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Balance the equation for the production of acetylene

Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro ISBN: 9780321809247 1

Solution for problem 96E Chapter 22

Chemistry: A Molecular Approach | 3rd Edition

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Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro

Chemistry: A Molecular Approach | 3rd Edition

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Problem 96E

Balance the equation for the production of acetylene (C2H2) from the reaction of calcium carbide with water. If the acetylene is burned to form water and carbon dioxide, how many kilojoules of energy are produced from the complete reaction of 18 g of calcium carbide?

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Solution:Step-1Here we will have to balance the chemical equation for the formation of acetylene from CaC (s) 2and H O2l), the reaction will beCaC (s) + H O (l) C H (g) + Ca (OH) (s) 2 2 2 2 2Now we have to balance the above equation.Here total number of H atoms in reactant is 2, where as in product it is 4. In order to balance thetotal number of H -atoms in both the sides , multiply 2 with H O .Hence the equati2 will beCaC (s) + 2H O (l) C H (g) + Ca (OH) (s) 2 2 2 2 2Step-2If the acetylene gas burned it will form H O and CO ,2he reaction i22C H (g) + 5O (g) 2H O (l) + 4CO (g) 2 2 2 2 2Now we calculate the heat of energy was produced from this reaction H = n H - n H reaction p products r reactants = [2 H H2O(l) 4 H CO(g) - [ 2H C2H2g) + 5H O2(g) = [(2 ×(-285))KJ/mol + 4(-393.5)KJ/mol] -[(2 ×(227.4))KJ/mol + 5(0)KJ/mol] = [-571 KJ/mol - 1574 KJ/mol] -[ 454.8 KJ/mol] = [-2145.6 KJ/mol]- [454.8 KJ/mol] = -2600.4 KJ/molThus enthalpy of reaction is -2600.4 KJ/mol.So we can say that 2600.4 KJ/mol energy was released per two of acetylene.In this reaction 64.10 g of CaC2 has burned to give 1 mole of acetyleneSo if 18.0 g of CaC2 will burned with air , the number of moles of C2H2 produced is= 1.0 mol of C H 2 2---------------------- ×18.0 g of CaC 264.10 g of CaC 2= 0.2808 mol of C H 2 2From 2 moles of acetylene 2600.4KJ of energy was released, hence the amount of energyreleased from 0.2808 mole of acetylene burn with air is,= 2600.4 KJ--------------- × 0.2808 mol of C H 2 22.0 mol of C H 2 2= 365.1 KJThus the amount of energy released from 18.0 g of CaC burned with air is 32.1 KJ.\n

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Chapter 22, Problem 96E is Solved
Step 3 of 3

Textbook: Chemistry: A Molecular Approach
Edition: 3
Author: Nivaldo J. Tro
ISBN: 9780321809247

The full step-by-step solution to problem: 96E from chapter: 22 was answered by , our top Chemistry solution expert on 02/22/17, 04:35PM. Chemistry: A Molecular Approach was written by and is associated to the ISBN: 9780321809247. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3. Since the solution to 96E from 22 chapter was answered, more than 389 students have viewed the full step-by-step answer. This full solution covers the following key subjects: acetylene, reaction, carbide, Calcium, Water. This expansive textbook survival guide covers 82 chapters, and 9454 solutions. The answer to “?Balance the equation for the production of acetylene (C2H2) from the reaction of calcium carbide with water. If the acetylene is burned to form water and carbon dioxide, how many kilojoules of energy are produced from the complete reaction of 18 g of calcium carbide?” is broken down into a number of easy to follow steps, and 45 words.

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