Consider the equation for the combustion of propane, \( \mathrm{C}_{3} \mathrm{H}_{8} \) \( \mathrm{C}_{3} \mathrm{H}_{8}+\mathrm{O}_{2} \rightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} \) 16. If the equation is correctly balanced, what are the coefficients? \( \begin{array}{ll}\text { A. } 2 ; 3 ; 2 ; 5 & \text { C. } 1 ; 5 ; 3 ; 4 \\ \text { B. } 2 ; 5 ; 1 ; 4 & \text { D. } 3 ; 5 ; 4: 10\end{array} \) 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) \( \begin{array}{ll}\text { A. } \mathrm{C}_{3} \mathrm{H}_{8} & \text { C. } \mathrm{CO}_{2} \\ \text { B. } \mathrm{O}_{2} & \text { D. } \mathrm{H}_{2} \mathrm{O}\end{array} \) \( \begin{array}{ll}\text { 18. How many moles of carbon dioxide can be produced from the reaction? (2points) } \\ \begin{array}{ll}\text { A. } 1.00 \text { mol } & \text { C. } 150 \text { mol } \\ \text { 19. } 1.14 \text { mol } & \text { D. } 3.41 \text { mol } \\ \text { A. } 18.0 \mathrm{~g} & \text { C. } 5.00 \mathrm{~g}\end{array} \\ \text { B. } 109 \mathrm{~g} & \text { D. } 60.0 \mathrm{~g}\end{array} \)

Sure, let's address each question step-by-step: --- ### **Question 16** **Balance the combustion equation of propane (\( \mathrm{C}_3\mathrm{H}_8 \)):** \[ \mathrm{C}_3\mathrm{H}_8 + \mathrm{O}_2 \rightarrow \mathrm{CO}_2 + \mathrm{H}_2\mathrm{O} \] **Balanced Equation:** \[ \mathrm{C}_3\mathrm{H}_8 + 5\,\mathrm{O}_2 \rightarrow 3\,\mathrm{CO}_2 + 4\,\mathrm{H}_2\mathrm{O} \] **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** **Determine the limiting reagent when 50.0 g of \( \mathrm{C}_3\mathrm{H}_8 \) reacts with 200 g of \( \mathrm{O}_2 \).** 1. **Calculate moles of each reactant:** - **Propane (\( \mathrm{C}_3\mathrm{H}_8 \)):** \[ \text{Molar Mass} = 3(12.01) + 8(1.008) = 44.11\,\mathrm{g/mol} \] \[ \text{Moles} = \frac{50.0\,\mathrm{g}}{44.11\,\mathrm{g/mol}} \approx 1.135\,\mathrm{mol} \] - **Oxygen (\( \mathrm{O}_2 \)):** \[ \text{Molar Mass} = 32.00\,\mathrm{g/mol} \] \[ \text{Moles} = \frac{200\,\mathrm{g}}{32.00\,\mathrm{g/mol}} = 6.25\,\mathrm{mol} \] 2. **Stoichiometry from the balanced equation:** \[ 1\,\mathrm{mol}\,\mathrm{C}_3\mathrm{H}_8 \text{ requires } 5\,\mathrm{mol}\,\mathrm{O}_2 \] \[ 1.135\,\mathrm{mol}\,\mathrm{C}_3\mathrm{H}_8 \text{ requires } 1.135 \times 5 = 5.675\,\mathrm{mol}\,\mathrm{O}_2 \] 3. **Compare available vs. required:** \[ 6.25\,\mathrm{mol}\,\mathrm{O}_2 > 5.675\,\mathrm{mol}\,\mathrm{O}_2 \] \[ \text{Thus, } \mathrm{C}_3\mathrm{H}_8 \text{ is the limiting reagent.} \] **Answer:** **A.** \( \mathrm{C}_3\mathrm{H}_8 \) --- ### **Question 18** **Calculate the moles of carbon dioxide (\( \mathrm{CO}_2 \)) produced.** 1. **From the balanced equation:** \[ 1\,\mathrm{mol}\,\mathrm{C}_3\mathrm{H}_8 \rightarrow 3\,\mathrm{mol}\,\mathrm{CO}_2 \] 2. **Using the moles of limiting reagent (\( \mathrm{C}_3\mathrm{H}_8 \)):** \[ 1.135\,\mathrm{mol}\,\mathrm{C}_3\mathrm{H}_8 \times 3 = 3.405\,\mathrm{mol}\,\mathrm{CO}_2 \] \[ \approx 3.41\,\mathrm{mol}\,\mathrm{CO}_2 \] **Answer:** **D.** 3.41 mol --- ### **Question 19** **Calculate the mass of carbon dioxide (\( \mathrm{CO}_2 \)) produced.** 1. **Moles of \( \mathrm{CO}_2 \) produced:** \( 3.41\,\mathrm{mol} \) (from Question 18) 2. **Calculate mass:** \[ \text{Molar Mass of } \mathrm{CO}_2 = 12.01 + 2(16.00) = 44.01\,\mathrm{g/mol} \] \[ \text{Mass} = 3.41\,\mathrm{mol} \times 44.01\,\mathrm{g/mol} \approx 150\,\mathrm{g} \] **Note:** The provided options for this question seem to be mismatched with the calculation. Based on the stoichiometry, the mass of \( \mathrm{CO}_2 \) should be approximately **150 g**. **Answer:** Assuming correct options, the mass of \( \mathrm{CO}_2 \) produced is approximately **150.0 g**. --- If there was a formatting issue with Question 19's options, please verify and provide the correct choices to ensure an accurate answer.