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How Many Moles of Lithium Metal React to Yield 5.00 Mol of Hydrogen Gas?
Introduction:
Chemical reactions involve the transformation of reactants into products. In this article, we will explore the stoichiometry behind the reaction between lithium metal and the production of hydrogen gas. Specifically, we will determine the number of moles of lithium metal needed to yield 5.00 mol of hydrogen gas.
Stoichiometry of the Reaction:
The balanced chemical equation for the reaction between lithium metal and hydrogen gas is as follows:
2Li + H2 -> 2LiH
This equation tells us that two moles of lithium react with one mole of hydrogen gas to produce two moles of lithium hydride. From this equation, we can determine the stoichiometric ratio between lithium and hydrogen.
To find the number of moles of lithium metal needed to produce 5.00 mol of hydrogen gas, we can use the stoichiometric ratio from the balanced equation. Since the ratio is 2:1 for lithium to hydrogen, we can set up the following proportion:
2 mol Li / 1 mol H2 = x mol Li / 5.00 mol H2
Cross-multiplying and solving for x, we get:
x = (2 mol Li / 1 mol H2) * 5.00 mol H2
x = 10.00 mol Li
Therefore, 10.00 moles of lithium metal are required to yield 5.00 mol of hydrogen gas.
FAQs:
Q: Can I use any other units instead of moles?
A: Moles are the most commonly used unit for stoichiometry calculations because they provide a consistent and uniform measure of the amount of substance. However, if you have the mass of lithium metal instead of moles, you can convert it to moles using the molar mass of lithium before performing the stoichiometric calculation.
Q: How do I calculate the molar mass of lithium?
A: The molar mass of an element is the mass of one mole of that element. For lithium, the atomic mass is approximately 6.94 g/mol. Therefore, the molar mass of lithium is 6.94 g/mol.
Q: What if the balanced equation is different?
A: The stoichiometry of a reaction depends on the balanced chemical equation. If the equation is different, the stoichiometric ratio between lithium and hydrogen may change. In that case, you would need to use the new stoichiometric ratio in the calculation.
Q: Are there any other factors that may affect the reaction?
A: Stoichiometry assumes that the reaction occurs under ideal conditions and that all reactants are consumed completely. However, in real-world scenarios, there may be factors such as impurities, temperature, and pressure that could affect the reaction. It is important to consider these factors when performing actual experiments.
Conclusion:
The stoichiometry of a chemical reaction helps us determine the relationship between reactants and products. In the case of the reaction between lithium metal and hydrogen gas, we found that 10.00 moles of lithium metal are required to yield 5.00 mol of hydrogen gas. Understanding stoichiometry allows chemists to predict the amounts of reactants needed or products formed, providing a crucial basis for experimental design and analysis.
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