50 mL of a 0.050 M solution of Cu2+ was reduced to solid copper. How many...
50 mL of a 0.050 M solution of Cu2+ was reduced to solid copper. How many coulombs had passed when the Cu2+ was completely reduced to Cu(s)? Use 2 significant figures. Please show all work, thank you!
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50 mL of a 0.050 M solution of Cu2+ was reduced to solid copper.
How many...
A-D A. How many miles of Cu2+ is present in the solution? B. How many miles...
A-D
A. How many miles of Cu2+ is present in the solution?
B. How many miles of electrons are needed to plate all the
Cu2+?
C. Calculate the coulombs of charge, q required to plate all
Cu2+?
D. How many hours will it take to plate out all the
Cu2+?
B. Electrodeposition A solution of 200.0 mL of a o015 M cu r solution was electrolyzed using a current, i, of 0.200 amp? The half reaction is shown below: 2...
The cathode compartment of a copper concentration cell contains 0.500 L of 1.00 M [Cu2+] solution...
The cathode compartment of a copper concentration cell contains 0.500 L of 1.00 M [Cu2+] solution while the anode compartment contains 0.800 L of 0.0500 M [Cu] with a copper electrode in each compartment. How many Coulombs of electric charge can the cell produce before the compartments reach equilibrium at 25°C?
How many moles of copper II ion, Cu2+, are present in 200 mL of a .250...
How many moles of copper II ion, Cu2+, are present in 200 mL of a .250 M solution of CuSO4?
Question 10 Consider the balanced equation representing the reaction of solid copper and aqueous silver nitrate:...
Question 10 Consider the balanced equation representing the reaction of solid copper and aqueous silver nitrate: Cu (s) + 2 AgNO3 → 2 Ag (s) + Cu(NO3)2 What mass of solid copper is required to completely react with 16.6 mL of 0.67 M silver nitrate? Calculate the mass in grams, and report your answer to 2 significant figures.
Consider a 50 mL solution of .55M CaCl2 (aq). a solid piece of NaCl (s) with...
Consider a 50 mL solution of .55M CaCl2 (aq). a solid piece of NaCl (s) with a volumw of 9.5 cm^3 is added to the aqueous calcium chloride solution. Calculate the chloride ion concentration in the mixture after the solid completely dissolves. please show all work
The cathode compartment of a copper concentration cell contains 0.500 L of 1.00 M [Cu2+] solution...
The cathode compartment of a copper concentration cell contains 0.500 L of 1.00 M [Cu2+] solution while the anode compartment contains 0.950 L of 0.0500 M [Cu2"] with a copper electrode in each compartment. How many Coulombs of electric charge can the cell produce before the compartments reach equilibrium at 25°C?
A solution contains 2.2 × 10-3 M in Cu2+ and 0.33 M in LiCN. If the...
A solution contains 2.2 × 10-3 M in Cu2+ and 0.33 M in LiCN. If the Kf for Cu(CN)42- is 1.0 × 1025, how much copper ion remains at equilibrium? Which is the answer: 6.7 × 10-28 M 3.8 × 10-24 M 3.1 x 10-24 M 2.9 × 10-27 M 4.6 × 10-25 M Please show your work, thank you!
How many grams of copper if you a 499.8 mL of a .10 M solution/. (Hint...
How many grams of copper if you a 499.8 mL of a .10 M solution/. (Hint M = mol/L and amu for Cu =63.546 g/mol)
A galvanic cell Cr(s)|Cr2+(aq) || Cu2+(aq)|Cu(s) is constructed using a completely immersed Cr electrode that weighs 35.4 g and a Cu electrode immersed in 462 mL of 1.00 M Cu2+(aq) solution. A steady...
A galvanic cell Cr(s)|Cr2+(aq) || Cu2+(aq)|Cu(s) is constructed using a completely immersed Cr electrode that weighs 35.4 g and a Cu electrode immersed in 462 mL of 1.00 M Cu2+(aq) solution. A steady current of 0.0795 A is drawn from the cell as the electrons move from the Cr electrode to the Cu electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? s...
If we have 50 mL of a 1.0M sodium hydroxide solution and 50 mL of a...
If we have 50 mL of a 1.0M sodium hydroxide solution and 50 mL of a 0.20 M iron (III) nitrate solution, what is the concentration of ions in each solution? Write the chemical, complete ionic and net ionic equations for the reaction. Chemical: Complete lonic: Net Ionic: What volume of 1.0M NaOH is required to precipitate all the Fe ions from 50. mL of a 0.20 M Fe(NO) solution? What mass of iron (II) hydroxide precipitate can be produced...
A-D
A. How many miles of Cu2+ is present in the solution?
B. How many miles of electrons are needed to plate all the
Cu2+?
C. Calculate the coulombs of charge, q required to plate all
Cu2+?
D. How many hours will it take to plate out all the
Cu2+?
B. Electrodeposition A solution of 200.0 mL of a o015 M cu r solution was electrolyzed using a current, i, of 0.200 amp? The half reaction is shown below: 2...
The cathode compartment of a copper concentration cell contains 0.500 L of 1.00 M [Cu2+] solution while the anode compartment contains 0.800 L of 0.0500 M [Cu] with a copper electrode in each compartment. How many Coulombs of electric charge can the cell produce before the compartments reach equilibrium at 25°C?
Question 10 Consider the balanced equation representing the reaction of solid copper and aqueous silver nitrate: Cu (s) + 2 AgNO3 → 2 Ag (s) + Cu(NO3)2 What mass of solid copper is required to completely react with 16.6 mL of 0.67 M silver nitrate? Calculate the mass in grams, and report your answer to 2 significant figures.
The cathode compartment of a copper concentration cell contains 0.500 L of 1.00 M [Cu2+] solution while the anode compartment contains 0.950 L of 0.0500 M [Cu2"] with a copper electrode in each compartment. How many Coulombs of electric charge can the cell produce before the compartments reach equilibrium at 25°C?
If we have 50 mL of a 1.0M sodium hydroxide solution and 50 mL of a 0.20 M iron (III) nitrate solution, what is the concentration of ions in each solution? Write the chemical, complete ionic and net ionic equations for the reaction. Chemical: Complete lonic: Net Ionic: What volume of 1.0M NaOH is required to precipitate all the Fe ions from 50. mL of a 0.20 M Fe(NO) solution? What mass of iron (II) hydroxide precipitate can be produced...
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