Consider the decomposition reaction of KCIO3 and answer the following questions: a. Write the balanced chemical equation of the decomposition reaction of KCIO3. B.Compute for the molar mass of KClO3 and KCl. C. What mass of KCIO3 will produce 48.0 g of oxygen gas, O2, if the decomposition of KCIO3 is complete? D. What mass of KCl is theoretically with 48.0 g of oxygen gas?
The Correct Answer and Explanation is :
A. Balanced Chemical Equation for the Decomposition of Potassium Chlorate (KClO₃):
The decomposition of potassium chlorate (KClO₃) produces potassium chloride (KCl) and oxygen gas (O₂). The balanced chemical equation is:
[ 2 \, \text{KClO}_3 \, (s) \rightarrow 2 \, \text{KCl} \, (s) + 3 \, \text{O}_2 \, (g) ]
B. Molar Mass of KClO₃ and KCl:
To compute the molar masses of KClO₃ and KCl, we’ll sum up the atomic masses of each element in the compounds.
- Molar Mass of KClO₃:
- Potassium (K): 39.1 g/mol
- Chlorine (Cl): 35.5 g/mol
- Oxygen (O): 16.0 g/mol × 3 = 48.0 g/mol [ \text{Molar Mass of KClO}_3 = 39.1 + 35.5 + 48.0 = 122.6 \, \text{g/mol} ]
- Molar Mass of KCl:
- Potassium (K): 39.1 g/mol
- Chlorine (Cl): 35.5 g/mol [ \text{Molar Mass of KCl} = 39.1 + 35.5 = 74.6 \, \text{g/mol} ]
C. Mass of KClO₃ to Produce 48.0 g of O₂:
We are given that 48.0 g of oxygen gas is produced. We can use stoichiometry to find the mass of KClO₃ required to produce this amount of oxygen.
- First, calculate the moles of O₂ produced:
[ \text{Moles of O}_2 = \frac{48.0 \, \text{g}}{32.0 \, \text{g/mol}} = 1.5 \, \text{mol} ] - From the balanced equation, 2 moles of KClO₃ produce 3 moles of O₂. So, the moles of KClO₃ needed to produce 1.5 moles of O₂ is:
[ \frac{2 \, \text{mol KClO}_3}{3 \, \text{mol O}_2} \times 1.5 \, \text{mol O}_2 = 1.0 \, \text{mol KClO}_3 ] - Now, calculate the mass of KClO₃ required:
[ \text{Mass of KClO}_3 = 1.0 \, \text{mol} \times 122.6 \, \text{g/mol} = 122.6 \, \text{g} ]
D. Mass of KCl Theoretically Produced:
From the balanced equation, for every 2 moles of KClO₃ decomposed, 2 moles of KCl are produced. Since we calculated that 1.0 mole of KClO₃ is required to produce 1.5 moles of O₂, it will also produce 1.0 mole of KCl.
Thus, the mass of KCl produced is:
[ \text{Mass of KCl} = 1.0 \, \text{mol} \times 74.6 \, \text{g/mol} = 74.6 \, \text{g} ]
Explanation:
In the decomposition of KClO₃, the reaction produces potassium chloride (KCl) and oxygen gas (O₂). The stoichiometric relationship between the reactants and products allows us to calculate the masses involved in the reaction. By using the molar masses of KClO₃ and O₂, and the balanced equation, we can find how much KClO₃ is required to produce a specific amount of oxygen and how much KCl will theoretically be produced.
Let me generate an image of the balanced equation for you.
Here is a visual representation of the balanced chemical equation for the decomposition of potassium chlorate (KClO₃). Let me know if you’d like any further explanation or have more questions!
