Aluminum reacts with hydrochloric acid according to the following equation: 2Al(s) + 6HCI(aq) → 2AIC13(aq) + 3H2(g) 1. If a sample of 27.0 g of aluminum metal is added to 333 mL of 3.0 M hydrochloric acid, the volume of hydrogen gas pro- duced at standard temperature and pressure is (A) 2.80 L. (B) 5.60 L. (C) 11.2 L. (D) 22.4 L.
Aluminum reacts with hydrochloric acid according to the following equation: 2Al(s) + 6HCI(aq) → 2AIC13(aq) + 3H2(g) 1. If a sample of 27.0 g of aluminum metal is added to 333 mL of 3.0 M hydrochloric acid, the volume of hydrogen gas pro- duced at standard temperature and pressure is (A) 2.80 L. (B) 5.60 L. (C) 11.2 L. (D) 22.4 L.
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Chapter1: Chemical Foundations
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Number 1. I get 33 liters. No idea what I did wrong as I calculate one mole of aluminum present one mole of hydrochloric acid present giving me 1.5 miles of hydrogen plug that in to
pv= nrt. With p= 1atm. T = 273.
![**Title: Chemical Reaction Calculations**
**Introduction**
This document outlines the process involved in calculating the volume of gases produced in a chemical reaction using stoichiometry concepts.
**Reaction Equation**
The primary chemical reaction discussed is:
1A + 6Cl₂ → 2AlCl₃ + 3Cl₂
The coefficients indicate the moles of each substance involved in the reaction.
**Calculations**
1. **Moles Calculation**
- The molar mass of aluminium (Al) is given as 27g/mol.
- An example setup: 1 mole of Al reacts with 6 moles of Cl₂.
2. **Volume Calculation**
- Moles of product gases are calculated using the equation for stoichiometry.
- The volume (V) of gas is derived from the moles using the ideal gas law principles.
\[
V = (1.5) \times (0.08206) \times (273)
\]
- The result of this calculation is approximately 33 liters.
**Conclusion**
The document demonstrates a step-by-step example of calculating the volume of gases produced from a chemical reaction based on initial moles and conditions. Such exercises are essential for understanding chemical stoichiometry and gas laws in educational settings.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10afd7d2-537b-4ce7-8158-a5546637b29c%2Fcb4234ba-335a-49cb-9f92-0e48341ec00e%2F01ty626.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Chemical Reaction Calculations**
**Introduction**
This document outlines the process involved in calculating the volume of gases produced in a chemical reaction using stoichiometry concepts.
**Reaction Equation**
The primary chemical reaction discussed is:
1A + 6Cl₂ → 2AlCl₃ + 3Cl₂
The coefficients indicate the moles of each substance involved in the reaction.
**Calculations**
1. **Moles Calculation**
- The molar mass of aluminium (Al) is given as 27g/mol.
- An example setup: 1 mole of Al reacts with 6 moles of Cl₂.
2. **Volume Calculation**
- Moles of product gases are calculated using the equation for stoichiometry.
- The volume (V) of gas is derived from the moles using the ideal gas law principles.
\[
V = (1.5) \times (0.08206) \times (273)
\]
- The result of this calculation is approximately 33 liters.
**Conclusion**
The document demonstrates a step-by-step example of calculating the volume of gases produced from a chemical reaction based on initial moles and conditions. Such exercises are essential for understanding chemical stoichiometry and gas laws in educational settings.
![**AP Multiple-Choice Review Questions**
Use the following information to answer questions 1 and 2.
Aluminum reacts with hydrochloric acid according to the following equation:
\[ 2\text{Al}(\text{s}) + 6\text{HCl}(\text{aq}) \rightarrow 2\text{AlCl}_3(\text{aq}) + 3\text{H}_2(\text{g}) \]
1. **If a sample of 27.0 g of aluminum metal is added to 333 mL of 3.0 M hydrochloric acid, the volume of hydrogen gas produced at standard temperature and pressure is:**
- (A) 2.80 L
- (B) 5.60 L
- (C) 11.2 L
- (D) 22.4 L
2. **What is the approximate density of the hydrogen gas produced at STP?**
- (A) 0.1 g/L
- (B) 0.2 g/L
- (C) 0.3 g/L
- (D) 0.4 g/L](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10afd7d2-537b-4ce7-8158-a5546637b29c%2Fcb4234ba-335a-49cb-9f92-0e48341ec00e%2Fh929vv.jpeg&w=3840&q=75)
Transcribed Image Text:**AP Multiple-Choice Review Questions**
Use the following information to answer questions 1 and 2.
Aluminum reacts with hydrochloric acid according to the following equation:
\[ 2\text{Al}(\text{s}) + 6\text{HCl}(\text{aq}) \rightarrow 2\text{AlCl}_3(\text{aq}) + 3\text{H}_2(\text{g}) \]
1. **If a sample of 27.0 g of aluminum metal is added to 333 mL of 3.0 M hydrochloric acid, the volume of hydrogen gas produced at standard temperature and pressure is:**
- (A) 2.80 L
- (B) 5.60 L
- (C) 11.2 L
- (D) 22.4 L
2. **What is the approximate density of the hydrogen gas produced at STP?**
- (A) 0.1 g/L
- (B) 0.2 g/L
- (C) 0.3 g/L
- (D) 0.4 g/L
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