1. Mole and Mass Relationships in a Chemical Reaction Calculations and Questions Help

2. Calculation #1 Convert the grams of copper consumed to moles. Convert the grams of copper consumed to moles. Grams Cu moles Cu Grams Cu moles Cu Use the “Mole Triangle” if necessary. Use the “Mole Triangle” if necessary.

3. Calculation #2 Convert the grams of silver produced to moles. Convert the grams of silver produced to moles. Grams Ag moles Ag Grams Ag moles Ag Use the “Mole Triangle” if necessary. Use the “Mole Triangle” if necessary.

4. Calculation #2 Convert the grams of silver produced to moles. Convert the grams of silver produced to moles. Grams Ag moles Ag Grams Ag moles Ag Use the “Mole Triangle” if necessary. Use the “Mole Triangle” if necessary.

5. Question #1 Use the mole values calculated in calculations #1 & #2 to determine the smallest whole number ratio. Use the mole values calculated in calculations #1 & #2 to determine the smallest whole number ratio. Do this by dividing both #’s by the smaller and then round to nearest whole number. Do this by dividing both #’s by the smaller and then round to nearest whole number.

6. Question #2 Use the whole #’s you just calculated to complete the equation in this question. Use the whole #’s you just calculated to complete the equation in this question. Re-write the equation replacing X and Y with the whole numbers. Re-write the equation replacing X and Y with the whole numbers.

7. Question #3 What if your silver was not dry at the end of the experiment? How would this ultimately change the coefficients? What if your silver was not dry at the end of the experiment? How would this ultimately change the coefficients? Still need help… (Next slide) Still need help… (Next slide)

8. Question #3 Try changing the mass of silver produced (more or less depending on what you think) and redo the calculations to see how the coefficients would change. Try changing the mass of silver produced (more or less depending on what you think) and redo the calculations to see how the coefficients would change.

9. Question #4 One of the reactants is in excess. This means that there was more present than needed so it did not all react. There was extra! One of the reactants is in excess. This means that there was more present than needed so it did not all react. There was extra! Some of this reactant would have been left over. Some of this reactant would have been left over.

10. Question #5 In Unit VI we discussed 4 different types of reactions. (See page 2 of those notes) In Unit VI we discussed 4 different types of reactions. (See page 2 of those notes) The answer to this question is one of the 4 types. The equation for the reaction is listed in question 2 of this lab. The answer to this question is one of the 4 types. The equation for the reaction is listed in question 2 of this lab.

11. Question #6 Use factor labeling to convert what you are given to what you need to know. Use factor labeling to convert what you are given to what you need to know. Use the “Mole Triangle” if needed. Use the “Mole Triangle” if needed. Each of these deal with two substances so you will need 2 triangles! Each of these deal with two substances so you will need 2 triangles!

12. Question #7 Use factor labeling to convert what you are given to what you need to know. Use factor labeling to convert what you are given to what you need to know. Use the “Mole Triangle” if needed. Use the “Mole Triangle” if needed. Each of these deal with two substances so you will need 2 triangles! Each of these deal with two substances so you will need 2 triangles! There is a typing error in the equation. It should be: There is a typing error in the equation. It should be: N 2(g) + 3 H 2(g) 2 NH 3(g) N 2(g) + 3 H 2(g) 2 NH 3(g)