 2 PbO(s) + 2 SO2(g) If 2.50 mol of PbS is heated in air, what amount of O2 is required for complete reaction? What amounts of PbO and SO2 are expected? 3.Iron ore is converted to iron metal in a reaction with carbon. 2 Fe2O3(s) + 3 C(s) ’!"#$%&⎯⎯) 4 Fe(s) + 3 CO2(g) If 6.2 mol of Fe2O3(s) is used, what amount of C(s) is needed, and what amounts of Fe and CO2 are produced? 4.Sodium sulfide, Na2S, is used in the leather industry to remove hair from hides. The Na2S is made by the reaction Na2SO4(s) + 4 C(s)…
For the following reaction, 3.65 grams of hydrogen gas are mixed with excess nitrogen gas. The reaction yields 16.8 grams of ammonia. N2 (g) + 3H2 - 2NH3 (g) (1) What is the theoretical yield of ammonia?| grams (2) What is the percent yield for this reaction?