The complete combustion of acetic acid, HC2H3O2(l) to form H2O(l) and CO2(g) at a constant pressure releases 871.7kJ of heat per mole of HC2H3O2.
a) Write a balanced thermochemical equation for this reaction.
The answer is HC2H3O2(l) + O2(g)—->2 H2O(l) + 2 CO2 Change (^) H = -871.7kJ
b) My question is, if I only know the first part (the question), how do I determine that this combustion reaction is going to form a gas? I do not understand how to look at the elements and determine that if they are combined, a gas will form? What is the equation to find the kJ? Solution Preview
The question itself already tells you everything. Please see below for a detailed working of the solution.
comubstion of HC2H3O2 (l): it means HC2H3O2 (l) reacts with oxygen O2(gas)
it mentions it forms …
This solution helps find the balanced thermochemical equation for the combustion of acetic acid and helps find the heat from the reaction. Step by step calculations are given, along with explanations for each step.
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