The Equation For The Reaction Is:$\[ Mg(s) + H_2O(g) \longrightarrow MgO(s) + H_2(g) \\](i) The Teacher Used 1.00 G Of Magnesium.Use The Equation To Calculate The Maximum Mass Of Magnesium Oxide Produced.Give Your Answer To Three Significant

Understanding the Chemical Equation

The given chemical equation is: ${ Mg(s) + H_2O(g) \longrightarrow MgO(s) + H_2(g) }$(i) This equation represents the reaction between magnesium (Mg) and water (H2O) to produce magnesium oxide (MgO) and hydrogen gas (H2). The equation is balanced, indicating that the number of atoms of each element is the same on both the reactant and product sides.

Calculating the Maximum Mass of Magnesium Oxide Produced

To calculate the maximum mass of magnesium oxide produced, we need to use the given information about the amount of magnesium used. The teacher used 1.00 g of magnesium. We can use the molar masses of magnesium and magnesium oxide to calculate the maximum mass of magnesium oxide produced.

Molar Masses of Magnesium and Magnesium Oxide

The molar mass of magnesium (Mg) is 24.31 g/mol, and the molar mass of magnesium oxide (MgO) is 40.30 g/mol.

Calculating the Number of Moles of Magnesium Used

We can calculate the number of moles of magnesium used by dividing the given mass of magnesium (1.00 g) by the molar mass of magnesium (24.31 g/mol).

${ \text{Number of moles of Mg} = \frac{\text{Mass of Mg}}{\text{Molar mass of Mg}} }$

${ \text{Number of moles of Mg} = \frac{1.00 \text{ g}}{24.31 \text{ g/mol}} }$

${ \text{Number of moles of Mg} = 0.0411 \text{ mol} }$

Calculating the Maximum Mass of Magnesium Oxide Produced

Since the equation is balanced, the number of moles of magnesium oxide produced is equal to the number of moles of magnesium used. We can calculate the maximum mass of magnesium oxide produced by multiplying the number of moles of magnesium oxide by the molar mass of magnesium oxide.

${ \text{Maximum mass of MgO} = \text{Number of moles of MgO} \times \text{Molar mass of MgO} }$

${ \text{Maximum mass of MgO} = 0.0411 \text{ mol} \times 40.30 \text{ g/mol} }$

${ \text{Maximum mass of MgO} = 1.66 \text{ g} }$

Conclusion

The maximum mass of magnesium oxide produced is 1.66 g. This calculation assumes that the reaction goes to completion and that all of the magnesium used is converted to magnesium oxide.

Limitations of the Calculation

This calculation has several limitations. First, it assumes that the reaction goes to completion, which is unlikely in a real-world scenario. Second, it assumes that all of the magnesium used is converted to magnesium oxide, which is also unlikely. Finally, it does not take into account any impurities or contaminants that may be present in the magnesium or water used.

Future Directions

Future research could focus on improving the accuracy of this calculation by taking into account the limitations mentioned above. This could involve using more advanced techniques, such as spectroscopy or chromatography, to analyze the products of the reaction. Additionally, researchers could investigate the effects of different conditions, such as temperature or pressure, on the reaction.

Applications of the Calculation

This calculation has several potential applications in fields such as chemistry, materials science, and engineering. For example, it could be used to design and optimize chemical reactors, or to predict the properties of materials produced through chemical reactions.

Conclusion

In conclusion, the maximum mass of magnesium oxide produced can be calculated using the given chemical equation and the molar masses of magnesium and magnesium oxide. This calculation has several limitations, but it provides a useful estimate of the maximum mass of magnesium oxide produced. Future research could focus on improving the accuracy of this calculation and exploring its potential applications in fields such as chemistry, materials science, and engineering.

Q: What is the chemical equation for the reaction between magnesium and water?

A: The chemical equation for the reaction between magnesium and water is: ${ Mg(s) + H_2O(g) \longrightarrow MgO(s) + H_2(g) }$(i)

Q: What is the molar mass of magnesium (Mg)?

A: The molar mass of magnesium (Mg) is 24.31 g/mol.

Q: What is the molar mass of magnesium oxide (MgO)?

A: The molar mass of magnesium oxide (MgO) is 40.30 g/mol.

Q: How can I calculate the number of moles of magnesium used?

A: To calculate the number of moles of magnesium used, you can divide the given mass of magnesium by the molar mass of magnesium. For example, if you have 1.00 g of magnesium, the number of moles of magnesium used would be: ${ \text{Number of moles of Mg} = \frac{\text{Mass of Mg}}{\text{Molar mass of Mg}} }$

${ \text{Number of moles of Mg} = \frac{1.00 \text{ g}}{24.31 \text{ g/mol}} }$

${ \text{Number of moles of Mg} = 0.0411 \text{ mol} }$

Q: How can I calculate the maximum mass of magnesium oxide produced?

A: To calculate the maximum mass of magnesium oxide produced, you can multiply the number of moles of magnesium oxide by the molar mass of magnesium oxide. For example, if you have 0.0411 mol of magnesium oxide, the maximum mass of magnesium oxide produced would be: ${ \text{Maximum mass of MgO} = \text{Number of moles of MgO} \times \text{Molar mass of MgO} }$

${ \text{Maximum mass of MgO} = 0.0411 \text{ mol} \times 40.30 \text{ g/mol} }$

${ \text{Maximum mass of MgO} = 1.66 \text{ g} }$

Q: What are some limitations of this calculation?

A: Some limitations of this calculation include the assumption that the reaction goes to completion, the assumption that all of the magnesium used is converted to magnesium oxide, and the lack of consideration for impurities or contaminants.

Q: What are some potential applications of this calculation?

A: Some potential applications of this calculation include designing and optimizing chemical reactors, predicting the properties of materials produced through chemical reactions, and understanding the behavior of chemical systems.

Q: Can I use this calculation to predict the properties of magnesium oxide?

A: Yes, you can use this calculation to predict the properties of magnesium oxide. By understanding the relationship between the number of moles of magnesium oxide and the molar mass of magnesium oxide, you can make predictions about the properties of magnesium oxide, such as its density, melting point, and boiling point.

Q: Can I use this calculation to design a chemical reactor?

A: Yes, you can use this calculation to design a chemical reactor. By understanding the relationship between the number of moles of magnesium oxide and the molar mass of magnesium oxide, you can design a reactor that is optimized for the production of magnesium oxide.

Q: What are some potential future directions for this research?

A: Some potential future directions for this research include improving the accuracy of this calculation by taking into account the limitations mentioned above, exploring the effects of different conditions, such as temperature or pressure, on the reaction, and investigating the behavior of chemical systems under different conditions.

Q: Can I use this calculation to understand the behavior of chemical systems?

A: Yes, you can use this calculation to understand the behavior of chemical systems. By understanding the relationship between the number of moles of magnesium oxide and the molar mass of magnesium oxide, you can gain insights into the behavior of chemical systems and make predictions about their behavior under different conditions.