16. If the equation is correctly balanced, what are the coefficients? $$ \begin{array}{ll} ext { A. } 2: 3 ; 2: 5 & ext { C. } 1 ; 5 ; 3 ; 4 \ ext { B. } 2 ; 5 ; 1: 4 & ext { D. } 3 ; 5 ; 4 ; 10\end{array} $$ 17. If 50.0 g of $$ \mathrm{C}_{3} \mathrm{H}_{8} $$ is allowed to react with 200 g of $$ \mathrm{O}_{2} $$, which is the limiting reagent? (2points) $$ \begin{array}{ll} ext { A. } \mathrm{C}_{3} \mathrm{H}_{8} & ext { C. } \mathrm{CO}_{2} \ ext { B. } \mathrm{O}_{2} & ext { D. } \mathrm{H}_{2} \mathrm{O}\end{array} $$ 18. How many moles of carbon dioxide can be produced from the reaction? (2points) $$ \begin{array}{ll} ext { A. } 1.00 \mathrm{~mol} & ext { C. } 150 \mathrm{~mol} \ ext { B. } 1.14 \mathrm{~mol} & ext { D. } 3.41 \mathrm{~mol} \ ext { 19. How much of the excess reactant would be left unused? }(2 ext { points) } \ ext { A. } 18.0 \mathrm{~g} & ext { C. } 5.00 \mathrm{~g}\end{array} $$

Question

16. If the equation is correctly balanced, what are the coefficients? $$ \begin{array}{ll}	ext { A. } 2: 3 ; 2: 5 & 	ext { C. } 1 ; 5 ; 3 ; 4 \ 	ext { B. } 2 ; 5 ; 1: 4 & 	ext { D. } 3 ; 5 ; 4 ; 10\end{array} $$ 17. If 50.0 g of $$ \mathrm{C}_{3} \mathrm{H}_{8} $$ is allowed to react with 200 g of $$ \mathrm{O}_{2} $$, which is the limiting reagent? (2points) $$ \begin{array}{ll}	ext { A. } \mathrm{C}_{3} \mathrm{H}_{8} & 	ext { C. } \mathrm{CO}_{2} \ 	ext { B. } \mathrm{O}_{2} & 	ext { D. } \mathrm{H}_{2} \mathrm{O}\end{array} $$ 18. How many moles of carbon dioxide can be produced from the reaction? (2points) $$ \begin{array}{ll}	ext { A. } 1.00 \mathrm{~mol} & 	ext { C. } 150 \mathrm{~mol} \ 	ext { B. } 1.14 \mathrm{~mol} & 	ext { D. } 3.41 \mathrm{~mol} \ 	ext { 19. How much of the excess reactant would be left unused? }(2 	ext { points) } \ 	ext { A. } 18.0 \mathrm{~g} & 	ext { C. } 5.00 \mathrm{~g}\end{array} $$

UpStudy AI · Accepted Answer

Sure, let's address each question step-by-step based on the provided information.

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### **Question 16**
**If the equation is correctly balanced, what are the coefficients?**

Since the chemical equation isn't explicitly provided, we'll assume it's the combustion of propane ($$ \mathrm{C}_3\mathrm{H}_8 $$) with oxygen ($$ \mathrm{O}_2 $$):

$$
\mathrm{C}_3\mathrm{H}_8 + 5 \mathrm{O}_2 \rightarrow 3 \mathrm{CO}_2 + 4 \mathrm{H}_2\mathrm{O}
$$

**Balanced Coefficients:**
- $$ \mathrm{C}_3\mathrm{H}_8 $$: 1
- $$ \mathrm{O}_2 $$: 5
- $$ \mathrm{CO}_2 $$: 3
- $$ \mathrm{H}_2\mathrm{O} $$: 4

**Answer:**  
**C. 1 ; 5 ; 3 ; 4**

---

### **Question 17**
**If 50.0 g of $$ \mathrm{C}_3\mathrm{H}_8 $$ is allowed to react with 200 g of $$ \mathrm{O}_2 $$, which is the limiting reagent?**

**Calculations:**
1. **Molar Masses:**
   - $$ \mathrm{C}_3\mathrm{H}_8 $$: $$ 3 \times 12 + 8 \times 1 = 44 $$ g/mol
   - $$ \mathrm{O}_2 $$: $$ 32 $$ g/mol

2. **Moles Available:**
   - $$ \mathrm{C}_3\mathrm{H}_8 $$: $$ \frac{50.0 \text{ g}}{44 \text{ g/mol}} \approx 1.136 $$ mol
   - $$ \mathrm{O}_2 $$: $$ \frac{200 \text{ g}}{32 \text{ g/mol}} = 6.25 $$ mol

3. **Stoichiometry:**
   - From the balanced equation, $$ 1 $$ mol $$ \mathrm{C}_3\mathrm{H}_8 $$ requires $$ 5 $$ mol $$ \mathrm{O}_2 $$.
   - Required $$ \mathrm{O}_2 $$ for $$ 1.136 $$ mol $$ \mathrm{C}_3\mathrm{H}_8 $$: $$ 1.136 \times 5 = 5.68 $$ mol

4. **Comparison:**
   - Available $$ \mathrm{O}_2 $$ (6.25 mol) > Required $$ \mathrm{O}_2 $$ (5.68 mol)
   - Thus, $$ \mathrm{C}_3\mathrm{H}_8 $$ is the **limiting reagent**.

**Answer:**  
**A. $$ \mathrm{C}_3\mathrm{H}_8 $$**

---

### **Question 18**
**How many moles of carbon dioxide can be produced from the reaction?**

**Calculations:**
- From the balanced equation, $$ 1 $$ mol $$ \mathrm{C}_3\mathrm{H}_8 $$ produces $$ 3 $$ mol $$ \mathrm{CO}_2 $$.
- Moles of $$ \mathrm{C}_3\mathrm{H}_8 $$ available: $$ 1.136 $$ mol
- Thus, moles of $$ \mathrm{CO}_2 $$: $$ 1.136 \times 3 \approx 3.41 $$ mol

**Answer:**  
**D. 3.41 mol**

---

### **Question 19**
**How much of the excess reactant would be left unused?**

**Calculations:**
1. **Excess Reactant:** $$ \mathrm{O}_2 $$
2. **Used $$ \mathrm{O}_2 $$:** $$ 5.68 $$ mol (from Question 17)
3. **Available $$ \mathrm{O}_2 $$:** $$ 6.25 $$ mol
4. **Excess $$ \mathrm{O}_2 $$:** $$ 6.25 - 5.68 = 0.57 $$ mol
5. **Mass of Excess $$ \mathrm{O}_2 $$:** $$ 0.57 \times 32 = 18.24 $$ g

**Closest Option:**  
**A. 18.0 g**

---

### **Summary of Answers:**
- **16.** C  
- **17.** A  
- **18.** D  
- **19.** A
**Answers:** - **16.** C - **17.** A - **18.** D - **19.** A

If the equation is correctly balanced, what are the coefficients?

If 50.0 g of is allowed to react with 200 g of , which is the limiting reagent? (2points)

How many moles of carbon dioxide can be produced from the reaction? (2points)

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Question 16

Question 17

Question 18

Question 19

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If the equation is correctly balanced, what are the coefficients? If 50.0 g of is allowed to react with 200 g of , which is the limiting reagent? (2points) How many moles of carbon dioxide can be produced from the reaction? (2points)