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CHE 105 Intro to Chemistry Lab: Mole to Mole Short Answer Mole to Mole Relationship between Cu and Ag Lab Results Data Analysis 1)

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CHE 105 Intro to Chemistry

Lab: Mole to Mole

Short Answer

Mole to Mole Relationship between Cu and Ag

Lab Results

Data Analysis

1).How many moles of silver nitrate were added to the reaction?

  Conclusions

2.Did all the silver ions get consumed in the reaction? The molar mass of silver is 107.87 g/mol. Justify your answer.

 

 

 

3. Write a balanced equation for the reaction of AgNO₃(aq) with Zn(s) to produce Ag(s) and Zn(NO₃)₂(aq) using the data from the table below.

Substance	Amount
AgNO3	0.30 moles
Zn	0.15 moles
Ag	0.30 moles
Zn(NO3)2	moles

 

 

 

4. What is the mole to mole ratio between aluminum and silver in the balanced equation below?
   
   Al(s) + 3AgNo3(aq) à 3Ag(s) + Al(No3)3(aq)

 

 

Mole to Mole Relationship between Cu and Ag

 

1. What was the mass of the empty beaker?
   1. 185.000 g
   2. 50.250 g
   3. 390.840 g
   4. 388.450 g
2. What was the mass of the beaker together with the silver nitrate?
   1. 50.250 g
   2. 185.000 g
   3. 388.450 g
   4. 390.233 g
3. What was the mass of the copper used in the reaction?
   1. 1.000 g
   2. 185.000 g
   3. 5.000 g
   4. 391.450 g
4. What happened to the color of the solution after the addition of copper?
   1. The color of the solution remained unchanged.
   2. The solution turned red.
   3. The solution turned white.
   4. The solution turned blue.
5. What was the mass of silver produced from the reaction?
   1. 391.843 g
   2. 185.000 g
   3. 3.395 g
   4. 188.395 g
6. How many moles of copper were used in the reaction? The atomic mass of copper is 63.55 g/mol.
   1. 0.03148 mol Cu
   2. 4.335 mol Cu
   3. 6.156 mol Cu
   4. 0.01574 mol Cu
7. How many moles of solid silver were produced in the reaction? The atomic mass of silver is 107.87 g/mol.
   1. 4.335 mol Ag
   2. 0.03147 mol Ag
   3. 0.01624 mol Ag
   4. 3.392 mol Ag
8. Select the reaction equation for the reaction between copper and silver ions that is closest to your experimental values.
   1. 0.016Cu(s) + 0.032Ag⁺(aq) -> Cu²⁺(aq) + Ag(s)
   2. Cu(s) + Ag⁺(aq) -> 0.016Cu²⁺(aq) + 0.032Ag(s)
   3. 0.016Cu(s) + 0.032Ag⁺(aq) -> 0.016Cu²⁺(aq) + 0.032Ag(s)
   4. Cu(s) + 0.016Ag⁺(aq) -> 0.032Cu²⁺(aq) + Ag(s)
9. Select the reaction equation for the reaction between copper and silver ions using the smallest whole number coefficients.
   1. 2Cu(s) + 26Ag⁺(aq) -> 2Cu²⁺(aq) + 2Ag(s)
   2. 2Cu(s) + Ag⁺(aq) -> 2Cu²⁺(aq) + Ag(s)
   3. Cu(s) + 2Ag⁺(aq) -> Cu²⁺(aq) + 2Ag(s)
   4. 5Cu(s) + 2Ag⁺(aq) -> 5Cu²⁺(aq) + 2Ag(s)
10. If the silver in the beaker contained water during your last weighing, how would this affect your results?
    1. The silver would appear to weigh more, leading to an incorrect calculation of the mole ratios in the reaction.
    2. The water would cause silver to weigh less, leading to an incorrect calculation of the mole ratios in the reaction.
    3. The silver would react with the water to form silver hydroxide.
    4. The water would prevent the silver from reacting with the copper.
11. What is the purpose of weighing the empty beaker?
    1. The weight of the empty beaker can be used as a positive control.
    2. The weight of the empty beaker can be subtracted out after the reaction is complete to determine the mass of the products of the reaction.
    3. The weight of the empty beaker can be used to calculate the amount of reactants that can be added for the experiment.
    4. The weight of the empty beaker is not essential to the calculations in this experiment.
12. What is the mole to mole relationship between the copper and silver respectively?
    1. 2:10
    2. 1:1
    3. 2:1
    4. 1:2
13. How many grams of copper would you need to add if you wanted to produce 8.000 grams of silver? The atomic mass of copper is 63.55 g/mol, and the atomic mass of silver is 107.87 g/mol.
    1. 12.357 g of copper
    2. 2.357 g of copper
    3. 4.000 g of copper
    4. 4.713 g of copper
14. Suppose that magnesium would react exactly the same as copper in this experiment. How many grams of magnesium would have been used in the reaction if 1.000 g of silver were produced? The atomic mass of magnesium is 24.31 g/mol, and the atomic mass of silver is 107.87 g/mol.
    1.  0.2254 g
    2. 2.563 g
    3. 2.000 g
    4. 0.1127 g
15. What is the source of the blue color of the solution after the reaction?
    1. aqueous silver ions (Ag⁺)
    2. aqueous copper ions (Cu²⁺)
    3. the silver nitrate solution (AgNO₃)
    4. the solid copper (Cu)
16. For the following reaction Cu²⁺(aq) + Zn(s) -> Cu(s) + Zn²⁺(aq), what is the mole to mole relationship between copper and zinc?
    1. It is a 2:1 relationship.
    2. It is a 1:1 relationship.
    3. The relationship cannot be determined from the equation.
    4. It is a 1:2 relationship.
17. What happens to the solid copper and the aqueous silver from the silver nitrate solution during the course of the reaction?
    1. The copper changed from a solid, metallic, unreacted state to an aqueous ion form. The metallic silver from the silver nitrate solution became aqueous ions.
    2. The copper changed from an aqueous ion form to a solid, metallic state. The aqueous silver ions from the silver nitrate solution became solid, metallic silver.
    3. The copper changed from an aqueous ion form to a solid, metallic state. The metallic silver from the silver nitrate solution became aqueous ions.
    4. The copper changed from a solid, metallic, unreacted state to an aqueous ion form. The aqueous silver ions from the silver nitrate solution became solid, metallic silver.
18. Symbols such as (s) or (aq) written in parentheses next to an atom, ion, or a compound indicate
    1. the solubility of the atom, ion, or compound.
    2. the molarity of the atom, ion, or compound.
    3. the physical state of the atom, ion, or compound.
    4. the charge of the atom, ion, or compound.
19. What does the symbol (s) represent when it is next to an atom?
    1. The atom is in the solid state.
    2. The atom is selenium.
    3. The atom is a charged salt.
    4. The atom is in the liquid state.
20. What does the symbol (aq) represent when it is next to an atom?
    1. The atom is in the gaseous state in solution.
    2. The atom is in the liquid state in solution.
    3. The atom is in the solid state, which means it is not aqueous.
    4. The atom is in the aqueous state, which means it is in solution.
21. Select the balanced equation for the reaction of HCl(aq) with Mg(s) to produce H₂(g) and MgCl₂(aq) using the data from the table.
    1. 2Mg(s) + 2HCl(aq) -> MgCl₂(aq) + H₂(g)
    2. Mg(s) + 2HCl(aq) -> MgCl₂(aq) + 2H₂(g)
    3. Mg(s) + 2HCl(aq) -> MgCl₂(aq) + H₂(g)
    4. 2Mg(s) + HCl(aq) -> 2MgCl₂(aq) + H₂(g)