Description B. Calculations: Determine the mass of iron consumed in the reaction. Show your work. ...

---

Description B. Calculations: Determine the mass of iron consumed in the reaction. Show your work. (4 pts) Formula: 2.Calculate the number of moles of iron consumed using dimensional analysis and the molar mass of iron as a conversion factor. Show your work. (10 pts) 3. Determine the mass of copper formed. Show your work. (4 pts) Formula: 4. Calculate the number of moles of copper formed using dimensional analysis and the molar mass of copper as a conversion factor. Show your work. (10 pts) 5. What is the experimental mole ratio between the iron and the copper? Determine the simplest whole number ratio of moles of iron consumed (see Question 2), to moles of copper formed (see Question 4). [Note: To find the ratio, you must use your answers to Question 2 and Question 4 and divide both values by whatever value is smaller.] (8 pts) C. Analysis Questions: 6. What color was the 1M CuCl22H20 solution before the nails were placed in it? What ion was responsible for this color? Explain your reasoning with support from the lab. (8 pts) 7. After the nails were allowed to react, did the solution change color? What was responsible for this color change? Explain your reasoning with support from the lab. (8 pts) 8. What type of chemical reaction was this? You need to determine the type of reaction and explain how you know it falls into that category. (8 pts) 9. What was the solid product that formed on the nails? Explain your reasoning with support from the lab. (8 pts) 10. Based on the experimental mole ratio, which of the following equations is MOST LIKELY to be the one represented by this experiment? Justify your answer with support from the lab. (9 pts) 11. Why is knowing the “mole ratio” essential when performing stoichiometric calculations? Your response must include (a) a discussion of balanced equations in the context of the law of conservation of mass (8 pts) and (b) an example different from the one in this lab that shows how a mole ratio is used in a stoichiometric calculation (9 pts).