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.

---

### **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)

Solución de inteligencia artificial de Upstudy

Responder

Solución

Mind Expander

preguntas relacionadas

Latest Chemistry Questions

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)