Mass of vial with AgNO3 12.61g Mass of vial 13.94g Mass of copper wire 3.24g Mas

Question

Mass of vial with AgNO3 12.61g Mass of vial 13.94g Mass of copper wire 3.24g Mass of copper wire (after reaction) 3.03g Mass of beaker 48.04g Mass of beaker with silver produced 49.69g

Calculations (Please show all numbers and set-ups for each calculation) 1. Mass of Copper Wire Put Into the Reaction (Not a calculation, just an important value)2. Moles of Cu Put Into the Reaction3. Mass of AgNO3 Put Into the Reaction4. Moles of AgNO3 Put Into the Reaction5. Determine the limiting reactant. 6. Mass of Cu Wire Reacted7. Moles of Cu Reacted 8. Mass of Ag Produced9. Moles of Ag Produced 10. Ratio of moles of Ag Produced to moles of AgNO3 Reacted (round off to the nearest whole number)11. Ratio of moles of Ag Produced to moles of Cu Reacted (round off to the nearest whole number)

Explanation / Answer

Cu + 2AgNO3 ---> Cu(NO3)2 + 2Ag

1. Mass of Cu in the reaction = 3.24 g

2. moles of Cu = 3.24/63.546 = 0.051 mols

3. mass AgNO3 in reaction = 13.94 - 12.61 = 1.33 g

4. moles AgNO3 = 1.33/169.87 = 0.008 mols

5. limiting reactant = AgNO3

6. Mass of Cu reacted = 3.24 - 3.03 = 0.21 g

7. moles of Cu reacted = 0.21/63.546 = 0.0033 mols

8. mass of Ag produced = 2 x 0.0033 x 108 = 0.713 g

9. moles of Ag produced = 2 x 0.0033 = 0.0066 mols

10. ratio (moles Ag produced/moles of AgNO3) = 0.0066/0.008 = 0.825

11. ratio (moles Ag/moles Cu) = 0.0066/0.0033 = 2

Related Questions

Navigate

• Browse (All)
• Browse M
• Subjects