Lithium and chlorine react according to the balanced chemical equation shown below. If the reaction is performed at STP, how many liters of chlorine are required to completely react with 12.3 grams of lithium ? 2 Li(s) + Cl₂(g)→ 2 LiCl(s)

To solve this problem, we need to determine how many liters of chlorine gas (\( \text{Cl}_2 \)) are required to completely react with 12.3 grams of lithium (\( \text{Li} \)) according to the balanced chemical equation:

\[
2 \text{Li(s)} + \text{Cl}_2(g) \rightarrow 2 \text{LiCl(s)}
\]

### Step 1: Calculate the moles of lithium
The molar mass of lithium (\( \text{Li} \)) is approximately 6.94 g/mol. We can use this to convert the given mass of lithium into moles.

\[
\text{moles of Li} = \frac{12.3 \text{ g}}{6.94 \text{ g/mol}} = 1.772 \text{ mol Li}
\]

### Step 2: Use the molar ratio
From the balanced equation, we know that 2 moles of lithium react with 1 mole of chlorine gas (\( \text{Cl}_2 \)). Therefore, the moles of chlorine gas required are:

\[
\text{moles of Cl}_2 = \frac{1.772 \text{ mol Li}}{2} = 0.886 \text{ mol Cl}_2
\]

### Step 3: Calculate the volume of chlorine gas at STP
At Standard Temperature and Pressure (STP), 1 mole of any ideal gas occupies 22.4 liters. Therefore, the volume of chlorine gas required is:

\[
\text{Volume of Cl}_2 = 0.886 \text{ mol} \times 22.4 \text{ L/mol} = 19.86 \text{ L}
\]

### Final Answer:
19.86 liters of chlorine gas are required to completely react with 12.3 grams of lithium at STP.

---

Would you like more details or have any questions on the process? Here are five follow-up questions to expand the topic:

1. What is the significance of STP conditions in gas law calculations?
2. How would the volume of chlorine gas change if the temperature were higher than STP?
3. What is the importance of balancing chemical equations in stoichiometry?
4. How would you approach this problem if you were given the volume of chlorine gas and asked to find the mass of lithium required?
5. How can you use the ideal gas law to calculate gas volumes at conditions other than STP?

**Tip:** Always check that the chemical equation is balanced before performing stoichiometry calculations.

Lithium and chlorine react according to the balanced chemical equation shown below. If the reaction is performed at STP, how many liters of chlorine are required to completely react with 12.3 grams of lithium? 2 Li(s) + Cl₂(g) → 2 LiCl(s)

Learn how to calculate the volume of chlorine gas needed to react with 12.3 grams of lithium using stoichiometry and gas laws. This step-by-step guide covers mole conversions, molar ratios, and ideal gas law principles. Suitable for students in Grades 10-12.

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