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In lab, you reacted copper metal with aqueous nitric acid to produce aqueous Copper (11) nitrate,...
In lab, you reacted copper metal with aqueous nitric acid to produce aqueous copper (II) nitrate, nitrogen dioxide gas and water. Cu (s) + 4HNO3 (aq) ---- > Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) a) If 0.210 gram of copper is reacted with 35.0 mL of 0.551 mol/L nitric acid, how many molecules and how grams of copper (II) nitrate are produced? b) How many moles of the reagent that is in excess are left over? c) If...
In lab, you reacted copper metal with aqueous nitric acid to produce aqueous copper (II) nitrate, nitrogen dioxide gas and water. Cu (s) + 4HNO3 (aq) ---- > Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) a) If 0.210 gram of copper is reacted with 35.0 mL of 0.551 mol/L nitric acid, how many molecules and how grams of copper (II) nitrate are produced? b) How many moles of the reagent that is in excess are left over? c) If...
Copper reacts with nitric acid to produce copper nitrate, nitrogen dioxide gas, and water. Cu(s) + 4 HNO (aq) Cu(NO ) (aq) + 2 NO (g) + 2 H O(l) If you have 0.60 moles of Cu and the reaction goes to completion, how many moles of HNO are needed to produce 1.2 moles of NO ?
In the reaction of copper with nitric acid if 25 g of copper reacted with 25 ml of 0.5M nitric acid, how much nitrogen dioxide gas would be produced?
5 attempts left Check my work Enter your answer in the provided box. Nitrogen dioxide is used industrially to produce nitric acid, but it contributes to acid rain and photochemical smog. What volume of nitrogen dioxide is formed at 725 torr and 28.2°C by reacting 3.31 cm of copper (d=8.95 g/cm) with 229 mL of nitric acid (d - 1.42 em 68.0% HNO, by mass)? Cu(s) + 4HNO3(aq) + Cu(NO3)2(aq) + 2NO2(8) + 2H20(1) 23.04 10
Calculate the volume of nitrogen dioxide produced at 707.4 torr and 22.0°C by the reaction of 8.45 cm3 copper (density = 8.95 g/cm3) with 202.3 mL of concentrated nitric acid if the acid has a density of 1.42 g/cm3 and contains 68.0% HNO3 by mass). Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)
) 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...
16 Cts with aqueous copper(II) chloride accord- 101. Zinc metal reacts with aqueous copper(1) ing to this equation: Zn (s) + CuCl2 (aq) → ZnCl2 (aq) + Cu (s) In this reaction, what mass of copper metal can be pro- duced from the reaction of 500 mL of 1.20-M aq. cu 2 with excess zinc? 10 103. The concentration of bromide ion may be determined by gravimetric analysis, using this reaction: Ag+ (aq) + Br (aq) → AgBr (s) A...
3. (14%) The metal copper is oxidized in nitric acid according to the equation: 3 Cu + 8 HNO3 → 3 Cu (NO3) 2 + 2 NO + 4 H2O a) Show how you set the oxidation-reduction reaction and get the equation here above (show as many steps in the process) b) You receive 0.3855 g of copper-containing metal together with other dissolved substances easily set up. You find that to dissolve the copper and form copper nitrate Cu (NO3)...
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...