(a) Methane, CH 4 , burns in the presence of oxygen to form water vapor and carb

Question

(a) Methane, CH4, burns in the presence of oxygen to form water vapor and carbon dioxide. Write a balanced chemical equation for this combustion reaction. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.)

(b) Specify the number and types of bonds broken for each molecule of methane burned.

Each molecule of CH4 has  carbon-hydrogen single bond(s). Each molecule of O2 has  oxygen-oxygen double bond(s). For each molecule of methane burned,  carbon-hydrogen single bond(s) are broken. Also, because  molecule(s) of oxygen are utilized in the balanced equation,  oxygen-oxygen double bond(s) are broken.

(c) If 50.0 kJ of energy is released for each gram of methane burned, how many kJ of energy will be released when 3.9 kg of the fuel undergoes combustion?
kJ

Explanation / Answer

a) CH4 +2 O2 (g) -----------> CO2 (g) + 2 H2O (g)

b)For each molecule of methane burned, 4 carbon-hydrogen single bond(s) are broken.

Since, 2 oxygen are utilized in the balanced equation, 2 oxygen-oxygen double bond(s) are broken.

c) 50 KJ / 1 g

So, 3.9 kg ------------> 3900 * 50

= 195000 Kj

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