Gaseous dichlorine monoxide decomposes readily to chlorine and oxygen gases.
(a) Which scene best depicts the product mixture after the decomposition?
(b) Write the balanced equation for the decomposition.
(c) If each oxygen atom represents 0.050 mol, how many molecules of dichlorine monoxide were present before the decomposition?
The Correct Answer and Explanation is :
It seems I am unable to access the image you provided due to restrictions. However, I can still help you with the questions based on the chemical reaction and the decomposition of dichlorine monoxide (Cl2O).
(a) Product Mixture After Decomposition
When dichlorine monoxide (Cl2O) decomposes, it breaks down into chlorine gas (Cl2) and oxygen gas (O2). The product mixture would consist of chlorine gas and oxygen gas. Since both chlorine and oxygen are diatomic molecules (Cl2 and O2), we would observe two distinct gases in the mixture.
- Chlorine gas (Cl2) is yellow-green in color and oxygen gas (O2) is colorless.
- Depending on the temperature and pressure, you might see the chlorine gas as a greenish-yellow vapor and oxygen gas as a colorless gas.
(b) Balanced Equation for the Decomposition
The decomposition of dichlorine monoxide can be represented by the following balanced chemical equation:
[ \text{Cl}_2\text{O} \rightarrow \text{Cl}_2 + \frac{1}{2} \text{O}_2 ]
This shows that one mole of dichlorine monoxide (Cl2O) decomposes into one mole of chlorine gas (Cl2) and half a mole of oxygen gas (O2).
(c) Molecule Calculation Before Decomposition
If each oxygen atom represents 0.050 moles, we can calculate how many molecules of dichlorine monoxide (Cl2O) were present before the decomposition. Here’s how:
- From the balanced equation, we know that for every mole of Cl2O, half a mole of O2 is produced.
- The number of oxygen atoms in the product will be the same as the number of oxygen atoms in the dichlorine monoxide before decomposition, since every Cl2O molecule contributes one oxygen atom.
Given that 0.050 mol of oxygen atoms (O) corresponds to 0.050 mol of O2 molecules (since each O2 molecule contains 2 oxygen atoms), the amount of Cl2O molecules present before the decomposition can be calculated as follows:
- For each O2 molecule produced, one Cl2O molecule decomposes. So, the amount of Cl2O molecules is the same as the amount of O2 molecules produced.
- Therefore, there were 0.050 moles of Cl2O molecules before the reaction.
Now, to find the number of molecules:
- The number of molecules in 1 mole is Avogadro’s number: (6.022 \times 10^{23}) molecules per mole.
- So, the number of molecules of Cl2O before the decomposition is:
[
0.050 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol} = 3.011 \times 10^{22} \, \text{molecules of Cl2O}
]
Thus, there were approximately (3.011 \times 10^{22}) molecules of dichlorine monoxide (Cl2O) before the decomposition.