Using the information given to you, fill out the rest of the table below:  Weight of Copper: 1.099 g Volume of Added Nitric Acid: 5.1 mL Total weight of Added Sodium Carbonate: 3.966 g  Weight of Watch Glass and Filter Paper: 48.791 g Weight of Watch Glass, Filter Paper and CuCl precipitate: 51.540 g  Experimental Yield of CuCl: ? Theoretical Yield of CuCl: ?  Percent Yield of CuCl: ? To help find the answers, use  reactions below out,  these reactions are in numerical order. Theoretical yield is based on amount of copper added in the first reaction: 1) Cu (s) + 4HNO3 (aq) -> Cu(NO3)2 (aq) +2NO2 (g) + 2H2O (l)   2) 2HNO3 (aq) + Na2CO3(s) -> H2O (l) + CO2 (g) + 2NaNO3 (aq)  3) Cu(NO3)2 (aq) +Na2(CO3) (s) -> CuCo3 (s) + 2NaNO3 (aq) 4) CuCO3 (s) + 2HCl (aq) -> CuCl2 (aq) + H2O (l) + CO2 (g)  5) CuCl2 (aq) + Cu (s) -> 2CuCl (s) ******************************************************************************* After completing the table, answer the followng question (multiple parts): A) Based on the amounts of copper metal and nitric acid you used in the first reaction, calculate the number of moles of HNO3 that are in excess. Concentrated Nitric Acid has a concentration of 15.8 M. B) Using the moles of HNO3 you calculated and the moles of Cu(NO3)2 produced from the first reaction, calculate the total mass of sodium carbonate needed for the second and third reactions. Did you add enough sodium carbonate in the experiment? C) What observations suggest that copper was added in excess during the last reaction? D) Why might a student obtain a percent yield more than a 100% for this preparation (excluding human error)? E) Copper metal reacts with dilute (1O M) nitric acid by the following reaction: 3 Cu(s) +8NO3 (aq) -> 3CU(NO3)2 (aq) + 2NO (g) + 4H20 (l) If this reaction took place rather than the first reaction, would your yield of CuCl be affected assuming you started with the same amount of copper metal? Explain. F) Could we use HCl to dissolve the copper metal instead of nitirc acid in the first reaction? Explain. G) Given the following three sequential reactions: 1) N2(g) + 3H2 (g)-> 2NH3 (g)  2) 4NH3(g) + 5O2(g) -> 4NO (g) + 6H2O (g) 3) 2NO (g) + O2 (g) -> 2NO2 (g) What mass of hydrogen gas is needed to produce 108.0 kg of nitrogen dioxide?

Using the information given to you, fill out the rest of the table below:

 Weight of Copper: 1.099 g

Volume of Added Nitric Acid: 5.1 mL

Total weight of Added Sodium Carbonate: 3.966 g 

Weight of Watch Glass and Filter Paper: 48.791 g

Weight of Watch Glass, Filter Paper and CuCl precipitate: 51.540 g 

Experimental Yield of CuCl: ?

Theoretical Yield of CuCl: ? 

Percent Yield of CuCl: ?

To help find the answers, use  reactions below out,  these reactions are in numerical order. Theoretical yield is based on amount of copper added in the first reaction:

1) Cu (s) + 4HNO₃ (aq) -> Cu(NO₃)₂ (aq) +2NO₂ (g) + 2H₂O (l)  

2) 2HNO₃ (aq) + Na₂CO₃(s) -> H₂O (l) + CO₂ (g) + 2NaNO₃ (aq) 

3) Cu(NO₃)₂ (aq) +Na₂(CO₃) (s) -> CuCo₃ (s) + 2NaNO₃ (aq)

4) CuCO₃ (s) + 2HCl (aq) -> CuCl₂ (aq) + H₂O (l) + CO₂ (g) 

5) CuCl₂ (aq) + Cu (s) -> 2CuCl (s)

*******************************************************************************

After completing the table, answer the followng question (multiple parts):

A) Based on the amounts of copper metal and nitric acid you used in the first reaction, calculate the number of moles of HNO₃ that are in excess. Concentrated Nitric Acid has a concentration of 15.8 M.

B) Using the moles of HNO₃ you calculated and the moles of Cu(NO₃)₂ produced from the first reaction, calculate the total mass of sodium carbonate needed for the second and third reactions. Did you add enough sodium carbonate in the experiment?

C) What observations suggest that copper was added in excess during the last reaction?

D) Why might a student obtain a percent yield more than a 100% for this preparation (excluding human error)?

E) Copper metal reacts with dilute (1O M) nitric acid by the following reaction:

3 Cu(s) +8NO₃ (aq) -> 3CU(NO₃)₂ (aq) + 2NO (g) + 4H₂0 (l)

If this reaction took place rather than the first reaction, would your yield of CuCl be affected assuming you started with the same amount of copper metal? Explain.

F) Could we use HCl to dissolve the copper metal instead of nitirc acid in the first reaction? Explain.

G) Given the following three sequential reactions:

1) N₂(g) + 3H₂ (g)-> 2NH₃ (g) 
2) 4NH₃(g) + 5O₂(g) -> 4NO (g) + 6H₂O (g)
3) 2NO (g) + O₂ (g) -> 2NO₂ (g)

What mass of hydrogen gas is needed to produce 108.0 kg of nitrogen dioxide?