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Chapter 6: Problem 25

Acetylene gas \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) is often used by plumbers, welders, and glass blowers because it burns in oxygen with an intensely hot flame. The products of the combustion of acetylene are carbon dioxide and water vapor. Write the unbalanced chemical equation for this process.

Short Answer

Expert verified
The unbalanced chemical equation for the combustion of acetylene gas (\(C_2H_2\)) in oxygen is: \(C_2H_2 + O_2 鈫� CO_2 + H_2O\)

Step by step solution

01

1. Identify the Reactants and Products

In the process of combustion, the reactants are acetylene gas (\(C_2H_2\)) and oxygen gas (O2). The products are carbon dioxide (CO2) and water vapor (H2O).
02

2. Write the Unbalanced Chemical Equation

To write the unbalanced chemical equation, we need to know the reactants and products we identified in the previous step. The chemical equation would look like this: \(C_2H_2 + O_2 鈫� CO_2 + H_2O\) Keep in mind that this equation is unbalanced, meaning that there are not the same number of each type of atom on both sides of the equation.

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Most popular questions from this chapter

The sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethyl alcohol (ethanol) and carbon dioxide gas. Balance the following equation for this reaction of sucrose.$$\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(a q)+\mathrm{CO}_{2}(g)$$

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