Balanced equation for reaction between Cute and HNO3
3 Cu(s) + 8 HNO3 ----> 3 Cu(NO3)2 (aq) + 2 NO (g) + 4 H2O(l)
3 eq of Cu reacts with 8 eq of HNO3
Moles of HNO3 = 3.5 mL *( 6 mol/ 1000 mL) => 0.021 mol
Molar mass of Cu = 63.54 g/mol
So 0.41 g / 63.54 g/mol => 0.00645 moles
For complete reaction of 0.00645 moles of Cu metal, we need 0.00645 mol * (8/3) = 0.017 mol of HNO3
but we have 0.021 moles of HNO3
Therefore Cu is the limiting reactant
limiting reagent ml Cu 2. In reaction (G), suppose that you add 3.5 ml of 6...
2. In reaction (i), suppose you add 4.0 mL of 6 M nitric acid to a sphere of copper metal that weighs 0.65 grams. Which reactant is the limiting reagent? (Show your work) We were unable to transcribe this image
1. Balance the three copper reactions: + H20 (1) Cu(NO3)2 (aq) + NO2(g) i) Cu (s) + HNO3 (aq) ii) Cu(NO3)2 (aq) + NaOH(aq) Cu(OH)2 (s) + NaNO3(aq) (aq) - iii) Cu(OH)2 (S) Cuo(s) + H2O (1) 2. In reaction (i), suppose you add 4.0 mL of 6 M nitric acid to a sphere of copper metal that weighs 0.65 grams. Which reactant is the limiting reagent? (Show your work)
1. Balance the three copper reactions: +H20 (1) +NO2 (g) Cu(NO3)2 (aq) i) Cu (s) HNO3 (aq) NANO3 (aq) NaOH (aq) Cu(OH)2 (s) + ii) Cu(NOs)2 (aq) + H2O (1I) CuO (s) iii) Cu(OH)2 (s) 2. In reaction (i), suppose you add 4.0 mL of 6M nitric acid to a sphere of copper metal that weighs 0.65 grams. Which reactant is the limiting reagent? (Show your work)
3. a. Why should the Cu(OH)2 precipitate that is formed during reaction (ii) be heated slowly during reaction (ii)? b. Why does reaction (i) have to be carried out in the fume hood? 4. Reaction (iii) is considered to be c) decomposition d) acid-base e) precipitation b) single displacement a) combination EXPERIMENT 9 REACTION OF COPPER AND ITS COMPOUNDS PRE-LABORATORY QUESTIONS The following preparatory questions should be answered before coming to lab. They are intended to introduce you to several...
REACTION OF COPPER AND ITS COMPOUNDS PRE-LABORATORY QUESTIONS The following preparatory questions should be answered before coming to lab. They are intended to introduce you to several ideas that are important to aspects of the experiment. You must turn in your work to your instructor before you will be allowed to begin the experiment. 1. Balance the three copper reactions: Cu(NO3)2 (aq) + NO2(g) + H2O (1) i) Cu (s) + HNO3(aq) ii) Cu(NO3)2 (aq) + NaOH(aq) Cu(OH)2 (s) +...
The following preparatory questions should be answered before coming to lab. They are intended to introduce you to several ideas that are important to aspects of the experiment. You must turn in your work to your instructor before you will be i allowed to begin the experiment. 1. Balance the three copper reactions: 1) Cu(s) + HNO3(aq) ii) Cu(NO3)2 (aq) + 2NaOH(aq) - iii) Cu(OH)2 (3) Cu(NO3)2 (aq) +NO2(g) + H2O (1) Cu(OH)2 (8) + NaNO (aq) CuO (s) +...
) Calculate the volume (in mL) of nitric acid that you plan to use in Reaction 1 in the procedure. Cu(s) + 4HNO3(aq) -----> Cu(NO3)2 (aq) + 2NO2(g) + 2H2O (l) 2) Calculate the amount of zinc granules (in grams) that must be added in reaction 5 in part 1 of the procedure CuSO4 (aq) + Zn (s) ------> ZnSO4 (aq) + Cu (s) Additional Information from procedure 1) . Weigh out approximately 0.50 g (starting material) of copper wire...
please help!! 2. When zinc metal reacts with copper(II) nitrate, zinc(II) nitrate and copper metal are the products. How many grams of zinc metal are required to react completely with 725 mL of 0.1955 M copper (II) nitrate solution? What mass of copper metal is produced? You will need a balanced equation to solve this problem! 3. One step in the process of manufacturing nitric acid (HNO3), a staple industrial chemical, is 3 NO2 (g) + H20 (1) ► 2HNO3...
You carry out the reaction as described in the lab, using 6.00 g of copper, 38.8 mL of 3.0 M H2SO4, and 16.6 mL of 16 M HNO3. What is the limiting reagent in this reaction? What is the theoretical yield of CuSO4·5H2O in grams? Cu(s) + 2 HNO3(aq) + H2SO4(aq) + 3 H2O(l) → CuSO4∙5H2O(s) + 2 NO2(g)
Balance the equation for the reaction observed: _ Cu(s) + HNO3(aq) → Cu(NO3)2(aq) +_ NO2(g) + H2O(1) 3. Add 40 mL of 3.0 M NaOH (sodium hydroxide) to the solution in your beaker. Write the balanced equation for the reaction observed: 4. Add 2-3 boiling chips to your beaker and carefully heat the solution, while stirring with a stirring rod, just to the boiling point. (Do NOT boil. Have a low flame and keep the beaker well above the flame.)...