If a student burns 0.65 grams of methane (CH4) according to the equation below, what mass of carbon dioxide will be released? Round your answer to the nearest 0.01 and remember to include units and substance! CH4 + 2 O2 --> CO2 + 2 H2O
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
When a fuel such as methane burns in air to form carbon dioxide, water vapour and give heat energy, the reaction is called combustion reaction.
CH4 + 2 O2 --> CO2 + 2 H2O
Mole relation gives relationship between number of moles and molar mass of the compound. According to it, 1 mol of the compound is equivalent to it's molar mass in grams.
1 mol = molar mass in grams
Atomic masse of elements involved in the reaction are as follows:
Element atomic mass (g/mol)
C 12
H 1
O 16
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