Question
Predict the products in the below chemical reactions and write the chemical equation. Balance the equation and identify the type of chemical reaction.
a. An aqueous solution of Copper(2) Chloride reacts with zinc metal.
b. An aqueous solution of ammonium sulfate reacts with an aqueous solution of barium nitrate.
c. Butane(C4H10) undergoes combustion in the presence of oxygen gas.
a. An aqueous solution of Copper(2) Chloride reacts with zinc metal.
b. An aqueous solution of ammonium sulfate reacts with an aqueous solution of barium nitrate.
c. Butane(C4H10) undergoes combustion in the presence of oxygen gas.
Answers
GPT-4o mini
Let’s analyze each reaction, predict the products, write and balance the chemical equations, and identify the type of reaction.
### Reaction a: Copper(II) Chloride with Zinc
**Reactants**: Copper(II) Chloride (CuCl₂, aqueous) and Zinc (Zn, solid)
**Predicted Products**: Zinc Chloride (ZnCl₂, aqueous) and Copper (Cu, solid)
**Chemical Equation**:
\[ \text{CuCl}_2 (aq) + \text{Zn} (s) \rightarrow \text{ZnCl}_2 (aq) + \text{Cu} (s) \]
**Balanced Equation**:
\[ \text{CuCl}_2 (aq) + \text{Zn} (s) \rightarrow \text{ZnCl}_2 (aq) + \text{Cu} (s) \]
**Type of Reaction**: Single Displacement Reaction (or Single Replacement Reaction).
---
### Reaction b: Ammonium Sulfate with Barium Nitrate
**Reactants**: Ammonium Sulfate \((\text{(NH}_4)_2\text{SO}_4, aq)\) and Barium Nitrate \((\text{Ba(NO}_3)_2, aq)\)
**Predicted Products**: Barium Sulfate (BaSO₄, solid) and Ammonium Nitrate \((\text{NH}_4\text{NO}_3, aq)\)
**Chemical Equation**:
\[ \text{(NH}_4)_2\text{SO}_4 (aq) + \text{Ba(NO}_3)_2 (aq) \rightarrow \text{BaSO}_4 (s) + 2\text{NH}_4\text{NO}_3 (aq) \]
**Balanced Equation**:
\[ \text{(NH}_4)_2\text{SO}_4 (aq) + \text{Ba(NO}_3)_2 (aq) \rightarrow \text{BaSO}_4 (s) + 2\text{NH}_4\text{NO}_3 (aq) \]
**Type of Reaction**: Double Displacement Reaction (or Double Replacement Reaction).
---
### Reaction c: Combustion of Butane
**Reactants**: Butane \((\text{C}_4\text{H}_{10}, g)\) and Oxygen gas \((\text{O}_2, g)\)
**Predicted Products**: Carbon Dioxide \((\text{CO}_2, g)\) and Water \((\text{H}_2\text{O}, g)\)
**Unbalanced Chemical Equation**:
\[ \text{C}_4\text{H}_{10} (g) + \text{O}_2 (g) \rightarrow \text{CO}_2 (g) + \text{H}_2\text{O} (g) \]
**Balancing the Equation**:
1. C: 4 \(\text{C}_4\text{H}_{10}\) → 4 \(\text{CO}_2\)
2. H: 10 \(\text{C}_4\text{H}_{10}\) → 5 \(\text{H}_2\text{O}\) (10 hydrogens)
3. O: There are 4 × 2 = 8 from \(\text{CO}_2\) and 5 from \(\text{H}_2\text{O}\), so total = 13 oxygen atoms needed.
The balanced equation:
\[ \text{C}_4\text{H}_{10} (g) + \frac{13}{2} \text{O}_2 (g) \rightarrow 4 \text{CO}_2 (g) + 5 \text{H}_2\text{O} (g) \]
To eliminate the fraction, multiply through by 2:
\[ 2\text{C}_4\text{H}_{10} (g) + 13 \text{O}_2 (g) \rightarrow 8 \text{CO}_2 (g) + 10 \text{H}_2\text{O} (g) \]
**Type of Reaction**: Combustion Reaction.
---
In summary, we have:
1. Single displacement reaction for the Copper(II) Chloride and Zinc.
2. Double displacement reaction for the Ammonium Sulfate and Barium Nitrate.
3. Combustion reaction for Butane.
### Reaction a: Copper(II) Chloride with Zinc
**Reactants**: Copper(II) Chloride (CuCl₂, aqueous) and Zinc (Zn, solid)
**Predicted Products**: Zinc Chloride (ZnCl₂, aqueous) and Copper (Cu, solid)
**Chemical Equation**:
\[ \text{CuCl}_2 (aq) + \text{Zn} (s) \rightarrow \text{ZnCl}_2 (aq) + \text{Cu} (s) \]
**Balanced Equation**:
\[ \text{CuCl}_2 (aq) + \text{Zn} (s) \rightarrow \text{ZnCl}_2 (aq) + \text{Cu} (s) \]
**Type of Reaction**: Single Displacement Reaction (or Single Replacement Reaction).
---
### Reaction b: Ammonium Sulfate with Barium Nitrate
**Reactants**: Ammonium Sulfate \((\text{(NH}_4)_2\text{SO}_4, aq)\) and Barium Nitrate \((\text{Ba(NO}_3)_2, aq)\)
**Predicted Products**: Barium Sulfate (BaSO₄, solid) and Ammonium Nitrate \((\text{NH}_4\text{NO}_3, aq)\)
**Chemical Equation**:
\[ \text{(NH}_4)_2\text{SO}_4 (aq) + \text{Ba(NO}_3)_2 (aq) \rightarrow \text{BaSO}_4 (s) + 2\text{NH}_4\text{NO}_3 (aq) \]
**Balanced Equation**:
\[ \text{(NH}_4)_2\text{SO}_4 (aq) + \text{Ba(NO}_3)_2 (aq) \rightarrow \text{BaSO}_4 (s) + 2\text{NH}_4\text{NO}_3 (aq) \]
**Type of Reaction**: Double Displacement Reaction (or Double Replacement Reaction).
---
### Reaction c: Combustion of Butane
**Reactants**: Butane \((\text{C}_4\text{H}_{10}, g)\) and Oxygen gas \((\text{O}_2, g)\)
**Predicted Products**: Carbon Dioxide \((\text{CO}_2, g)\) and Water \((\text{H}_2\text{O}, g)\)
**Unbalanced Chemical Equation**:
\[ \text{C}_4\text{H}_{10} (g) + \text{O}_2 (g) \rightarrow \text{CO}_2 (g) + \text{H}_2\text{O} (g) \]
**Balancing the Equation**:
1. C: 4 \(\text{C}_4\text{H}_{10}\) → 4 \(\text{CO}_2\)
2. H: 10 \(\text{C}_4\text{H}_{10}\) → 5 \(\text{H}_2\text{O}\) (10 hydrogens)
3. O: There are 4 × 2 = 8 from \(\text{CO}_2\) and 5 from \(\text{H}_2\text{O}\), so total = 13 oxygen atoms needed.
The balanced equation:
\[ \text{C}_4\text{H}_{10} (g) + \frac{13}{2} \text{O}_2 (g) \rightarrow 4 \text{CO}_2 (g) + 5 \text{H}_2\text{O} (g) \]
To eliminate the fraction, multiply through by 2:
\[ 2\text{C}_4\text{H}_{10} (g) + 13 \text{O}_2 (g) \rightarrow 8 \text{CO}_2 (g) + 10 \text{H}_2\text{O} (g) \]
**Type of Reaction**: Combustion Reaction.
---
In summary, we have:
1. Single displacement reaction for the Copper(II) Chloride and Zinc.
2. Double displacement reaction for the Ammonium Sulfate and Barium Nitrate.
3. Combustion reaction for Butane.