1. **Problem:** Consider the combustion of carbon monoxide in oxygen gas: $$2 \text{ CO}(g) + \text{O}_2(g) \to 2 \text{ CO}_2(g)$$ a. If you start with 6.04 moles of CO, how many moles of CO2 can you make? 2. **Formula and Rules:** The balanced chemical equation shows the mole ratio between CO and CO2 is 2:2 or 1:1. 3. **Calculation for part a:** Since 2 moles of CO produce 2 moles of CO2, 6.04 moles of CO will produce the same number of moles of CO2: $$\text{moles CO}_2 = 6.04 \text{ moles CO} \times \frac{2}{2} = 6.04 \text{ moles CO}_2$$ 4. **Answer for part a:** You can make **6.04 moles of CO2**. 5. **Calculation for part b:** From the balanced equation, 2 moles of CO react with 1 mole of O2. So for 6.04 moles of CO: $$\text{moles O}_2 = 6.04 \times \frac{1}{2} = 3.02 \text{ moles O}_2$$ 6. **Answer for part b:** You used **3.02 moles of O2** in the reaction. --- **Summary:** - a. Moles of CO2 produced = 6.04 - b. Moles of O2 used = 3.02 All answers are rounded to two decimal places as requested.