Chemistry: An Introduction to General, Organic, and Biological Chemistry (12th Edition)

Published by Prentice Hall
ISBN 10: 0321908449
ISBN 13: 978-0-32190-844-5

Chapter 7 - Section 7.8 - Energy in Chemical Reactions - Challenge Questions - Page 251: 7.109a

Answer

The balanced equation for that combustion is: $2 C_2H_2(g) + 5O_2(g) -^{\Delta}-\gt 4CO_2(g) +2 H_2O(g) + 2600 kJ$

Work Step by Step

1. In a combustion reaction, a carbon-containing compound reacts with oxygen gas ($O_2$) to produce carbon dioxide ($CO_2$), water $(H_2O)$ and energy in the form of heat. Write the equation for the combustion of $C_2H_2$. $C_2H_2(g) + O_2(g) -^{\Delta}-\gt CO_2(g) + H_2O(g) + 1300 kJ$ 2. Balance the equation a. Balance the number of carbon atoms, by putting a "2" in the front of $CO_2$: $C_2H_2(g) + O_2(g) -^{\Delta}-\gt 2CO_2(g) + H_2O(g) + 1300 kJ$ b. The number of hydrogen atoms is already balanced. c. Balance the number of oxygen atoms by putting a "$\frac{5}{2}$" in the front of $O_2(g)$ $C_2H_2(g) + \frac{5}{2}O_2(g) -^{\Delta}-\gt 2CO_2(g) + H_2O(g) + 1300 kJ$ 3. In order to remove the fraction, we have to multiply all the coefficients and the heat by 2. $2 C_2H_2(g) + 2 * \frac{5}{2}O_2(g) -^{\Delta}-\gt 2*2CO_2(g) +2 H_2O(g) + 2 * 1300 kJ$ $2 C_2H_2(g) + 5O_2(g) -^{\Delta}-\gt4CO_2(g) +2 H_2O(g) + 2600 kJ$
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