Disilane gas undergoes combustion to form solid silicon dioxide and water
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2Si2H6+7O2= 4SiO2+6H2O is the balanced equation for the above question.
The balanced chemical equation for the combustion of disilane (Si2H6) to form solid silicon dioxide (SiO2) and water (H2O) is as follows:
2 Si2H6 + 7 O2 → 2 SiO2 + 6 H2O
In this equation, disilane reacts with oxygen gas to produce silicon dioxide and water vapor as the products. The coefficients in front of each compound indicate the stoichiometric ratio of reactants and products. According to the equation, for every 2 molecules of disilane, 7 molecules of oxygen are required to produce 2 molecules of silicon dioxide and 6 molecules of water.
To understand this combustion reaction, we can start by looking at the chemical formula of disilane gas, which is Si2H6.
The balanced equation for the combustion of disilane gas can be written as follows:
Si2H6 + 3 O2 → SiO2 + 3 H2O
Let's break down the reaction step by step:
1. Disilane gas (Si2H6) reacts with oxygen gas (O2) from the air.
2. The carbon-silicon bonds in disilane gas are broken, and the carbon atoms combine with oxygen, forming silicon dioxide (SiO2).
3. The hydrogen atoms in disilane gas combine with oxygen to form water (H2O).
4. The reaction is balanced by ensuring that the number of atoms of each element is the same on both sides of the equation.
- On the left side, there are 2 silicon atoms, 6 hydrogen atoms, and 6 oxygen atoms.
- On the right side, there are 2 silicon atoms, 6 hydrogen atoms, and 6 oxygen atoms, which confirms that the reaction is balanced.
Overall, the combustion of disilane gas produces solid silicon dioxide (SiO2) and water (H2O).