1) 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. noitanen garwollol odi yd bios bin (M 01) sulthy O.HP OMSOPOR blov wo blow noites tent TON apoy melqxdl Slom de to upora 2) 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?

The two questions on the second photo are based on the table? How do I do them?

? H₂O, HCI, benzene ONa О 1. HCI, 2. 1. BH3, 2. H2O2, aq NaOH; 3. 1. H3O+; 2. CI ONa

A Show Time Remaining A You are asked to prepare 850 mL of a 0.15 M HNO, solution using a 2.5 M stock solution of HNO3. What volume of the 2.5 M solution of HNO3 should you take? How much water should be added? Filling blanks in the diagram can be helpful. water OA 440 mL of the HNO, stock solution and 410 mL of water O B. 51 mL of the HNO3 stock solution and 799 ml of water Oc 320 mL of the HNO, stock solution and 530 mL of water OD 850 mL of the HNO, stock solution and 1000 ml of water OE 150 mL of the HNO3 stock solution and 700 ml of water

2. Calculate the number of moles and mass (in grams) of C,H, required to react with water to produce 9.55 g C,H,0. CH, + H20 ---> C,H,0