Consider the balanced chemical reaction below. How many grams of carbon monoxide are required to react with 6.4 g of iron(III) oxide? Fe:O:(s) + 3 CO(g) 2 Fe(s) + 3 CO:(g) 2 NEXT Based on your knowledge of stoichiometry, set up the table below to determine the minimum number of moles of CO required to react with the Fe2Os and then determine the amounts after the reaction goes to completion. Fe:O:(s) 3 CO(g) 2 Fe(s) 3 CO:(g) Before (mol) Change (mol) After (mol) 5 RESET 6.4 -6.4 3.2 -3.2 0.020 -0.020 0.040 -0.040 0.060 -0.060 0.080 -0.080 0.12 -0.12 0.089 -0.089 0.27 -0.27

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### Stoichiometry and the Balanced Chemical Reaction

**Problem Statement:**
Consider the balanced chemical reaction presented below. The task is to determine how many grams of carbon monoxide (CO) are required to react completely with 6.4 grams of iron(III) oxide (Fe₂O₃).

The reaction is:
\[ \text{Fe}_2\text{O}_3(s) + 3 \text{CO}(g) \rightarrow 2 \text{Fe}(s) + 3 \text{CO}_2(g) \]

**Interactive Activity:**
Based on your understanding of stoichiometry, complete the table below to ascertain the minimum moles of CO required to react with Fe₂O₃, followed by the determination of the amounts after the reaction goes to completion.

**Reactant and Product Table:** 

\[
\begin{array}{|c|c|c|c|c|}
\hline
 & \text{Fe}_2\text{O}_3(s) & + & 3 \text{CO}(g) & \rightarrow  & 2 \text{Fe}(s)  & + & 3 \text{CO}_2(g) \\
\hline
\text{Before (mol)} & \text{} & & \text{} & & \text{} & & \text{} \\
\hline
\text{Change (mol)} & \text{} & & \text{} & & \text{} & & \text{} \\
\hline
\text{After (mol)} & \text{} & & \text{} & & \text{} & & \text{} \\
\hline
\end{array}
\]

**Values Provided for Calculations:**

- \(\text{0}\)
- \(\text{6.4}\)
- \(\text{-6.4}\)
- \(\text{3.2}\)
- \(\text{-3.2}\)
- \(\text{0.020}\)
- \(\text{-0.020}\)
- \(\text{0.040}\)
- \(\text{-0.040}\)
- \(\text{0.060}\)
- \(\text{0.080}\)
- \(\text{-0.080}\)
- \(\text{0.089}\)
- \(\text{-0
Transcribed Image Text:### Stoichiometry and the Balanced Chemical Reaction **Problem Statement:** Consider the balanced chemical reaction presented below. The task is to determine how many grams of carbon monoxide (CO) are required to react completely with 6.4 grams of iron(III) oxide (Fe₂O₃). The reaction is: \[ \text{Fe}_2\text{O}_3(s) + 3 \text{CO}(g) \rightarrow 2 \text{Fe}(s) + 3 \text{CO}_2(g) \] **Interactive Activity:** Based on your understanding of stoichiometry, complete the table below to ascertain the minimum moles of CO required to react with Fe₂O₃, followed by the determination of the amounts after the reaction goes to completion. **Reactant and Product Table:** \[ \begin{array}{|c|c|c|c|c|} \hline & \text{Fe}_2\text{O}_3(s) & + & 3 \text{CO}(g) & \rightarrow & 2 \text{Fe}(s) & + & 3 \text{CO}_2(g) \\ \hline \text{Before (mol)} & \text{} & & \text{} & & \text{} & & \text{} \\ \hline \text{Change (mol)} & \text{} & & \text{} & & \text{} & & \text{} \\ \hline \text{After (mol)} & \text{} & & \text{} & & \text{} & & \text{} \\ \hline \end{array} \] **Values Provided for Calculations:** - \(\text{0}\) - \(\text{6.4}\) - \(\text{-6.4}\) - \(\text{3.2}\) - \(\text{-3.2}\) - \(\text{0.020}\) - \(\text{-0.020}\) - \(\text{0.040}\) - \(\text{-0.040}\) - \(\text{0.060}\) - \(\text{0.080}\) - \(\text{-0.080}\) - \(\text{0.089}\) - \(\text{-0
**Chemical Reaction and Stoichiometry Analysis**

Consider the balanced chemical reaction below. How many grams of carbon monoxide are required to react with 6.4 g of iron(III) oxide?

\[ \text{Fe}_2\text{O}_3(\text{s}) + 3 \text{CO}(\text{g}) \rightarrow 2 \text{Fe}(\text{s}) + 3 \text{CO}_2(\text{g}) \]

Based on the setup of your table from the previous step, determine the grams of carbon monoxide required.

\[ \text{mass}_{\text{CO}} = \_\_\_\_\_\_ \text{g} \]

**Options for Mass of CO:**
- 0 g
- 6.4 g
- 3.2 g
- 19 g
- 0.56 g
- 1.1 g
- 1.7 g
- 2.2 g
- 3.4 g
- 7.6 g

Make sure to follow stoichiometric principles and molar mass calculations to determine the correct mass of carbon monoxide required. Use the balanced equation to establish the mole ratio between iron(III) oxide and carbon monoxide. Then, apply the molar masses of the substances involved to find the mass in grams.

If an error occurs or a reset is needed, you can use the reset button: 
\[ \text{RESET} \]

This exercise helps in understanding stoichiometry and its application in chemical reactions, crucial for mastering concepts in chemistry.
Transcribed Image Text:**Chemical Reaction and Stoichiometry Analysis** Consider the balanced chemical reaction below. How many grams of carbon monoxide are required to react with 6.4 g of iron(III) oxide? \[ \text{Fe}_2\text{O}_3(\text{s}) + 3 \text{CO}(\text{g}) \rightarrow 2 \text{Fe}(\text{s}) + 3 \text{CO}_2(\text{g}) \] Based on the setup of your table from the previous step, determine the grams of carbon monoxide required. \[ \text{mass}_{\text{CO}} = \_\_\_\_\_\_ \text{g} \] **Options for Mass of CO:** - 0 g - 6.4 g - 3.2 g - 19 g - 0.56 g - 1.1 g - 1.7 g - 2.2 g - 3.4 g - 7.6 g Make sure to follow stoichiometric principles and molar mass calculations to determine the correct mass of carbon monoxide required. Use the balanced equation to establish the mole ratio between iron(III) oxide and carbon monoxide. Then, apply the molar masses of the substances involved to find the mass in grams. If an error occurs or a reset is needed, you can use the reset button: \[ \text{RESET} \] This exercise helps in understanding stoichiometry and its application in chemical reactions, crucial for mastering concepts in chemistry.
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